Classification Of Elements And Periodicity In Properties Questions

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List of classification of elements and periodicity in properties Questions

Question No Questions Class
1 The last element in Newlands’ periodic table was:
A . zinc
B. barium
c. cesium
D. thorium
11
2 In Mendeleev’s periodic table, gaps were left for the elements to be discovered
later. Which of the following elements found a place in the periodic table later?
A. Germanium
B. Chlorine
c. oxygen
D. silicon
11
3 Q5. (a) How does atomic radius vary in group in the periodic table?
(6) Explain
(i) Radius of cation is less than that of the atom.
(ii) Radius of anion is more than that of the atom.
(iii) In iso-electronic ion, the ionic radii decreases with increase in atomic number.
11
4 Among the following groupings, which represents the collection of isoelectronic species?
A ( cdot C O, N O^{+}, C N^{-}, C_{2}^{2} )
B. ( N_{2}, C_{2}^{2-}, C O, N O )
c. ( N O, C N, N_{2}, O_{2}^{-} )
D. ( N O^{+}, C_{2}^{2-}, O_{2}^{-}, C O )
11
5 Which of the following is a formula of
methanides : ( (a) B e_{2} C(b) C a C_{2}(c) )
( boldsymbol{M} boldsymbol{g}_{2} boldsymbol{C}_{3}(mathrm{d}) boldsymbol{A} boldsymbol{l}_{4} boldsymbol{C}_{3} )
A. Only ( a, d )
B. Only ( a, b )
c. only ( c, d )
D. only ( b, d )
11
6 The most reactive metal is:
A. sodium
B. magnesium
c. potassium
D. calcium
11
7 If the two members of a Dobereiner triad
are phosphorus and antimony, the third member of this triad is :
A. arsenic
B. sulphur
c. iodine
D. calcium
11
8 Which amongst the following has largest size?
A . ( A l )
B. ( A l^{3} )
c. ( C l )
D. ( C l^{-} )
11
9 When a Dobernier triad is considered,
the sum of the atomic weights of the terminal elements ‘X’ and ‘Z’ is 162.5.
The atomic weight of ‘Z’ is 50 units less than 5 times that of ( X ). Calculate the
atomic weights of ( X, Y, ) and ( Z . ) Identify their positions in the present periodic table.
11
10 The electronic configuration of silicon is and that of sulphur is
A. silicon – 2, 8, 1; Sulphur – 2, 8, 6
B. Silicon – 2, 8, 4; Sulphur – 2, 8, 3
c. silicon – 2, 8, 2; sulphur – 2, 8, 6
D. silicon – 2, 8, 4; Sulphur – 2, 8, 6
11
11 Which of the following species have the same number of electrons in its
outermost as well as penultimate shell?
A ( cdot C l )
B. ( O^{2} )
c. ( N a^{+} )
D. ( M g^{2+} )
11
12 What type of oxide would aluminium
form ?
A. ( E O_{3} )
в. ( E_{3} O_{2} )
( mathrm{c} cdot E_{2} mathrm{O}_{3} )
D. EO
11
13 The correct option with respect to the Pauling electronegativity values of the elements is:
This question has multiple correct options
A. Ga <Ge
B. ( S is )
D. B <C
11
14 Identify the wrong statement for long
form of periodic table.
A. It reflects the sequence of filling the electrons in the order of energy levels ( mathrm{K}, mathrm{L}, mathrm{M}, mathrm{N} )
B. It helps to predict the stable valence states of the elements
C. It reflects trends in physical and chemical properties of the elements
D. It helps to predict the relative ionicity of the bond between any two elements
11
15 Assertion:
In the periodic table, the atomic radius increases from left to right.
Reason:
The number of protons is increasing
from left to right.
( A )
Both Assertion and Reason are true and the Reason is the correct explanation of the Assertion.
B. Both Assertion and Reason are true, but Reason is not the correct explanation of the Assertion.
c. Assertion is true, but the Reason is false.
D. Assertion is false, but the Reason is true
E. Both assertion and reason is incorrect
11
16 The alkaline earth metal which shows
some properties similar to aluminium
is:
A. ( C a )
в. ( B e )
( c cdot s r )
D. ( B a )
11
17 The most electronegative element is:
A. nitrogen
B. fluorine
c. oxygen
D. chlorine
11
18 Of the given alkali metals, the one with the smallest size is:
( A cdot R b )
B. cs
( c cdot k )
D. Na
11
19 From the elements of the following atomic numbers 9,12,16,20,38,47
and ( 56, ) identify the elements that belong to same group in periodic table:
A .9,16,39
В. 12,20,47
c. 20,38,47
D. 12,20,56
11
20 033. In the modern periodic table, the period indicates the value of
(a) atomic number (b) mass number (C) principal quantum number (d) azimuthal quantum
number?
.
obou
11
21 The first ionization potential of ( N a ) is 5.1 ( e V ). The value of electron gain
enthalpy of ( N a^{+} ) will be :
A. ( -5.1 mathrm{eV} )
B. ( -10.2 mathrm{eV} )
( mathbf{c} .+2.55 mathrm{eV} )
D. -2.55 eV
11
22 ( x, y, z ) are 3 members of
Doheriner Periods. Atomic masses of ( x )
y are ( 7 mathrm{u} ) & ( 23 mathrm{u} ). What should be the
mass of z? How?
11
23 Mendeleev arrange the elements in the increasing order of their atomic weight in his periodic table.
If true enter 1 , else enter 0 .
11
24 As we go down in the electro-chemical
series of metals, the reactivity
A. decreases and then increases
B. increases and then decreases
c. decreases
D. increases
11
25 Which of the following represent(s) the correct order of electron affinities?
This question has multiple correct options
( A cdot F>C mid>B r>1 )
B. ( c<N<C I<F )
c. ( N<c<0<F )
( D cdot c<operatorname{sic} P<N )
11
26 Recently discovered elements (August 2003 ) with atomic number 113 and 115
have valence electrons in:
A . ( s ) -orbital
B. ( p ) -orbital
c. ( d ) -orbital
D. ( f ) -orbital
11
27 10. Which element has smallest size?
(a) B
(b) N
(c) Al
(d) P
5
11
28 ( left(frac{m}{m}right) )
mand
nth
ith
ution
( ^{M(s)+frac{1}{2} x_{1} rightarrow M^{+} X-(s)} )
ใermsseseous met geeous cati
def
tortereonmere
nswer
‘spositien why
11
29 True or False
Potassium is the most reactive alkali
metals.
11
30 What are the limitations of Mendeleev
periodic table:
11
31 When a Dobereiner’s triad is
considered, the sum of atomic weights of the terminal elements ( X ) and ( Z ) is
162.5. The atomic weight of ( Z ) is 50 units
less than 5 times that of ( X ). Identify the
periods of ( X, Y ) and ( Z ) respectively in the present periodic table.
A. 3,4,5
в. 4,5,6
c. 2,3,4
D. 3,5,4
11
32 Equal lengths of magnesium ribbons are taken in two test-tubes ( X ) and ( Y )
Hydrochloric acid is added to test-tube
( X ) and acetic acid is added to test-tube
( boldsymbol{Y} )
In which test-tube, the reaction will be
more vigorous ? Why?
11
33 Mendeleev classified elements in:
A. increasing order of atomic groups.
B. seven periods and eight groups.
C. seven periods and nine groups
D. eight periods and seven groups
11
34 Which one of the following elements show different oxidation states?
A. Sodium
B. Fluorine
c. chlorine
D. Potassium
11
35 Why was the method of classification,
suggested by Dobereiner, discarded?
A. The weights were wrongly calculated
B. Many elements were unknown at that time
c. only three triads were formed from the elements known at that time
D. None of the above
11
36 The elements with atomic numbers
2,10,18,36,54 and 86 are all
A. Light metals
B. Halogens
c. Rare earths
D. Noble gases
11
37 Which of the above is reactive non
metal?
( mathbf{A} cdot mathbf{1} )
B. 2
( c cdot 3 )
( D )
11
38 The element having most stable oxidation state +2 is
A. ( Q )
B.
( c cdot s )
D. T
11
39 The valency of elements in group I A is:
( A cdot 0 )
B.
( c cdot 2 )
D. 3
11
40 The magnetic nature of elements depends on the presence of unpaired electrons. Identify the configuration of transition elements which shows
highest magnetic momentum:
( mathbf{A} cdot 3 d^{7} 4 s^{2} )
B. ( 3 d^{5} 4 s^{1} )
c. ( 3 d^{8} 4 s^{2} )
D. ( 3 d^{2} 4 s^{2} )
11
41 The correct order of electron affinity of ( B, C, N, O ) is :
A. ( O>C>N>B )
в. ( B>N>C>O )
c. ( O>C>B>N )
D. ( O>B>C>N )
11
42 Why is the ( boldsymbol{E}^{0} ) value of ( boldsymbol{M} boldsymbol{n}^{+3} / boldsymbol{M} boldsymbol{n}^{+2} )
couple much more positive than ( boldsymbol{C r}^{+mathbf{3}} / boldsymbol{C r}^{+mathbf{2}} )
A. Due to larger third ionisation enthalpy of Mn.
B. Due larger third ionisation enthalpy of Cr.
c. Due to smaller third ionisation enthalpy of Mn.
D. Due to lesser hydration enthalpy of Cr.
11
43 The given diagram represents 11
44 Which of the following relation is
correct?
( mathbf{A} cdot I^{s t} ) IE of ( C>I^{s t} ) IE of ( B )
B ( cdot I^{s t} ) IE of ( CI I^{n d} ) IE of ( B )
D. Both (B) and (C)
11
45 Effective nuclear charge ( left(Z^{*}right) ) can be
calculated by using the formula:
( mathbf{A} cdot Z^{*}=Z-S )
B . ( Z^{*}=Z+S )
c. ( Z^{*}=S-Z )
D. ( Z=Z^{*}-S )
11
46 The last element of actinide series is :
A. thorium
B. cerium
c. lawrencium
D. Iutetium
11
47 Which of the following is incorrectly matched?
A . alkali metal ( rightarrow ) cesium
B. alkali earth metal ( rightarrow ) barium
c. chalcogens ( rightarrow ) silicon
D. halogon ( rightarrow ) iodine
11
48 Forces of attraction between particles in a pure substance are associated with physical properties. Additionally, specific trends are associated with a given group of elements. Of the following, which shows the greatest variation in physical properties for the given group of elements?
A. Alkali metals
B. Alkaline earth metals
c. Halogens
D. Noble gases
11
49 Reducing nature in increases
with increase in atomic number in
alkali metals.
A. period
B. group
c. both ( A ) and ( B )
D. none of these
11
50 How would you react on this statement?
Electronegativity of nitrogen (N) on Pauling scale is 3.0 in all the nitrogen compounds.
11
51 Mendeleev corrected the atomic weight
of :
( A cdot B e )
B. ( N )
( c cdot O )
D. ( C l )
11
52 An inert gas with more than one orbit,
has electrons in its outermost
shell.
( A cdot O )
B. 2
( c cdot 4 )
D. 8
11
53 What type of oxide would Ekaaluminium form?
A. ( E O_{3} )
в. ( E_{3} O_{2} )
( mathrm{c} cdot E_{2} mathrm{O}_{3} )
D. ( E O )
11
54 Which one of the following belongs to representative group of elements in the periodic table?
A. Lanthanum
B. Tungston
c. Chromium
D. Aluminium
11
55 In general, the properties that decrease and increase down a group in the periodic table, respectively, are:
A. electronegativity and electron gain enthalpy.
B. electronegativity and atomic radius
c. atomic radius and electronegativity
D. electron gain enthalpy and electronegativity
11
56 Which group of elements does not show diagonal relationship?
A. ( L i, M g )
в. ( B e, A l )
( mathbf{c} cdot B, S i )
D. ( C, P )
11
57 The columns of the periodic table are called groups.
A . True
B. False
11
58 In a group, basic nature
from top to bottom.
A. increases
B. decreases
c. remains same
D. none of these
11
59 The element, with atomic number 118 will be
A . Alkali
B. Noble gas
c. Lanthanide
D. Transition element
11
60 Among the following outermost configuration of metals which shows the highest oxidation state?
A ( cdot 3 d^{3} 3 s^{2} )
B . ( 3 d^{5} 4 s^{1} )
( mathbf{c} cdot 3 d^{5} mathbf{4} s^{2} )
D. ( 3 d^{4} 4 s^{2} )
11
61 Q. 13 Electronic configuration of four elements A, B, C, and D are given below
A. 15° 2s 2p
B. 1s 2s 2p
C. 1s 2s 2p 3s
D. 1s 2s 2p
Which of the following is the correct order of increasing tendency to
gain electron?
(a) A <C<B<D
(b) A <B<C<D
(CD <B<C<A
(d) D<A <B<C
11
62 Which ion has the least value of
theoritical magnetic moment?
A ( cdot C r^{3} )
в. ( C o^{3} )
( c cdot T i^{3} )
D. ( V^{3+} )
11
63 The elements which have taken the
place of Eka aluminium is :
A. Germanium
B. Gallium
c. silicon
D. Aluminium
11
64 The attempt for classifying elements by plotting the atomic masses of elements against the atomic volumes was made
by:
A. Dobereiner
B. Newlands
c. Lother Meyer
D. Mendeleev
11
65 Classification of periodic table based on atomic number is given by:
A. Mendeleev’s
B. Mosley
c. Both A and B
D. None of these
11
66 An element having atomic number 50 Find its group number and period numbers. 11
67 Following statements regarding the periodic trends of chemical reactivity of
alkali metals and the halogens are
given.Which of these statements give
the correct picture?
A. In alkali metals, the reactivity increases but for halogens it decreases with increase in atomic number down the group.
B. The reactivity decreases in the alkali metals but increases in the halogens with increase in atomic number down the group.
C. In both the alkali metals and the halogen the chemical reactivity decreases with increase in atomic number down the group.
D. Chemical reactivity increases with increase in atomic number down the group.
11
68 Q29. Write the general electronic configuration of s-, p-, d-, and f-block elements? 11
69 Consider an atom with the electron
configuration of ( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} )
Which successive ionization energy will be significantly higher than the previous value?
A. First ionization energy.
B. Second ionization energy
c. Third ionization energy.
D. Fourth ionization energy
11
70 The biggest atom is:
A. radium
B. francium
c. caesium
D. rhodium
11
71 Which of the following properly explains why the atomic radius decreases going cross a period from left to right?
A. As you cross the period from left to right, the number of electron orbital shells decreases as the number of protons remains constant
B. As you cross the period from left to right, the number of protons decreases as the number of electron orbitals remains constant.
C. As you cross the period from left to right, the number of electron orbital shells increases as the number of protons remains constant
D. As you cross the period from left to right, the number of protons increases as the number of electron orbitals remains constant
11
72 A newly discovered element ( X ) is placed
in group ( I A ) of the periodic table since it forms :
A. an oxide which is acidic
B. a volatile chloride having a formula ( X C l )
c. an ionic chloride having the formula ( X C l )
D. an insoluble ( X S O_{4} )
11
73 In the periodic table as formulated by Mendeleev, which of the following
constitute an anomalous pair of elements?
( mathbf{A} cdot H ) and ( H e )
B. ( B r ) and ( N e )
c. ( K ) and ( A r )
D. ( N a ) and ( B )
11
74 What were the limitations of
Dobereiner’s classification?
11
75 Which reaction is most spontaneous?
A ( cdot G a^{3+}+2 e^{-} rightarrow G a^{+} )
B. ( I n^{3+}+2 e^{-} rightarrow I n^{+} )
( mathbf{c} cdot T l^{3+}+2 e^{-} rightarrow T l^{+} )
D. cannot be predicted
11
76 Atomic size of nickel, cobalt and iron is
in order of : ( boldsymbol{F e}>boldsymbol{C o}>boldsymbol{N i} )
A. True
B. False
11
77 Consider the following changes:
( boldsymbol{A} rightarrow boldsymbol{A}^{+}+boldsymbol{e}^{-}: boldsymbol{E}_{1} ) and ( boldsymbol{A}^{+} rightarrow boldsymbol{A}^{2+}+ )
( e^{-}: E_{2} )
The energy required to pull out the two
electrons are ( E_{1} ) and ( E_{2} ) respectively. The correct relationship between two energies would be:
A ( cdot E_{1}E_{2} )
D. ( E_{1} neq E_{2} )
11
78 The Newland’s law of octaves for the
classification of elements was found to
be applicable only up to the element
A. potassium
B. calcium
c. cobalt
D. phosphorous
11
79 Without knowing the electronic configurations of the atoms of elements Mendeleev still could arrange the elements nearly close to the arrangements in the Modern periodic table. How can you appreciate this? 11
80 The element placed with cerium, in the table formed by Newlands’ was:
A . actinium
B. lanthanum
c. lawrencium
D. zirconium
11
81 enthalpies and electron gain enthalpies of
.44 Match the correct ionisation enthalpies and electron gain en
the following elements.
Elements
AH, AH AH
Most reactive non-metal A 419
3051
– 48
(1) Most reactive metal B. 1681 3374 -328
(ii) Least reactive element C 738 1451 – 40
(iv) Metal forming binary halide D. 2372 5251 +48
11
82 most
Q. 21 The electronic configuration of the outer most shell
electronegative elements is
(a) 2s22p5
(b) 3s 3p5
(C) 45-4p
(d) 5s25p5
11
83 Number of vertical columns in the
modern periodic table are:
A. 7
B. 8
c. 10
D. 18
11
84 The elements having more masses were placed before elements having lower masses in Mendleev’s periodic table. Guess the pair of elements (higher mass, lower mass)
A. Cobalt, Nickel
B. Vanadium, Chromium
c. Tellurium, lodine
D. All of the above
11
85 The maximum number of valence
electrons possible for atoms in the second period of the periodic table is :
A .2
B. 8
c. 18
D. 32
11
86 The ( 4 f ) level is successively filled up in:
A. alkali metalss
B. rare gases
c. lanthanides
D. actinides
11
87 The electronic configurations of three elements ( X, Y ) and ( Z ) are given below. Which of the following is correct? ( x: 2,8 )
( Y: 2,8,7 )
( Z: 2,8,2 )
A. ( x ) is a metal
B. Y is a metal
c. ( z ) is a non-metal
D. Y is a non-metal and ( z ) is a metal
11
88 Q. 31 Illustrate by taking examples of transition elements and non-transition
elements that oxidation states of elements are largely based on
electronic configuration.
11
89 According to the law of triads:
A. the properties of the middle element were in between those of the other two members.
B. three elements arranged according to increasing weights have similar properties.
C. the elements can be grouped in the groups of six elements.
D. every third element resembles the first element in periodic table.
11
90 With reference to periodic table,
indicate:
First transition element of the fourth
period.
11
91 Which of the following pair has electron deficient compounds?
A. ( B_{2} H_{6}, ) AlCla
в. ( C_{2} H_{6}, ) Аl( _{2} C l_{6} )
c. ( S F_{2}, C l_{2} O )
D. ( N a B H_{4}, I C l )
11
92 ( A l ) has lower ionization potential than
that of ( M g ) because:
A. ( A l ) atom is bigger than ( M g ) atom
B. ( M g ) atom is bigger than ( A l ) atom
c. all electrons in ( M g ) are paired, but those of ( A l ) are not
D. all belongs to a higher group
11
93 Which of the following statement is
incorrect?
A. The most electronegative element is fluorine
B. Alkali metals generally have negative value of electron gain enthalpy
C. The oxidation number of ( sin N a_{2} S_{4} O_{6} ) is greater than
in the case of ( N a_{2} S_{2} O_{3} )
D. The electronegativity values for ( 2 p ) series elements is less than that for ( 3 p ) series elements on account of small size and high inter electronic repulsion
11
94 The properties of were predicted by Mendeleev before their isolation.
( A cdot ) Co and ( N i )
B. I and Te
c. ( mathrm{sc} ), Ga and ( mathrm{Ge} )
D. Cl, Ar and K
11
95 Number of electrons in ( M ) shell of an
element with atomic number 28 is
A . 18
B. 16
( c cdot 8 )
D. 2
11
96 Using the periodic table, predict the formulas of compounds which might be formed by the following pairs of elements:
(a) silicon and bromine
(b) aluminium and suplhur.
11
97 Number of orbits present in argon is:
( A cdot 1 )
B. 2
( c .3 )
D. 4
11
98 The decreasing order of electron affinity is:
A. ( I>B r>C l>F )
B. ( B r>C l>F>l )
c. ( F>C l>B r>l )
( mathrm{D} cdot C l>F>B r>l )
11
99 Which of the following is not a noble
gas?
A. Helium
B. Neon
c. Argon
D. Hydrogen
11
100 The non-metal with valency 1 in period 3
is :
A. ( N a )
в. ( M g )
c. ( A l )
D. ( C l )
11
101 Q2. Show by a chemical reaction with water that Na O is a basic oxide and C1,0- is an acidic
oxide.
11
102 Which of the following elements is a metalloid?
A. Lithium
B. Beryllium
c. Boron
D. Carbon
11
103 In the first two groups of periodic table, the group number represents the :
A. valency
B. atomic weight
c. atomic number
D. oxidising nature
11
104 Atomic number of a few elements are
given below:
10,20,7,14
Identify the period to which these elements belong?
A. 2,4,2,3
B. 3, 2, 3, २.
c. 2,2,3,3
D. 3, 3, 2, 2.
11
105 Which of the following electronic configurations in the outermost shell is
characteristic of alkali metals?
A ( cdot(n-1) s^{2} p^{6} n s^{2} p^{1} )
B . ( (n-1) s^{2} p^{6} d^{10} n s^{1} )
C ( cdot(n-1) s^{2} p^{6} n s^{1} )
D ( cdot n s^{2} n p^{6}(n-1) d^{1} )
11
106 The electronic configuration is given as:
( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6} 4 d^{10} 5 s^{2} )
is for:
A. ( f ) -block element
B. ( d ) -block element
c. ( p ) -block element
D. ( s ) -block element
11
107 Arrange the following elements in increasing order of their size.
Be, Ca, Ba, Ra
A. Be <Ca<Ba<Ra
B. ( mathrm{Ca}<mathrm{Be}<mathrm{Ba}<mathrm{Ra} )
c. ( mathrm{Be}<mathrm{Ca}<mathrm{Ra}<mathrm{Ba} )
D. None of these
11
108 Which of the following carbon atoms is most electronegative? ( stackrel{I I I}{C H_{3}}-C_{I H_{2}}^{I I}-C equiv C_{H}^{I} )
( A )
B. I
( c )
D. All are equal electronegative
11
109 An element has its electronic
configuration as ( 2,8,2 . ) Now answer the following question:

To which period does does this element belong?

11
110 What are the demerits of Mendeleev’s
periodic table with respect to the
arrangement of elements in ascending order? (Any three)
11
111 Aluminium does not react with water at
room temperature but reacts with both dil. ( H C l ) and ( N a O H ) solutions. Verify
these statements experimentally. Write your observations with chemical equations. From these observations,
can we conclude that ( A l ) is a metalloid?
11
112 The electronegativity of the elments ( mathrm{C}, mathrm{N}, mathrm{Si} ) and ( mathrm{P} ) increases in the order of ( mathrm{Si} )
( P, C, N )
If true enter 1 , else enter 0 .
A
11
113 Fluorine is the most reactive among all the halogens, because of it’s:
A. small size
B. low dissociation energy of F-F bond
c. large size
D. high dissociation energy of F – F bond
11
114 In chemistry lab class, your teacher asks you to find magnesium oxide, ( M g O, ) to use in the experiment. When you go to the stockroom, you realized there is no magnesium oxide available. Which of the following would be the
most suitable replacement?
A. Sodium oxide, ( N a_{2} O )
B. Calcium oxide, ( C a O )
c. carbon dioxide, ( C O_{2} )
D. silicon dioxide, ( S i O_{2} )
11
115 Isotopes could find a position in Mendeleev’s periodic table.
A. True
B. False
11
116 Arrange the following set of atoms in the order of increasing atomic radius:
( boldsymbol{F}, boldsymbol{C l}, boldsymbol{C}, boldsymbol{O} )
A. ( F, C l, O, C )
в. ( C, O, F, C l )
c. ( O, C, F, C l )
D. ( F, O, C, C l )
11
117 Assertion
Mendeleev’s periodic table have some demerits.
Reason
There was no place for all isotopes of the elements and some heavy elements
were placed before lighter elements.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
118 Electronic configuration of element T is 2,8,7
What is the group number of T?
A . 15
B. 16
( c cdot 17 )
D. 18
11
119 Dobereiner classified elements into
groups based on their properties. The number of elements in each group is
11
120 In the periodic table, the element with atomic number 6 will be in:
A. second period
B. third period
c. fourth period
D. fifth period
11
121 The correct order of decreasing polarity
¡s:
( mathbf{A} cdot H F>S O_{2}>H_{2} O>N H_{3} )
B ( cdot H F>H_{2} O>S O_{2}>N H_{3} )
( mathbf{C} cdot H F>N H_{3}>S O_{2}>H_{2} O>H F )
D. none of the above
11
122 Hydrogen resembles:
A. alkali metals
B. halogens
C. both ( A ) and ( B )
D. none of the above
11
123 Which scientist came up with the
concept of a periodic table that included all of the known elements?
A. Joseph Priestly
B. Dmitri Mendeleev
c. Antoine Lavoisier
D. Albert Einstein
11
124 The elements whose atomic weight was corrected by Mendeleev are
A. Uranium.
B. Indium
c. Beryllium
D. All of these
11
125 In the periodic table, vertical columns of elements are called ( ldots . . ) and horizontal
rows of elements are called
A. Groups, periods
B. Periods, groups
c. Periods, periods
D. Groups, groups
11
126 What is the value (including the sign) of the electron gain enthalpy or electron
affinity of ( N a^{+} ) ion in electron -volts?
The first ionization potential for Na is ( 118 mathrm{k} ) cal/mole.
11
127 An atom has electronic configuration
( 2,8,7 . ) To which of the following elements would it be chemically similar? (Atomic numbers are given in parentheses)
A . N(7)
B. F(9)
c. ( P(15) )
D. ( operatorname{Ar}(18) )
11
128 The standard emf of a galvanic cell involving cell reaction with ( n=2 ) is found to be ( 0.295 mathrm{V} ) at ( 25 mathrm{C}^{circ} ). The
equilibrium constant of the reaction would be
(Given, ( boldsymbol{F}=mathbf{9 6 5 0 0} boldsymbol{C m o l}^{-1}, boldsymbol{R}= )
( left.8.314 J K^{-1} m o l^{-1}right) )
A ( .2 .0 times 10^{11} )
B . ( 4 times 10^{12} )
( c cdot 1 times 10^{2} )
D. ( 1 times 10^{10} )
11
129 Find the oxidation numbers to the
underlined species in the following compounds or ions.
A) ( N a underline{B} H_{4} )
B) ( boldsymbol{H}_{2} boldsymbol{P} boldsymbol{t} boldsymbol{C l}_{boldsymbol{6}} )
11
130 The element which cannot form a cation
is:
A . ( A l )
в. ( B )
c. ( C s )
D. ( B i )
11
131 6. The pair of amphoteric hydrogen is:
(a) Li(OH), Al(OH), (b) Be(OH),, Mg(OH)2
(c) B(OH)2, Be(OH), (d) Be(OH)2, Zn(OH)2
11
132 Q17. How would you explain the fact that the first ionization enthalpy of sodium is lower than that
of magnesium but its second iorization enthalpy is higher than that of magnesium?
11
133 The correct order of stability of
( boldsymbol{A l}^{+}, boldsymbol{A l}^{+2}, boldsymbol{A l}^{+mathbf{3}} mathbf{i s} )
A ( cdot A l^{+3}>A l^{+2}>A l^{+} )
B. ( A l^{+2}>A l^{+3}>A l^{+} )
c. ( A l^{+2}A l^{+} )
D. ( A l^{+3}>A l^{+}>A l^{+} )
11
134 If each orbital can hold a maximum of 3
electrons. The number of elements in
( 2^{n d} ) period of the periodic table (long form) will be:
A . 27
B. 9
c. 18
D. 12
11
135 ( ln ) a triad of ( A, B, C ) elements if the
atomic masses of ( A ) and ( C ) respectively
are 100 and ( 200, ) then the atomic mass
of ( B ) is:
A . 300
в. 175
c. 125
D. 150
11
136 6. In the isoelectronic species the ionic radii (Å) of N3-,
02- and F are respectively given by
(a) 1.71, 1.40, 1.36 (b) 1.71, 1.36, 1.40
(c) 1.36, 1.40, 1.71 (d) 1.36, 1.71, 1.40
11
137 Write Newland’s Law of ‘Octaves’ for
classification of elements.
11
138 The ratio of magnetic moments of ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+} )
( & C o^{3+} ) is:
B. ( sqrt{35}: sqrt{24} )
( c cdot 7: 3 )
D. ( sqrt{24}: sqrt{15} )
11
139 The electronic configuration of neon is:
( mathbf{A} cdot 1 mathbf{s}^{2} 2 mathbf{s}^{2} 2 mathbf{p}^{6} )
B. ( 1 mathrm{s}^{2} )
( c cdot 2 s^{2} )
D. ( 1 s^{2} 2 s^{2} 2 p^{2} )
11
140 Q.53 Write the drawbacks in Mendeleef’s periodic table that led to its
modification.
11
141 Which of the following elements doesn’t belong to group IIA or 2nd group?
A . Be
в. Мв
( c cdot L )
D. ca
11
142 The following statements concern elements in the periodic table. Which of the following is true?
A. For Group 15 elements, the stability of +5 oxidation state increases down the group
B. Elements of Group 16 have lower ionization enthalpy values compared to those of Group 15 in the corresponding periods
c. The Group 13 elements are all metals
D. All the elements in Group 17 are gases
11
143 Isotopes could find a position in Mendeleev’s periodic table. State whether the given statement is
true or false.
A. True
B. False
11
144 The number of atoms contained in a fcc
unit cell of a monatomic substance is
11
145 The atomic number of natural
radioactive element is:
A. greater than 82
B. lesser than 82
c. not defined
D. at least 92
11
146 Which of the following group of elements belong to the representative
group?
A. ( L i, M g, N, Z n )
в. ( A g, A u, Z n )
c. ( N a, K, B e )
D. ( F e, C u, M n )
11
147 1. The highest ionization energy is exhibited by
(a) halogens
(b) alkaline earth metals
c) transition metals
(d) noble gases
11
148 For the data given, calculate the energy
deficit in the formation ( B e C l_{2} ) (it is a
stable molecule)
I. ( boldsymbol{E}_{1} ) for ( boldsymbol{B e}=mathbf{8 9 9 k J} / boldsymbol{m o l} )
I. ( boldsymbol{E} ). for ( boldsymbol{B e}=mathbf{1 7 5 7 k J} / boldsymbol{m o l} )
I.A. for ( C l=-348 k J / ) mol
11
149 Which gases were unknown at the time of Mendeleev?
A. Oxygen
B. Noble gases
( c cdot C O_{2} )
D. None of the above
11
150 Fill in the blanks: Periods are
[5,6,7] horizontal rows of
elements in the periodic table and an element with three electron shells and
two electrons in its valence shell
belongs to period [6,3,1] and
group [3,6,2]
11
151 What is the electronic configuration for ( operatorname{an} F e(I I I) ) ion in its ground state?
( mathbf{A} cdot[A r] 3 d^{5} )
B . ( [A r] 3 d^{6} )
( mathbf{c} cdot[A r] 4 s^{2} 3 d^{3} )
D ( cdot[A r] 4 s^{2} 3 d^{6} )
11
152 How did Mendeleev predict the existence of some yet to be discovered elements in his periodic table?
A. Gaps
B. Atomic number
c. Mass number
D. None of the above
11
153 Choose the correct answer from the four
alternatives given in the brackets:
Number of periods in modern periodic table is
(7,17,8,18)
11
154 The second ionization energies among Li. Be. ( B ) and ( C ) s lowest for
( mathbf{A} cdot L i )
в. ( B e )
( c . B )
D. ( C )
11
155 Can the following groups of elements be classified as Dobereiner’s triad:
(a) ( mathrm{Na}, mathrm{Si}, mathrm{Cl} )
(b) Be, Mg, Ca
Justify the answer in each case.
[Atomic mass of ( boldsymbol{B e}-mathbf{9} ; boldsymbol{N} boldsymbol{a}- )
( mathbf{2 3} ; boldsymbol{M} boldsymbol{g}-mathbf{2 4} ; boldsymbol{S} boldsymbol{i}-mathbf{2 8} ; boldsymbol{C l}-mathbf{3 5} ; boldsymbol{C} boldsymbol{a}- )
40]
11
156 Consider the above figure as Periodic
Table. Then the element with a possible
oxidation number of -2 is
begin{tabular}{|c|c|c|c|c|c|}
hline ( mathbf{z}_{mathbf{L i}} ) & & & & & ( mathbf{( D )} ) & ( mathbf{1 0} ) \
hline & ( mathbf{( A )} ) & & & & ( mathbf{( C )} ) & & \
hline ( mathbf{( B )} ) & ( mathbf{2 0} ) & & & & & \
hline
end{tabular}
( mathbf{A} )
( B )
a
( D )
11
157 Representative elements
are
A. Elements of s and p block
B. Elements of s, p and f block
C. Elements of ( s, p ) and d block
D. Elements of s and d block
11
158 toppr LoGın
Q Type your question
enthalpy ( left(text { in } mathrm{kJ} mathrm{mol}^{-1}right) ) of a few elements
are given below:
begin{tabular}{llll}
Elements & ( boldsymbol{Delta} boldsymbol{H}_{1} ) & ( boldsymbol{Delta} boldsymbol{H}_{2} ) & ( boldsymbol{Delta}_{e g} mathbf{H} ) \
1 & 520 & 7300 & -60 \
11 & 419 & 3051 & -48 \
hline 111 & 1681 & 3374 & -328 \
hline ( mathrm{IV} ) & 1008 & 1846 & -295 \
( mathrm{V} ) & 2372 & 5251 & +48 \
hline ( mathrm{V} ) & 738 & 1451 & -40
end{tabular} Which of the above elements is likely to
be:
(a) the least reactive element,
(b) the most reactive metal,
(c) the most reactive non-metal,
(d) the least reactive non-metal,
(e) the metal which can form a stable
binary halide of the formula ( mathrm{M} mathrm{X}_{2} )
(X=halogen) and
(f) the metal which can form a
predominantly stable covalent halide of
th ( cdot ) mula MX (X=halogen)?
11
159 Write Newland’s Law of Octaves.
Write the name of element having similar properties of the following.
(a) Nitrogen
(b) Lithium
11
160 In hydrogen atom the energy difference between the states ( n=2 ) and ( n=3 ) is
Ee ( V ). The ionisation potential of ( H )
atom is:
A . ( 3.2 E )
в. ( 5.6 E )
( c .7 .2 E )
D. ( 13.2 E )
11
161 Calculate the electronegativity of chlorine from bond energy of ( boldsymbol{C l}-boldsymbol{F} )
bond ( left(61 k c a l m o l^{-1}right) F- )
( Fleft(38 k c a l m o l^{-1}right) ) and ( C l-C l ) bond
( left(58 k c a l m o l^{-1}right) ) and electronegativity
of fluorine ( 4.0 e V )
A. 1.42 eV
в. 1.89 eV
c. 2.67 eV
D. 3.22 eV
11
162 The electron configuration of ( _{11} N a^{23} ) is
A ( cdot 1 s^{2}, 2 s^{2}, 2 p^{5}, 3 s^{2} )
B . ( 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{1} )
C ( cdot 1 s^{2}, 2 s^{2}, 2 p^{4}, 3 s^{1}, 3 p^{2} )
D. ( 1 s^{1}, 2 s^{1}, 2 P^{6}, 3 s^{2}, 3 p^{1} )
11
163 Describe the two merits of long form periodic table over the Mendeleev’s
periodic?
11
164 If ( (N, P, A s) ) was Dobereiner’s triads
then what would be the absolute error in
atomic mass of phosphorous as compared to the original mass?
Atomic mass: Nitrogen ( =14 ) amu, Arsenic ( =mathbf{7 4 . 9} ) amu, Phosphorous ( =mathbf{3 1} )
amu
A. 13.45
B. 12.45
c. 15.55
D. 16.55
11
165 Ba is
A. more electronegative
B. more electropostive
C . less electropositive
D. none of the above
11
166 Which of the following reactions are
possible?
This question has multiple correct options
( mathbf{A} cdot 3 M g+2 A l^{3+} rightarrow 2 A l+3 M g^{2+} )
B ( cdot C l_{2}+2 I^{-} rightarrow I_{2}+2 C l^{-} )
( mathbf{c} cdot K^{+}+N a rightarrow K+N a^{+} )
( mathbf{D} cdot K+N rightarrow K^{-}+N^{+} )
11
167 How does number of (i) valence
electrons (ii) valency; vary on moving from to right:
(a) in the second period of a periodic table ?
(b) in the third period of a periodic table
( ? )
11
168 Electronegativity across the period:
A. increases
B. decreases
c. remains constant
D. can’t be predicted
11
169 How many elements were known at the
time of Mendeleevs classification of
elements?
11
170 What is the apparent oxidation state of
( boldsymbol{K} ) element in the compound ( boldsymbol{K} boldsymbol{H} boldsymbol{C} boldsymbol{O}_{3} ? )
A ( .+1 )
B. +2
( c cdot+3 )
D. +4
( mathrm{E} cdot+5 )
11
171 The third ionization energy amongst ( boldsymbol{L} boldsymbol{i}, boldsymbol{B} e, boldsymbol{B} ) and ( boldsymbol{C} ) is lowest for
A . ( L i )
в. ( B e )
( c . B )
D. ( C )
11
172 The element with atomic number 16
belongs to which period?
A .2
B. 3
( c cdot 4 )
D.
11
173 Q14. What is the significance of the terms – isolated gaseous atom and ground state while defining
the ionization enthalpy and electron gain enthalpy?
[Hint: Requirements for comparison purposes]
macamus state are
11
174 Assertion
lonisation potential increases with
increase in nuclear charge of the
elements.
Reason
lonization energies increase moving from left to right across a period.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
175 In the electronic configuration,
outermost orbit number is considered
as its period number.
A. True
B. False
11
176 Complete the following Table:
Electronic

Bo
Element configuration ( quad ) forms
Magnesium
Oxygen
Chlorine

11
177 Mendeleev’s periodic law states that the properties of elements are a periodic function of their:
A. reactivity of elements
B. atomic size
c. atomic mass
D. electronic configuration
11
178 Match column I with column II and
select the correct answer using the codes given below:
Column I ( quad ) Column
(A) ( frac{14}{6} C ) and ( _{6}^{13} C )
(p) Different
number of neutrons
(B) 40
20 ( mathrm{Ca} ) and ( _{18}^{40} boldsymbol{A r} )
(q) Different
number of protons and neutrons
(C) ( boldsymbol{K}(mathbf{1} mathbf{9}) )
(r) Non-metal
(D) Chlorine (17)
(s) Metal
( A cdot A-(p) ; B-(q) ; C-(r) ; D-(s) )
B. ( A-(q) ; B-(p) ; C-(s) ; D-(r) )
c. ( A-(p) ; B-(q) ; C-(s) ; D-(r) )
( D cdot A-(p) ; B-(s) ; C-(q) ; D-(r) )
11
179 Mendeleev arranged the known elements in a/an order of
their atomic masses.
A. increasing
B. decreasing
c. random
D. none of the above
11
180 The element with atomic number ( Z= )
115 will be placed in :
A ( cdot 7^{t h} ) period , 1 A group
B. ( 8^{t h} ) period , IV A group
C. ( 7^{t h} ) period ( , ) V A group
D. ( 6^{t h} ) period , ( vee ) B group
11
181 In periodic table, which period have most electronegative elements?
A .
B. 2
( c cdot 3 )
D. 4
E. 5
11
182 Which element exhibits the greatest
number of oxidation states in its
compounds?
A. ( C a )
в. ( V )
c. ( C u )
D. Na
11
183 Q9. What does atomic radius and ionic radius really mean to you? 11
184 The second ionization enthalpy is ( ? )
A. smaller than the first ionization enthalpy.
B. almost equal to the first ionization enthalpy.
C. smaller than the third ionization enthalpy.
D. equal to the second electron gain enthalpy.
11
185 Assertion
Atomic number of the element
ununtrium is 113
Reason
According to IUPAC systematic nomenclature, the numerical roots for
1,1 and 3 are un, un and tri respectively
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
186 Which of the following is correct order of increasing size?
(a) Br”>52- > Cr > Nat > Mg2+ > Be2+
(b) Be2+ > Mg2+ > Nat > 82-> Ci* >Brid
(c) s->cr > Br”> Na* > Mg2+ > Be 2+
(d) Na > Mg2+ > Be2+ > Br > 52->cr
11
187 Modern periodic table contains vertical columns.
A . 17
B. 19
c. 18
D. 20
11
188 Assertion
The atomic radii of the elements of
oxygen family are smaller than the atomic radii of corresponding elements of the nitrogen family.
Reason
The members of oxygen family are all more electronegative and thus have
lower value of nuclear charge than
those of the nitrogen family.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
189 In the electronic configuration, outermost orbit number is considered
as:
A. period
B. group
c. octet
D. none of these
11
190 The pair of amphoteric hydroxides is:
A. ( A l(O H)_{3}, L i O H )
B. ( B e(O H)_{2}, M g(O H)_{2} )
c. ( B(O H)_{3}, B e(O H)_{2} )
D. ( B e(O H)_{2}, Z n(O H) )
11
191 The total number of groups in Modern Periodic table is
A. 7
B. 17
c. 18
( D )
11
192 Alkyl halides react with dialkyl copper
reagents to give:
A. Alkenyl Halide
B. Alkanes
c. Alkyl copper halides
D. alkenes
11
193 Which of the following is not a metalloid?
A. Silicon
B. Germanium
c. Arsenic
D. Beryllium
11
194 Q20. Which of the following pairs of elements would have a move negative electron gain enthalpy?
O O or F (ii) For CI.
Bottle and liind period An era move from
the atomic size
11
195 ( boldsymbol{M}+mathbf{8} boldsymbol{C} boldsymbol{N}^{-}+mathbf{2} boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{O}_{2} rightarrow )
( mathbf{4}left[boldsymbol{M}(boldsymbol{C} boldsymbol{N})_{2}right]^{-}+mathbf{4} boldsymbol{O} boldsymbol{H}^{-} )
metal M is:
A. cu
в. ( mathrm{Hg} )
c. ( A g )
D. Au
11
196 Which element of 2nd period forms most acidic oxide?
A. Flourine
B. Nitrogen
c. Boron
D. Carbon
11
197 Which has the same electronic
configuration as of inert gas?
A ( cdot mathrm{Ag}^{3} )
B. ( mathrm{Cu}^{2} )
( c cdot P b^{4} )
D. ( mathrm{Ti}^{4} )
11
198 The element whose II (I.P.) is less than
its ( |(mid . P .) )
A. ( L )
B. Be
c. не
D. None
11
199 Hydrargyrum is the latin name of: 11
200 In the long form of periodic table, the total number of period is:
A. 5
B. 7
( c cdot 8 )
D.
11
201 The atomic numbers of elements
( A, B, C ) and ( D ) are ( Z-1, Z, Z+1 ) and
( Z+2, ) respectively. If ( ^{prime} B^{prime} ) is a noble gas, choose the correct answers from the following statements
(1) ( ^{prime} A^{prime} ) has higher electron affinity
(2) ‘ ( C^{prime} ) exists in +2 oxidation state
(3) ‘ ( D^{prime} ) is an alkaline earth metal
A ( cdot(1) ) and (2)
B. (2) and (3)
c. (1) and (3)
D. (1),(2) and (3)
11
202 The element placed with nickel in the table formed by Newlands was:
A . iron
B. cobalt
c. chromium
D. copper
11
203 For ( _{24} C r, ) which of the following statements is/are correct?

This question has multiple correct options
A. Number of electrons with principle quantum number is 13
B. Number of electrons with azimuthal quantum number is 12
c. Number of electrons with magnetic quantum number 0 is 12
D. Number of minimum or maximum electrons with spin quantum number ( +1 / 2 ) is 9 or 15

11
204 The oxidation states exhibited by Tin
are:
( mathbf{A} cdot+2 ) and +4
B. +1 and +2
c. +3 and +4
D. +4 only
11
205 Which of the following statement is
incorrect?
A. Reducing power in aqueous solution is maximum for lithium metal.
B. Electron affinity order ( O^{+}>O>O^{-}>O^{2-} )
C. Order of oxidation number of oxygen ( O_{3}>K O_{2}> )
( B a O_{2}>K_{2} O )
D. ( p H ) of aqueous solution ( L i C l>B e C l_{2}>M g C l_{2}> )
( A l C l_{3} )
11
206 Assertion
Electron affinity value of ( C l^{-} ) has negative value.
Reason
Electron affinity values of all uninegative ions are negative.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
207 An element with the electron
configuration ( [boldsymbol{X} boldsymbol{e}] boldsymbol{4} boldsymbol{f}^{14} boldsymbol{5} boldsymbol{d}^{7} boldsymbol{6} boldsymbol{s}^{2} ) is:
A. an alkaline earth element
B. a transition element
c. an inertgas
D. a rare earth
11
208 un tne basıs or Ivlenaeleevs rerıoaıc
Table given below, answer the question
that follow the table:
Ref. image
Besides gallium, which two other
elements have since been discovered
for which Mendeleev had left gaps in his
Periodic Table? Using atomic masses of
Li,NaLi,Na, find the average atomic
mass of and compare it with the atomic
mass of. State the conclusion drawn
from this activity.
11
209 Prussian blue has two types of iron with oxidation number as shown ( prod_{boldsymbol{F}}^{boldsymbol{I I I}}[stackrel{boldsymbol{I I}}{left.boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]}] )
net charge on Prussian blue is – ( x ). The value of ( x ) is
11
210 Atomic radii of fluorine is 42 pm. Atomic radii of oxygen is :
A. ( 42 mathrm{pm} )
B. 39 pm
c. ( 41 mathrm{pm} )
D. ( 48 mathrm{pm} )
11
211 Among the following compounds, which one is not responsible for the depletion of ozone layer?
A ( . C H_{4} ) н 2 СО
в. ( C F C l_{3} )
c. ( N O )
D. ( C l_{2} )
11
212 Electron affinity of chlorine is ( -3.61 mathrm{eV} ) ( I P ) value of the same element is 12.967
eV. ( 3 times 10^{23} ) atoms of chlorine are
converted to ( C l^{-} ) ions and the energy
liberated is used to ionize chlorine
atoms to ( C l^{+} ) ions. How many chlorine atoms could be ionized in the above
process?
A ( .5 .45 times 10^{21} )
В. ( 6.11 times 10^{18} )
c. ( 8.35 times 10^{22} )
D. ( 7.11 times 10^{28} )
11
213 Out of the elements with atomic
numbers given below which one would be a halogen?
A . 25
B. 35
c. 45
D. 55
11
214 Mendeleev predicted the existence of
certain elements not known at that
time and named two of them as Eka –
silicon and Eka – Aluminium.

Mention the group of these elements in
the Modern Periodic Table :
A. Group 12 and Group 13.
B. Group 14 and Group 15.
c. Group 14 and Group 13.
D. Group 15 and Group 13

11
215 Consecutive elements ( X, Y ) and ( Z ) are in
Period 3 of the Periodic Table. Element ( Y )
has the highest first ionisation energy and the lowest melting point of these three elements.

What are the identities of ( X, Y ) and ( Z ? )
A. Sodium, magnesium, aluminium
B. Magnesium, aluminium, silicon
c. Aluminium, silicon, phosphorus
D. silicon, phosphorous, sulfur

11
216 What is the IUPAC symbol of Rutherfordium?
A . Rt
B. Ru
c. Rf
D. Rd
11
217 has 6 valence electrons.
A. Nitrogen
B. Oxygen
c. Chlorine
D. Neon
E. Beryllium
11
218 The number of electrons having ( n+ )
( s=2.5 ) in sulphide ion is:
( A cdot 3 )
B. 4
( c cdot 6 )
D. 2
11
219 Which pair of elements of atomic numbers given below will have similar chemical properties?
( mathbf{A} cdot 13,22 )
в. 3,11
( c cdot 4,24 )
D. 2,4
11
220 Number of elements in 6 th period are:
A . 28
B. 26
( c cdot 34 )
D. 32
11
221 The ( 100^{t h} ) element is named in honor of
A. Einstein
B. Bohr
c. Fermi
D. Curie
11
222 The electronic configuration of the two
outermost shells of an atom is
( 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{2} . ) What is this atom?
A. Manganese
B. Phosphorus
c. strontium
D. Vanadium
11
223 If the two members of a Dobereiner’s
triad are chlorine and iodine, then
the third member of this triad is :
A. fluorine
B. bromine
c. sodium
D. calcium
11
224 Which of the following has the lowest ionization energy?
A ( . L i )
в. ( N a )
c. ( K )
D. ( R b )
ह. ( C s )
11
225 The maximum number of electrons
that L shell can accommodate are :
A . 4
B. 8
c. 16
D. 32
11
226 With respect to oxygen maximum valency is shown by:
A. Halogen family
B. Oxygen family
c. Nitrogen family
D. Boron family
11
227 The spectrum of helium is expected to be similar to that of :
( mathbf{A} cdot H )
в. ( B e )
( mathbf{c} cdot L i^{+} )
D. Ne
11
228 Statement: In Dobernier classification
of elements, the atomic weight of the
middle element is equal to the average of the extreme elements of a triad.
State whether the given statement is true or false.
A. True
B. False
11
229 The noble gases are nonreactive
because:
A. they react with sodium
B. they have a full outer shell of electrons
C. they have a half outer shell of neutrons
D. they are too thin
11
230 Assertion
Boron can only form ( left[boldsymbol{B} boldsymbol{F}_{4}right]^{-}, ) whereas
aluminum forms ( left[A l F_{6}right]^{3-} )
Reason
The first member of a group of elements in the ( s- ) and ( p- ) blocks shows
anomalous behavior
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
231 Dobereiner was the first person to
illustrate the relationship between the of elements and
their properties.
A. atomic masses
B. electron negativity
c. molecular masses
D. number of protons
11
232 Third period of the periodic table contains the following number elements:
( A cdot 2 )
B. 18
( c cdot 8 )
D. 32
11
233 The family of elements to which sodium belongs is :
A. alkali metalss
B. alkaline earth metals
c. halogens
D. inert gases
11
234 What is the total number of valence
electrons in the peroxydisulphate, ( S_{2} O_{8}^{2-}, ) ion ( ? )
A . 58
B. 60
( c cdot 62 )
D. 64
11
235 What name is given to the elements belonging to the third period of Mendeleev’s periodic table? 11
236 Explain why to ionize ( M g ) to ( M g^{+2} ) it
needs three times as much energy as to
form ( M g^{2+} )
11
237 Which of the following contains same number of elements?
A. 1st period and Ogroup
B. 6th period and III B group
c. 5th period and III B group
D. 3rd period and VII A group
11
238 Compare and contrast the arrangement of elements in Mendeleev’s periodic
table and the Modern periodic table.
11
239 The modern periodic table is ordered on the basis of:
A. atomic mass
B. atomic radius
c. atomic charge
D. atomic number
11
240 Which is the correct symbol for manganese?
A.
в. ма
( c . ) мп
D. Mg
11
241 Which of the following has the highest
electronegativity?
A. ( C )
в. ( M g )
( c cdot O )
D. ( S )
11
242 In Doberenier triads, the atomic weights of the elements in a triad are in
increasing order.
A. True
B. False
11
243 Which is the correct order of increasing energy of the listed orbitals in the atom
of titanium?
(At. no. ( Z=22) )
( mathbf{A} cdot 3 s 3 p 3 d 4 s )
B. 3s 3p 4s 3d
c. ( 3 s ) 4s ( 3 p 3 d )
D. ( 4 s 3 s 3 p 3 d )
11
244 Which of the following order is wrong?
( mathbf{A} cdot N H_{3}<P H_{3}<A s H_{3}: ) Acidic strength
B . ( L i<B e<B<C: I E_{1} )
c. ( A l_{2} O_{3}<M g O<N a_{2} O<K_{2} O: ) Basic strength
D ( cdot L i^{+}<N a^{+}<K^{+}<C s^{+}: ) Ionic character
11
245 Group 18 of the periodic table is known by the name as:
A . alkal
B. alkaline
c. halogen
D. noble
11
246 When the atom Li, Be, B and Na are
arranged in order of increasing atomic radius, what is the correct order?
( A cdot B, B e, ) Li, ( N a )
B. Li, Be, B Na a
c. Ве, Li, В, Na
11
247 A molecule ( boldsymbol{H}-boldsymbol{X} ) will be ( 50 % ) ionic if
electronegativity difference of ( boldsymbol{H} ) and ( boldsymbol{X} )
is:
A . 1.2 ev
B. ( 1.4 mathrm{eV} )
c. ( 1.5 mathrm{ev} )
D. 1.7 ev
11
248 The law used by Newland to arrange elements is known as 11
249 Multiple Answer Question Which of the following position of elements have same number of valence
electrons as that of element of atomic
number 6?
This question has multiple correct options
A. Group 14 and period 3
B. Group 14 and period 4
C. Group 6 and period 4
D. Group 14 and period 6
11
250 The most negative oxidation state of an atom of group 15 (VA) element is equal to the number of electrons required to fill the valence shell of the neutral
atom. If true enter 1 ,if false enter 0
11
251 Dobereiner grouped the elements into triads and Newland gave the:
A. law of Octaves
B. mass number
c. atomic number
D. valency
11
252 State True or False.
IUPAC representation of atomic number
108 is ( boldsymbol{U} boldsymbol{n} boldsymbol{o} )
A. True
B. False
11
253 State the electronic configuration for Neon ( [p=10, n=10] )
A. 2,6
в. 2,
c. 2,9
D. 2, 8
11
254 Q9. What are representative elements? 11
255 B and Si resemble each other in their
properties. If true enter 1 , else enter 0
11
256 The plot of ( sqrt{boldsymbol{v}} ) vs ( mathbf{Z}, ) where ( boldsymbol{v} ) is frequency and ( z ) is atomic number, is :
A. a straight line
B. an exponential curve
c. a hyperbolic
D. a curve with – ve slope
11
257 The position of three elements ( A, B ) and
( mathrm{C} ) in the Periodic Table are shown below-
Group 16
( B )
( begin{array}{ll}6 & text { Group17 } \ & \ & mathrm{A} \ & \ & \ & mathrm{C}end{array} )
(a) State whether A is a metal or non-
metal.
(b) State whether ( C ) is more reactive or
less reactive than ( mathbf{A} )
(c) Will ( C ) be larger or smaller in size than B?
(d) Which type of ion, cation or anion, will be formed by element A?
11
258 If three elements ( X, Y, ) and ( Z ) form a Dobereiner’s triad and atomic weights of ( X ) and ( Z ) are 9 and 40 respectively
then the atomic weight of the element ( Y ) is approximately:
A . 24.
B. 49
c. 34.5
D. 29
11
259 Which of the following would be different in a ground state and in excited state of neon atom?
A. The number of neutrons
B. The number of electrons
c. The atomic weight
D. The electronic configuration
E. Everything would remain the same
11
260 Atomic number of ( S c^{3+}(18 e) )
is
11
261 Which of the following statement(s) is
(are) true?
This question has multiple correct options
A ( cdot ) Ionisation energy ( alpha frac{1}{text { Screening effect }} )
B. The first ionization energies of Be and Mg are more than ionization energies of ( B ) and ( A I ) respectively.
C. Atomic and ionic radii of Niobium and Tantalum are
almost same.
D. Metallic and covalent radii of potassium are ( 2.3 A^{circ} )
and ( 2.03 A^{circ} ) respectively.
11
262 Atomic number 112 placed in:
A. s- block
B. d- block
c. f- block
D. p- block
11
263 What is the atomic number of the
element with symbol Uus?
A . 117
B. 116
c. 115
D. 114
11
264 First transitional series is present in:
A. third period
B. fifth period
c. fourth period
D. sixth period
11
265 An element with atomic number 21 is
a/an:
A. Halogen
B. Representative element
c. Transition element
D. Alkali metal
11
266 that of Li (lithium).
Q32. Predict the formulas of the stable binary compounds that would be formed by the combination
of the following pairs of elements:
(a) Lithium and oxygen
(b) Magnesium and nitrogen
(c) Aluminium and iodine
(d) Silicon and oxygen
(e) Phosphorous and fluorine
(0) Element 71 and fluorine.
11
267 How many periods are there in the long form of the periodic table?
A. 6
B. 7
( c cdot 8 )
( D )
11
268 The ionization energy of a hydrogen-like atom is 9 Rydberg. The radius of first orbit of this atom, as compared to the radius of first orbit of hydrogen atom, will be
A. One-fourth
B. Half
c. One-third
D. Three times
11
269 Zero group was introduced by :
A. Lother Meyer
B. Mendeleev
c. Ramsay
D. Lockyer
11
270 Two atoms of similar electronegativity would be expected to form a covalent compound if true enter 1 else 0 11
271 Which of the following sets of elements has strongest tendency to form anions?
A. ( A s, S e, B r )
в. ( P, S, C l )
c. ( N, O, F )
D. ( S b, T e, I )
11
272 Define: Atomic radius, lonic radius, lonisation Enthalpy, Electron Gain enthalpy, Electronegativity. 11
273 How many vertical columns are there in
the modern periodic table and what are they called?
11
274 The group of the element with electronic configurations: ( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} ) is
2. If true enter 1 , else enter 0 .
11
275 The resistance of ( 1 mathrm{N} ) solution of acetic
acid is ( 250 Omega ) when measured in a cell
having a cell constant of ( 1.15 mathrm{cm}^{-1} . ) The
equivalent conduction (in oh ( m^{-1} c m^{2} e q u i v^{-1} ) ) of ( 1 N ) acetic acid is
A . 2.3
B. 4.6
c. 9.2
D. 18.4
11
276 Give the number of periods and groups in Modern Periodic Table. 11
277 The atomicity of neon gas is :
A . two
B. one
c. four
D. three
11
278 Select the correct order of
electronegativity:
A ( . F>C l>B r>I )
B. ( N>P>A s )
( c . ) both (a) and (b)
( D S>O>S e )
11
279 The general name of the elements of
17th group are:
A. hydrides
B. halogens
c. chacogens
D. noble gases
11
280 Mendeleev arranged the elements in increasing order of their atomic masses and according to their physical properties.
A. True
B. False
11
281 If an element A is present in group I of the periodic table, the formula of its chloride should be:
A ( cdot A_{2} C l )
в. ( A C l_{2} )
c. ( A C l )
D. ( A C l_{3} )
11
282 As we move from left to right in a period, which of the periodic properties decreases?

This question has multiple correct options
A. electronegativity
B. atomic size
c. electropositivity
D. metallic character

11
283 The energy required to convert all atoms
presents in ( 1.2 g ) magnesium to ( M g^{2+} )
ions if ( I E . ) and ( I E_{2} ) of magnesium are ( 120 mathrm{kJ} ) mol ( ^{-1} ) and ( 240 mathrm{kJ} ) mol( ^{-1} )
respectively:
A. ( 18 mathrm{kJ} )
J
в. 36 к
c. 360 k.
D. 24 kJ
11
284 Increasing order of density: ( N a<A l< )
( boldsymbol{F} boldsymbol{e}<boldsymbol{P} boldsymbol{b} )
if true enter 1 , else enter 0 .
( A cdot 1 )
11
285 Which of the following pair of atomic numbers represents s-block elements?
A .7,15
B. 6,12
( mathrm{c} .9,17 )
D. 3,12
11
286 Which of the following element belongs to the halogen group? This question has multiple correct options
A ( cdot 1 s^{2}, 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5} )
B . ( 1 s^{2}, 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}, 4 s^{2} )
C ( cdot[A r] 3 d^{10}, 4 s^{2} 4 p^{5} )
D . ( [K r] 4 d^{10}, 5 s^{2} 5 p^{5} )
11
287 An element ( M ) has an atomic number 9
and atomic mass ( 19 . ) Its negative ion will be represented by:
( mathbf{A} cdot M )
В. ( M^{2} )
( c cdot M^{-} )
D. ( M^{2} )
11
288 System indicated in parentheses by Roman numerals. to name compounds is called as:
A . periodic table
B. stock nomenclature
c. roman nomenclature
D. all of the above
11
289 Which of the following configurations has the highest ionization energy?
A ( cdot 1 s^{2} 2 s^{2} 2 p^{1} )
B ( cdot 1 s^{2} 2 s^{2} 2 p^{3} )
C ( cdot 1 s^{2} 2 s^{2} 2 p^{2} )
D. ( 1 s^{2} 2 s^{2} 2 p^{4} )
11
290 The elements ( (z=117 text { and } 120) ) have
not yet been discovered in which family or group would you place these elements and also give electronic
configuration in each case?
11
291 The electronic configuration of the element with maximum electron
affinity is :
A ( cdot 1 s^{2}, 2 s^{2} 2 p^{3} )
B . ( 1 s^{2}, 2 s^{2} 2 p^{5} )
C. ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{5} )
D. ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{3} )
11
292 The number of water molecules in
hydrated beryllium salt never exceeds:
A. 6
B. 3
( c cdot 2 )
( D )
11
293 Alkali and alkaline earth metals are
elements.
A. same
B. different
c. both A and B
D. none of these
11
294 The ( I_{1}, I_{2}, I_{3}, I_{4} ) values of an element ( M )
are ( 120 mathrm{kJ} / mathrm{mole}, 600 mathrm{kJ} / mathrm{mole}, 1000 )
kJ/mole and ( 8000 mathrm{kJ} / ) mole. Then the
formula of its sulphate is:
A. ( M S O_{4} )
в. ( M_{2}left(S O_{4}right)_{3} )
( mathrm{c} cdot M_{2} mathrm{SO}_{4} )
D. ( M_{3}left(S O_{4}right)_{2} )
11
295 08. What are Dobereiner’s triads? Name two such triads. 11
296 If electronegativity values of element ( boldsymbol{X} )
and ( Y ) are 3.8 and 1.8 respectively, then
an ionic percentage of compound ( boldsymbol{X} boldsymbol{Y} ) is:
A . 50
B. 46
( c cdot 64 )
D. 36
11
297 Eka-aluminium forms oxide of the type :
( A cdot E_{2} O )
B. ( E O )
( mathrm{c} cdot E_{2} mathrm{O}_{3} )
D. ( E_{3} O_{4} )
11
298 Which one of ( mathrm{K}, mathrm{I}, mathrm{Cl} ) and ( mathrm{Li} ) Will display the highest first ionisation energy?
( A cdot K )
B.
c. ( c )
D. L
11
299 Identify the property which does not reflect the periodicity of the elements.
A. Bonding behaviour
B. Electronegativity
c. lonization potential
D. Neutron-proton ratio
11
300 The electronic configuration of calcium
is ( 2,8,8,2 . ) Find the valency of the element?
A . 1
B . 2
( c .3 )
D.
11
301 Q8. Which has a larger radius?
(i) Mg or Ca (ii) S or Cl
11
302 Electronic configuration of Mg is:
( mathbf{A} cdot 1 s^{2} 2 s^{1} p^{5} 3 s^{2} 3 d^{2} )
B. ( 1 s^{2} 2 s^{2} p^{6} 3 s^{2} )
C ( cdot 1 s^{2} 2 s^{2} p^{7} 3 s^{1} )
D. ( 1 s^{2} 2 s^{2} p^{6} 3 s^{2} p^{2} )
11
303 Recently discovered element with atomic number 115 is:
A. Uun
в. ( U u b )
c. ( U u p )
D. Uus
11
304 Two metals ( M ) and ( N ) have the following values of ionization energies. Find
energy required for formation of ( boldsymbol{M}^{+} )
from ( M, M^{+2} ) from ( M^{+}, ) and total
energy required to form ( M^{+2} ) from ( M )
Do similar calculations for metal ( N )
( I E_{1} quad I E_{2} )
[
496 quad 4560
]
738 1450
11
305 Q35. Anything that influences the valence electrons will affect the chemistry of the element. Which
one of the following factors does not affect the valence shell?
(a) Valence principal quantum number (n)
(b) Nuclear charge (Z)
(c) Nuclear mass
(d) Number of core electrons.
11
306 Q.54 In what manner is the long from of periodic table better than
Mendeleef’s periodic table? Explain with examples.
11
307 Which has the lowest anion to cation
size ratio?
A . ( L i F )
В. ( N a F )
c. ( C s I )
D. ( C s F )
11
308 Which of the following options are incorrect?
A. Decreasing ( I . E_{2}: F>N>0 )
B. Increasing atomic size : Be < B < Li < Na a
c. Metallic bond strength: Na < Zn < Ca
D. Increasing electron affinity : ( O^{2-}<O^{-}<O^{+}<O )
11
309 Which periods were not divided into two series in the Mendeleev’s periodic
table?
A .4
B. 5
( c .6 )
D. None of the above
11
310 Q. 21 Which of the following have no unit?
(a) Electronegativity
(b) Electron gain enthalpy
(c) lonisation enthalpy
(d) Metallic character
11
311 A particular atom has the 4 th shell as its valence shell. If the difference
between the number of electrons
between K and N shell and L and M shell
is zero, find the electronic configuration of its stable ion.
A. 2,8,8,2
B. 2, 8, 18,8
c. 2,8,8
D. 2, 8
11
312 The formulae of chloride of metal ( M ) is
( M C l_{2} . ) The metal ( M ) belongs to
group.
11
313 3. Which of the following is arranged in order of increasing radius?
(a) K (aq) < Na+ (aq)
  • Na (aq) > Zn2+ (aq)
    (c) K+ (aq) > Li* (aq) > Na (aq) (d) Lit (aq) < Nat (aq) <K+ (aq)
    a) Lit can nama
  • 11
    314 Dobereiner was able to identify triads from the elements
    known at that time.
    11
    315 A quantity of 15.8 g of ( K M n O_{4} ) can be decolourized in acidic medium by ( (mathrm{K}= )
    ( 39, M n=55, F e=56 )
    This question has multiple correct options
    A . ( 18.25 mathrm{g} ) HCll
    B . ( 22.5 g H_{2} C_{2} O_{4} )
    c. ( 32 g S O_{4} )
    ( mathrm{D} cdot 38 mathrm{g} mathrm{FeSO}_{4} )
    11
    316 Which one of the following electronic configuration corresponds to the element with maximum electopositive
    character?
    A ( cdot[K r] 5 s^{1} )
    в. ( [N e] 3 s^{1} )
    c. ( [A r] 4 s^{1} )
    D. ( [X e] 6 s^{1} )
    11
    317 In Newland’s classification, elements are arranged in an increasing order of their:
    A. mass number
    B. atomic number
    c. atomic weight
    D. all of these
    11
    318 Elements ( A, B ) and ( C ) belong to the same period in the long form of the periodic table. The nature of the oxides of ( A, B )
    and ( mathrm{C} ) is amphoteric, basic and acidic respectively. The correct order of the
    atomic numbers of these elements is:
    A. ( C>B>A )
    в. ( C>A>B )
    c. ( A>B>C )
    D. ( B>A>C )
    11
    319 The properties that have increasing values with increase in atomic number
    for the elements of 1A are?
    I. Ionization energy (potential)
    I. Atomic radius
    III. Atomic mass
    A. I only
    B. III only
    c. I and II only
    D. Il and III only
    E . ।, ॥।, and III
    11
    320 Number of unpaired electrons in inert gas is:
    A. 0
    B. 8
    ( c cdot 4 )
    D. 18
    11
    321 Which of the following statement is
    false?
    A. Elements of ( n s^{2} n p^{6} ) electronic configuration lies in ( 1^{s t} ) to ( 6^{t h} ) period
    B. Typical elements lies in ( 3^{r d} ) period
    C. The seventh period will accommodate thirty two elements
    D. Boron and silicon are diagonally related
    11
    322 Q8. Why do elements in the same group have similar physical and chemical properties? 11
    323 When a Dobereiner triad is considered,
    the sum of atomic weights of extreme elements ( X ) and ( Z ) is 177.6 and difference
    of ( Z ) and ( Y ) is five times the number of
    protons present in a neon atom. Identify ( x, Y ) and ( z )
    ( mathbf{A} cdot X rightarrow C a, Y rightarrow S r, Z rightarrow B a )
    в. ( X rightarrow L i, Y rightarrow N a, Z rightarrow K )
    c. ( X rightarrow K, Y rightarrow R b, Z rightarrow C s )
    D. ( X rightarrow S r, Y rightarrow B a, Z rightarrow R a )
    11
    324 Identify the factor that distinguishes each element from every other element in the periodic table ?
    A. The number of protons in the nucleus
    B. The number of neutrons in the nucleus
    c. The number of electrons about the nucleus
    D. The total mass of the nucleus (protons plus neutrons)
    E. Its position in the periodic table
    11
    325 Which of the following elements are metals?
    This question has multiple correct options
    A. Calcium
    B. Chlorine
    c. Potassium
    D. Sulphur
    11
    326 If the valence electron configuration of this element is ( x s^{2} 6 f^{y} ) and ( 7 d^{z}, ) then find out the value of ( x, y ) and ( z )
    A. ( x=8, y=14, z=10 )
    B . ( x=7, y=12, z=10 )
    c. ( x=9, y=10, z=10 )
    D. None of the above
    11
    327 Element with similar chemical
    properties:
    A. occur only within the same period
    B. have identical atomic mass(weight)
    C. have identical number of neutrons
    D. have the same number of electrons in the outer shell
    11
    328 What is the valency of magnesium with atomic number ( 12 ? )
    A . 2
    B. 4
    c. 5
    ( D )
    11
    329 ( mathrm{Cl}, mathrm{Br}, mathrm{I} ) follows Dobereiner’s triads, the atomic masses of ( mathrm{Cl} ) and I are 35.5 and
    127 respectively. The atomic mass of Br is :
    A . 162.5
    B. 91.5
    c. 81.25
    D. 45.625
    11
    330 ( M g ) forms ( M g(I I), ) because of:
    A. The oxidation state of ( M g ) is +2
    B. Difference between ( I . P_{1} ) and ( I . P_{2} ) is greater than 16.0 ( e v )
    c. There are only two electrons in the outermost energy level of ( M g )
    D. Difference between ( I . P_{1} ) and ( I . P_{2} ) is less than 11 ev
    11
    331 Q. 1 Consider the isoelectronic species, Na+, Mg2+, F and 02. The correct
    order of increasing length of their radii is
    (a) F <0 < Mg2+ < Na+ (b) Mg2+ < Na+ <F <02-
    (c) O2- <F < Na+ < Mg2+ (d) O2- < < Mg2+ < Nat
    11
    332 An element ( X ) (atomic number 17 ) reacts
    with an element Y (atomic number 12)
    to form a divalent halide. Where do ( x )
    and Y are placed in the modern periodic table? (mention the group and period of each
    11
    333 All elements of the same group will
    have:
    A. same electronic configuration
    B. similar outer electron configuration
    C. same ionization potential value
    D. different chemical properties
    11
    334 Electronic configurations of few
    elements are given below. Mark the
    incorrect match.
    A ( cdot l s^{2} 2 s^{2} 2 p^{5} ) – Most electronegative element
    B. ( l s^{2} 2 s^{2} 2 p^{3}- ) An element belonging to 3rd period and 5 th
    group
    C ( cdot 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{8} 4 s^{2}- ) A d-block element
    D. ( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} ) – An element from 18th group
    11
    335 An element has six electrons in its
    outermost shell, then its valency can be
    ( A cdot 6 )
    B. 2
    ( c cdot 4 )
    D. All of the above
    11
    336 The element with ( Z=120 ) (not yet discovered) will be an/ a:
    A. transition metal
    B. inner-transition metal
    c. alkaline earth metal
    D. alkali metal
    11
    337 Q26. What are major differences between metals and non-metals? 11
    338 Which of the following is a transition element?
    A. Element with atomic number 2
    B. Element with atomic number 7
    c. Element with atomic number 19
    D. Element with atomic number 35
    E. Element with atomic number 74
    11
    339 The term periodicity is the properties of elements, which are arranged in the increasing order of their atomic numbers. Then the elements
    with similar properties:
    A. reoccur after a fixed interval
    B. reoccur after certain regular interval
    c. form vertical groups
    D. form horizontal rows
    11
    340 State Newland’s law of octaves. 11
    341 In laboratory burners, we use
    A. Producer gas
    B. oil gas
    c. Gobar Gas
    D. None of the above
    11
    342 How do the following properties vary in a Period and in a Group?
    (A) Atomic radius
    (B) Ionization energy
    (C) Electronegativity
    (D) Electropositivity
    11
    343 Which of the following is the most chemically reactive?
    A ( . L i )
    в. ( N a )
    c. ( K )
    D. ( R b )
    ह. ( C s )
    11
    344 All halogens are:
    A. s-block elements
    B. d-block elements
    C . representative elements
    D. transition elements
    11
    345 Ratio of radii of ( mathrm{K}, mathrm{L}, mathrm{M} ) shells of hydrogen atom is :
    A. 1: 2: 3
    B . ( 1: frac{1}{4}: frac{1}{9} )
    c. 1: 4: 9
    D. ( 1: frac{1}{2}: frac{1}{3} )
    11
    346 Which of the following has the largest radius?
    A ( . S r )
    в. ( P )
    c. ( M g )
    D. ( A l^{3} )
    E ( . M g^{2+} )
    11
    347 Q13. Explain why cation are smaller and anions larger in radii than their parent atoms?
    ILOV
    LI
    11
    348 Sodium has
    compared to potassium.
    A. less electronegativity
    B. more ionization potential
    c. larger atomic radius
    D. lower melting point
    11
    349 In which of the following reaction, Boron does not act as reducing agent?
    A. ( B+C O_{2} rightarrow )
    в. ( B+M g rightarrow )
    c. ( B+S i O_{2} rightarrow )
    D. ( B+H N O_{3} rightarrow )
    11
    350 Name the anomalous pairs 11
    351 Which element has least atomic
    diameter?
    A. ( F )
    в. ( F e )
    ( c cdot C l_{2} )
    D. ( N a )
    11
    352 Statement ( I- ) Zinc and berylium have
    electron affinities which are
    significantly different from each other.
    Statement ( I I- ) Electron affinity is a
    measure of the energy used to add an
    electron to an atom.
    A. Statement ( I ) is true, Statement ( I I ) is true
    B. Statement I is true, Statement II is false
    c. statement ( I ) is false, statement ( I I ) is true
    D. Statement I is false, Statement ( I I ) is false
    E. Statement I is true, Statement ( I I ) is true and is a correct explanation of the phenomena described in 1
    11
    353 The electropositive character is the maximum for which of the following elements in Group 13?
    A ( cdot ) Al
    в. T
    c. Both of the above
    D. None of the above
    11
    354 Identify the electronic configuration of an element whose atomic radii is determined by taking half the internuclear distance between like
    atoms.
    ( mathbf{A} cdot[H e] 2 s^{2} 2 p^{5} )
    B . ( [A r] 4 s^{2} )
    c. ( [N e] 3 s^{2} )
    D ( cdot[K r] 4 d^{5} 5 s^{2} )
    11
    355 In a group from top to bottom, ionisation energy
    A. increases
    B. decreases
    c. remains same
    D. none of these
    11
    356 Assertion
    Tin exhibits +2 and +4 oxidation
    states only and not +3 oxidation state.
    Reason
    Inert pair effect of electrons in the sorbital is responsible.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    357 State True or False.
    The atomic number of Uus is 117
    11
    358 Pair having elements from same period
    is :
    A . Na,Ca
    B. Na,CI
    c. са,С
    D. Cl,Br
    11
    359 The electronegativity of elements below sodium in the same group will be :
    A. lower
    B. higher
    c. same
    D. none of these
    11
    360 What do oxygen atom and oxide ion have in common?
    A. Same size
    B. Same number of electrons
    c. Same electronic configuration
    D. Same number of protons
    11
    361 The element in between lithium and
    potassium in Dobereiner’s classification is:
    A . Mg
    B. Na
    ( c cdot c a )
    D. Rb
    11
    362 Which is non-metal (excluding noble
    gas)?
    A.
    B. ( Q )
    ( c cdot R )
    ( D )
    11
    363 A metal that forms a stable binary
    halide of formula ( A X_{2}(X= ) Halogen) is :
    ( A )
    B. 2
    ( c cdot 3 )
    D.
    11
    364 In terms of polar character which one of
    the following orders is correct?
    ( mathbf{A} cdot H_{2} S<N H_{3}<H_{2} O<H F )
    B. ( H_{2} S<N H_{3}<H_{2} SH_{2} O<N H_{3}<H_{2} S )
    ( mathbf{D} cdot N H_{3}<H_{2} O<H F<H_{2} S )
    11
    365 In the following four elements, the
    ionisation potential of which one is the highest?
    A. Oxygen
    B. Argon
    c. Barium
    D. cesium
    11
    366 Which one of the following pairs of atomic numbers represents elements belonging to the same group?
    A. 11 and 20
    B. 13 and 30
    c. 13 and 31
    D. 14 and 31
    11
    367 Read below given tabular form and
    answer the questions.
    begin{tabular}{llll}
    Element & Electronic configuration & Element & Elec conf \
    ( mathrm{He} ) & ( 1 s^{2} ) & ( mathrm{Kr} ) & ( 4 s^{2} 4 ) \
    ( mathrm{Ne} ) & ( 2 s^{2} 2 p^{6} ) & ( mathrm{xe} ) & ( 5 s^{2} 5 ) \
    ( mathrm{Ar} ) & ( 3 s^{2} 3 p^{6} ) & ( mathrm{Rn} ) & ( 6 s^{2} 6 ) \
    hline
    end{tabular}
    Write the names of ‘noble gas’ elements
    11
    368 1) On the Pauling’s electronegativity
    scale,which element is next to ( F )
    2) Why ( C a^{2+} ) has smaller ionic radius
    ( operatorname{than} boldsymbol{K}^{+} ? )
    11
    369 How does number of valence electrons
    vary on moving from left to right In the first period of a periodic table?
    A .
    в.
    ( c cdot 2 )
    D.
    11
    370 lonization potential of ( N a ) would be
    numerically the same as:
    A. electron affiniy of ( N a^{+} )
    B. electronegativity of ( N a^{+} )
    c. electron affiniy of ( H e )
    D. ionization potential of ( M g )
    11
    371 The metal showing resemblance with lithium is
    ( A . B e )
    в. ( M g )
    c. ( A l )
    D. ( C a )
    11
    372 Which of the following is true about Mendeleev’s Periodic Table?
    A. Systematic study of elements
    B. Prediction of new elements
    c. correction of doubtful atomic weights
    D. All of the above
    11
    373 Identify less reactive element from the following:
    ( mathbf{A} cdot_{8} Y^{16} )
    B. ( _{10} Y^{20} )
    C. ( _{11} Y^{23} )
    D. ( _{9} Y^{19} )
    11
    374 The anomalous pairs in Mendeleev’s periodic table is/are
    ( A cdot C o, N i )
    в. Te,
    c. Ar, ( k )
    D. All the above
    11
    375 Identify the odd one out:
    Barium, Radium, Calcium, Francium
    11
    376 Which of the following elements will form acidic oxide?
    This question has multiple correct options
    A. Na a
    в. ( s )
    ( c . ) мв
    D. P
    11
    377 Arrange the elements
    ( F, N a, F e, C l, N e ) in increasing order
    of ionization energy.
    A. ( N a<F e<C l<FF>C l>F e>N a )
    c. ( F e>C l>F>N e>N a )
    11
    378 Q6. Define the term ionization enthalpy? How does it vary along a period and along a group 11
    379 Mendeleev’s classified elements in:
    A. Increasing order of atomic number
    B. Increasing order of atomic masses
    C. Decreasing order of atomic masses
    D. Decreasing order of atomic number
    11
    380 Assertion
    According to Mendeleev’s periodic law;
    The properties of elements are the
    periodic a function of their atomic
    numbers.
    Reason
    Mendeleev’s periodic law could explain
    the phenomenon of anomalous pairs.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is correct but Reason is incorrect
    D. Both Assertion and Reason are incorrect
    11
    381 Classification of elements are done on
    the basis of
    A. atomic number
    B. atomic weight
    c. valency
    D. none of these
    11
    382 Which of the following is the correct electronic configuration of potassium?
    A .2,8,9
    B. 8,2,9
    c. 2,8,8,1
    D. 1, 2,8, 8
    11
    383 Correct order of ( 1^{s t} ) IP among following elements Be, B, C, N, O is:
    ( A cdot B<B e<C<0<N )
    B. ( B<B e<C<N<0 )
    ( c cdot B e<B<C<N<0 )
    ( D cdot B e<B<C<0<N )
    11
    384 Which of the following explains the
    reason why atomic radii decrease
    across a period?
    A. As you move across the period, the number of protons increases, which increases the nuclear charge. The number of electrons remains the same creating a larger Coulombic attraction and decreasing the radii
    B. As you move across the period, the number of protons and electrons increases. The increased Coulombic attraction decreases the overall size of the atom.
    C. As you move across the period, the number of protons remains constant while the number of electrons
    increases. The decreased Coulombic attraction
    decreases the overall size of the atom.
    D. The atomic radii do not decrease across a period. It actually increases, duh!
    11
    385 In group I of alkali metals, the ionization potential decreases down the
    group. Therefore lithium is a poor
    reducing agent in gaseous state.
    A. True
    B. False
    11
    386 As atomic radii increases, ionisation
    potential:
    A. increases
    B. decreases
    c. remains same
    D. none of the above
    11
    387 Oxygen and sulphur are identical in
    respect of :
    A. chemical properties
    B. distribution of electrons in outer shell
    c. atomicity
    D. electronic configuration
    11
    388 Elements in the same column/group of the periodic table have similar chemical properties because their atoms have the same
    A. number of protons
    B. number electrons
    c. number of valence electrons
    D. atomic mass
    11
    389 Which element reacts most explosively in water?
    ( mathbf{A} cdot K )
    в. ( C a )
    ( c cdot B r )
    D. ( K r )
    E. ( Z n )
    11
    390 Which of the following elements follow Dobereiner’s law of Triads?
    A. ( mathrm{Na}=23, mathrm{Li}=7 ) and ( mathrm{K}=39 )
    B. Cl = ( 35, mathrm{Br}=80 ) and ( mathrm{F}=19 )
    c. ( mathrm{ca}=40, mathrm{Mg}=24 ) and ( mathrm{Sr}=88 )
    D. ( mathrm{Na}=23, mathrm{K}=39 ) and ( mathrm{Rb}=85 )
    11
    391 The elements of one period are given below in order from left to right
    ( boldsymbol{L} boldsymbol{i}, boldsymbol{B} boldsymbol{e}, boldsymbol{B}, boldsymbol{C}, boldsymbol{O}, boldsymbol{F}, boldsymbol{N} boldsymbol{e} )
    Which one of the above elements
    belongs to the halogen series?
    ( mathbf{A} cdot L i )
    B. ( O )
    ( c . F )
    D. Ne
    11
    392 Why is electronegativity directly
    proportional to ( s ) character?
    11
    393 The main reason for showing anomalous properties of the first
    member of a group in s or p-block is :
    A. maximum chemical reactivity
    B. maximum electronegativity and different configurations
    c. small size, large charge, /radius ratio
    D. tendency to form multiple bonds
    11
    394 Few values are given in the table in the
    direction from left to right and top to
    bottom. Predict the property which
    could be depicted in the table.
    A. Atomic number
    B. Ionisation enthalpy
    c. Atomic radius
    D. Electron gain enthalpy
    11
    395 Which of the following statements is/are wrong?
    I) ( B i^{3+} ) is more stable than ( B i^{5+} )
    II) ( M n ) shows +8 oxidation state.
    III) The oxidation state of an element is
    always less than or equal to its group number.
    IV) ( s- ) Block elements show variable
    oxidation states.
    A. Il and IV
    c. ।, ॥ and III
    D. II, III and IV
    11
    396 The physical properties of elements changes according
    to
    A. classification of elements in groups and periods
    B. classification of elements in groups
    c. classification of elements in periods
    D. None of these
    11
    397 Newland could classify elements only
    upto:
    A. copper
    B. chlorine
    c. calcium
    D. chromium
    11
    398 The given arranged sequence on the basis of their increasing atomic masses represents which law of classification of elements?
    ( boldsymbol{F}, boldsymbol{N} boldsymbol{a}, boldsymbol{M} boldsymbol{g}, boldsymbol{A l}, boldsymbol{S} boldsymbol{i}, boldsymbol{P}, boldsymbol{S}, boldsymbol{C l} & boldsymbol{K} )
    A. Modern table
    B. Newton’s law
    c. Newland’s law of octaves
    D. Mendeleev’s periodic table
    11
    399 If the valence shell electronic
    configuration for an element is ( n s^{2} n p^{5} ) this element belongs to the group of
    A. alkali metals
    B. inert metals
    c. noble gases
    D. halogens
    11
    400 Why do third period elements expand
    their coalence above four?
    11
    401 John Newlands arranged the known elements in a/an order of
    their atomic
    A. increasing, masses
    B. decreasing, masses
    c. increasing, numbers
    D. decreasing, numbers
    11
    402 The electronic configuration of ( boldsymbol{R} boldsymbol{b}^{+} ) in absence of Aufbau Principle, is:
    A ( cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{10}, 4 s^{2} 4 p^{6} )
    B ( cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{3} 3 p^{6} 3 d^{10}, 4 s^{2} 4 p^{4} )
    c. ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{10}, 4 s^{2} 4 p^{3} )
    D. None of these
    11
    403 What is the correct name of ( C l O_{2} ? )
    A. Chlorine dioxide
    B. Chlorine (II) oxide
    c. Chlorine oxide
    D. Monochlorine dioxide
    E. Chlorine dioxygen
    11
    404 The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species,
    ( mathrm{K}^{+}, mathrm{Ca}^{2+}, mathrm{Mg}^{2+}, mathrm{Be}^{2+} ? )
    ( A cdot M g^{2+}<B e^{2+}<K^{+}<C a^{2+} )
    B. ( B e^{2+}<K^{+}<C a^{2+}<M g^{2} )
    C ( cdot mathrm{k}^{+}<mathrm{Ca}^{2+}<mathrm{Mg}^{2+}<mathrm{Be}^{2+} )
    D. ( mathrm{Ca}^{2+}<mathrm{Mg}^{2+}<mathrm{Be}^{2+}<mathrm{K}^{+} )
    11
    405 ( mathbf{a} )
    b
    ( d )
    As
    ( mathrm{Sn} )
    ( e ) Te What are a, b, c, d and e in the given
    figure ?
    ( A cdot a=S i b=P c=S d=G e e=S b )
    ( B cdot a=sin b=P c=S d=S b e=G e )
    ( mathbf{C} cdot a=mathrm{Si} mathrm{b}=mathrm{P} mathrm{c}=mathrm{Sb} mathrm{d}=mathrm{S} mathrm{e}=mathrm{Ge} )
    D. ( a=P b=S c=S i d=G e e=S b )
    11
    406 The set representing the correct order of first ionization potential is :
    ( A cdot K>N a>L i )
    в. ( mathrm{Mg}>mathrm{Be}>mathrm{Ca} )
    C. ( B>C>N )
    D. ( S c>Y>L a )
    11
    407 Which group of elements could be placed in Mendeleev’s Periodic Table
    without disturbing the original order?
    A . Alkali metals
    B. Alkaline earth metals
    c. Non – metals
    D. Noble gases
    11
    408 Arrange ( s, p ) and ( d ) sub-shells of a shell in the increasing order to effective
    nuclear charge ( left(Z_{e f f}right) ) experienced by the electron present in them.
    ( A cdot s>p>d )
    B. p>s>dd
    ( c cdot d>p>s )
    D. none of the above
    11
    409 Noble gases do not react because they have electrons in their
    valence shell.
    ( A cdot 3 )
    B. 6
    ( c )
    D. 8
    11
    410 Q. 28 Among the elements B, AL, C and Si,
    (a) which element has the highest first ionisation enthalpy?
    (b) which element has the most metallic character?
    Justify your answer in each case.
    11
    411 The properties which are not common to
    both groups 1 and 17 elements in the
    periodic table are:
    A. electropositive character increases down the groups
    B. reactivity decreases from top to bottom in these groups
    c. atomic radii increases as the atomic number increases
    D. electronegativity decreases on moving down group
    11
    412 Which of the following sets of atomic masses do not correspond to Dobereiner’s triad?
    This question has multiple correct options
    A. 7,23,39
    B. 20, 38, 56
    c. 47,91,178
    D. 54, 95, 183
    11
    413 The elements of groups, 1,2,13,14,15,16 and 17 are collectively called:
    A. Noble gases
    B. Representative or normal elements
    c. Transition elements
    D. Inner transition elements
    11
    414 The total number of elements present in 6th period are:
    ( A cdot 18 )
    B. 31
    c. 32
    D. 17
    11
    415 Assertion
    ( P b I_{4} ) doesn’t exist and converts into
    ( P b I_{2} ) and ( I_{2} ) spontaneously at room
    temperature but ( P b C l_{4} ) needs heating
    to convert into ( P b C l_{2} ) and ( C l_{2} )
    Reason
    ( P b^{2+} ) is more stable than ( P b^{4+} ) due to
    inert pair effect.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion.
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion.
    C. Assertion is correct but Reason is incorrect.
    D. Assertion is correct but Reason is not correct.
    11
    416 Which of the following is not correct statement for periodic classification of elements?
    A. The properties of elements are the periodic functions of their atomic number
    B. Non-metallic elements are less in number than metallic elements
    c. For transition elements, the last electron enters into (n
    – 2) d-subshell
    D. None of these
    11
    417 Why did Mendeleev’s leave some gaps in his periodic table of elements? 11
    418 is the electronic
    configuration of the highest electronegative element.
    11
    419 Write the periodic properties which always increases along the periodic table in moving from left to right? 11
    420 ( 25 mathrm{cm}^{3} ) of oxalic acid completely neutralise 0.064 g of sodium hydroxide. Molarity of the oxalic acid solution is
    A .0 .064
    B. 0.045
    begin{tabular}{l}
    c. 0.015 \
    hline
    end{tabular}
    D. 0.032
    11
    421 The electronegativity of fluorine
    obtained from the following data is ( x ) ( boldsymbol{E}_{boldsymbol{H}-boldsymbol{H}}=mathbf{1 0 4} . boldsymbol{2} boldsymbol{k} boldsymbol{c} boldsymbol{n} boldsymbol{m} boldsymbol{l}^{-1} )
    ( boldsymbol{E}_{boldsymbol{F}-boldsymbol{F}}=mathbf{3 6 . 6} ) kcal ( boldsymbol{m o l}^{-1} )
    ( boldsymbol{E}_{boldsymbol{H}-boldsymbol{F}}=mathbf{1 3 4 . 6} boldsymbol{k c a l} boldsymbol{m o l}^{-1} )
    Electronegativity of hydrogen ( =2.1 )
    Find the value of ( x ) to the nearest
    integer.
    11
    422 The graph below shows the atomic radii
    of atoms in picometers ( (mathrm{pm}) ) as a function of atomic number.
    Which letter on this graph most closely
    shows the location of the transition
    metals of period 5?

    Atomic Radius vs. Atomic Number
    A. Region E
    B. Region D
    c. Region ( c )
    D. Region B

    11
    423 Which of the following is true about
    Mendeleev’s periodic table?
    A. The accommodation of the noble gases in the periodic table did not disturb the position of other elements
    B. Noble gases were known at the time when Mendeleev gave the periodic table
    C. When noble gases were discovered, they got a place in Mendeleev’s periodic table as a separate row
    D. All of the above
    11
    424 The element 119 has not been
    discovered. What would be the symbol for this element?
    A. ( U u e )
    в. UUe
    c. ( U U E )
    D. None of these
    11
    425 0.41 The radius of Na+ cation is less than that of Na atom. Give reason.
    Alben
    11
    426 Which of the following pair of element
    has same property? This question has multiple correct options
    A ( cdot 10,12 )
    B. 11,20
    c. 20,38
    D. 13, 31
    11
    427 ( M^{3+} ) has electronic configuration as
    ( [A r] 3 d^{10}, ) hence it lies in:
    A. ( s ) -block
    B. p-block
    c. ( d ) -block
    D. ( f ) -block
    11
    428 Law of Triad was proposed by:
    A. Newland
    B. Gay Lussac
    C . Mendeleev
    D. Dobereiner
    11
    429 What is the trick to memorize periodic
    table?
    11
    430 Elements with eight electrons in their
    outermost energy shell are called:
    A. noble gases
    B. halogens
    c. alkalis
    D. oxides
    11
    431 If screening effect is not considered,
    and thus effective nuclear charge is the atomic number then the larger radius out of ( L i, N a ) is 11
    (consider only atomic number)
    11
    432 The electronic configuration of an element is ( 2,8,8,2 . ) This element is :
    A. An alkali metal
    B. An alkaline earth metal
    c. A halogen
    D. A noble gas
    11
    433 An element ( Z ) has atomic number 16 .
    Answer the following questions on ( Z ) :
    State the formula between ( Z ) and
    Hydrogen?
    11
    434 The wavelength of a spectral line in Lyman series, when electronjumps back from 2nd orbit, is:
    в. 1216 А
    c. ( 1362 dot{h} )
    D. None of the above
    11
    435 Assertion
    Across the period effective nuclear charge decreases.
    Reason
    The third period contains only 8
    elements and not 18 like 4 th period.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is incorrect but Reason is correct
    D. Both Assertion and Reason are incorrect
    11
    436 How does tendency to lose electrons
    change in a period and why?
    11
    437 Q5. Which two elements of the following belong to the same period?
    AI, Si, Ba and O
    11
    438 in Mendeleev’s
    periodic table was not possible.
    11
    439 If ( X ) and ( Y ) are two elements which
    belong to same group of Newland’s periodic table, how many elements exists between ( X ) and ( Y ? )
    A . 4
    B. 5
    ( c cdot 6 )
    D.
    11
    440 Arrange ( F, C, O, N ) in the decreasing order electronegativity:
    A. ( O>F>N>C )
    в. ( F>N>C>0 )
    c. ( C>F>N>O )
    D. ( F>O>N>C )
    11
    441 Which compound is mainly responsible for the depletion of ozone layer?
    A. ( C O_{2} )
    в. ( C H_{4} )
    c. ( C H_{3} ) ОН
    D. ( C F_{2} C l_{2} )
    11
    442 The pair of elements having same number of valence electrons are
    This question has multiple correct options
    A. ( Z n, M g )
    в. ( C l, )
    c. ( N a, C a )
    D. ( C, G e )
    11
    443 Reactivity of elements …….. down the
    group.
    A. increases
    B. decreases
    c. increases and then decreases
    D. decreases and then increases
    11
    444 If the same element is forming oxides in different oxidation states then:
    A. that oxide will be neutral in nature in which element will be in its highest oxidation state
    B. the oxide will be highest acidic in nature in which element will be in its highest oxidation state
    c. that oxide will be amphoteric in nature in which element will be in its highest oxidation state
    D. that oxide will be highly basic in nature in which element will be in its highest oxidation state
    11
    445 What is electronegativity, and how it is related to the type of bond formed? 11
    446 Study the image above. How are the
    elements arranged in the modern
    periodic table?
    A. Elements are arranged by their atomic numbers
    B. Elements are arranged by their atomic mass
    C. Elements are arranged by their valence electron configurations.
    D. Electrons are arranged in alphabetical order
    11
    447 Why are noble gases missing from Newland’s octaves? 11
    448 The first element of group number 15 is:
    A. carbon
    B. nitrogen
    c. oxygen
    D. beryllium
    11
    449 The number of elements present in fourth period is:
    A . 32
    B. 8
    ( c cdot 18 )
    ( D )
    11
    450 The groups from ( 1^{s t} ) to ( 7^{t h} ) of
    Mendeleev’s periodic table were divided into ( _{-}-_{-}-_{-}- ) subgroups
    A .2
    B. 3
    ( c cdot 4 )
    D.
    11
    451 The electronic configuration of the
    element which is just above the
    element with atomic number 43 in the
    same periodic group is:
    ( mathbf{A} cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{5}, 4 s^{2} )
    B ( cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{5} )
    C ( cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{6}, 4 s^{1} )
    D. ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{10}, 4 s^{1} 4 p^{6} )
    11
    452 Which of the following match is correct?
    A. Mendeleev periodic table is based on number of protons
    B. One of the Doberenier’s triad is ( N a, K, R b )
    C. Newland’s octave rule is obeyed by ( H, F, C l )
    D. Lother meyer curve plotted between atomic number and atomic weight
    11
    453 Number of elements present in Period 1
    are
    ( A cdot 2 )
    B. 4
    ( c .6 )
    ( D )
    11
    454 As we move from left to right, the electronegativity increases. An atom which is highly electronegative has:
    A. large size
    B. low electron affinity
    c. high ionisation enthalpy
    D. low chemical reactivity
    11
    455 Structures of nuclei of three atoms ( A, B )
    and ( C ) are given below-
    A has 90 protons and 146 neutrons
    B has 92 protons and 146 neutrons
    C has 90 protons and 148 neutrons
    Based on the above data, which of these
    atoms are isotopes and which are
    İsobars?
    ( A cdot A ) and ( C ) are isotopes; ( B ) and ( C ) are isobars
    B. A and B are isotopes; A and C are isobars
    C. ( B ) and ( C ) are isobars; ( A ) and ( B ) are isobars
    D. ( A ) and ( C ) are isotopes; ( A ) and ( B ) are isobars
    11
    456 The name given by Newlands to the arrangement created by him was:
    A. law of octane
    B. law of octaves
    c. law of octagon
    D. law of eight elements
    11
    457 Write down the characteristics of the
    elements having atomic number 17 Electronic configuration
    Period number
    Group number
    Element family
    No. of valence electrons
    Valency
    Metal or non-metal
    11
    458 Elements of same group in the periodic table are characterised by the same:
    A. ionization potential
    B. electronegativity
    c. electron affinity
    D. number of valency electrons
    11
    459 Assertion
    In the present form of periodic table, the period number corresponds to the
    highest principal quantum number of the elements in the period.
    Reason
    Elements having similar outer electronic configurations in their atoms
    belong to same period.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is correct but Reason is incorrect
    D. Both Assertion and Reason are incorrect
    11
    460 What does ‘like dissolves like’ mean?
    A. That compounds that are from the same period on the periodic table will dissolve each other.
    B. Polar solutes dissolve in polar solvents.
    C. Nonpolar solutes dissolve in polar solvents.
    D. Polar solutes dissolve in nonpolar solvents.
    E. That compounds from the same family on the periodic table will dissolve each other.
    11
    461 The atomic number of third alkali metal
    is :
    ( mathbf{A} cdot mathbf{3} )
    B. 11
    c. 19
    D. 37
    11
    462 Give the electronic configuration of fifth element of the first transition series. 11
    463 Q. 29 Write four characteristic properties of p-block elements. 11
    464 Q.52 Write down the outermost electronic configurations of alkali metals.
    How will you justify their placement in group 1 of the periodic table?
    11
    465 0.34 p-block elements form acidic, basic and amphoteric oxides. Explain each
    property by giving two examples and also write the reactions of these
    oxides with water.
    11
    466 According to Mendeleev’s periodic law, the properties of elements are a periodic function of:
    A. atomic number
    B. atomic weight
    c. number of electrons
    D. density
    11
    467 On moving down the group from ( boldsymbol{F} ) to ( boldsymbol{I} ) which of the properties decrease? This question has multiple correct options
    A. Ionic radius
    B. Ionization energy
    c. oxidizing agent
    D. Electronegativity
    11
    468 Which of the following statements is
    incorrect about the trends in periodic
    properties in the periodic table ?
    A. Metallic character increases from Li to Cs
    B. The acidity of oxides increases from left to right in a period
    C. Noble gases have the highest electron affinity among all the elements in the periodic table
    D. Ionisation energy of aluminium is lower than that of magnesium
    11
    469 The formula of hydride of the halogen in period 3 is:
    A. ( H C l_{2} )
    в. ( H C l_{3} )
    c. ( H_{2} C l_{4} )
    D. ( H C l )
    11
    470 The total number of metals discovered
    so far are:
    ( mathbf{A} cdot 92 )
    B. 82
    c. 80
    D. 11
    11
    471 Which ranks the following atoms ( (L i, N a, K, R b) ) from the smallest to
    largest atomic radius?
    A. ( L i<N a<K<R b )
    в. ( R b<K<N a<L i )
    c. ( K<N a<L i<R b )
    D. ( N a<L i<R b<K )
    11
    472 Out of ( N a^{+}, M g^{+2}, O^{-2} ) and ( N^{-3}, ) the pair of species having the minimum and the maximum IP would be?
    A ( . N a^{+}, M g^{+2} )
    B . ( M g^{+2}, N^{-3} )
    C . ( N^{-3}, M g^{+2} )
    D. ( O^{-2}, N^{-3} )
    11
    473 Four elements ( A, B, C, D ) have 1,2,6,7
    valence electrons in their atoms.
    Assuming that they belong to the same period identify the strongest oxidizing agent among them.
    ( A cdot A )
    B. B
    ( c cdot c )
    D.
    11
    474 Lothar Meyer obtained the curve for the
    known elements by plotting their atomic volumes against:
    A. atomic numbers
    B. atomic masses
    c. densities
    D. ionization energies
    11
    475 Q. 20 In which of the following options order of arrangement does not agree
    with the variation of property indicated against it?
    (a) AP+ < Mg2+ < Na+ <F (Increasing ionic size)
    (b) B<C<N< (Increasing first ionisation enthalpy)
    (c) I< Br< Cl< F (Increasing electron gain enthalpy)
    (d) Li< Na<K< Rb (Increasing metallic radius)
    11
    476 Recently (in 2003) element with atomic
    number 110 has been named by IUPAC
    as:
    A. ( H s )
    в. ( M t )
    ( c . D s )
    D. ( S g )
    11
    477 The correct set of four quantum
    numbers for the valence electron of
    rubidium atom ( (Z=37) ) is
    ( mathbf{A} cdot+5,+1,+1 / 2 )
    В. ( 6,0,0,+1 / 2 )
    c. ( 5,0,0,+1 / 2 )
    D. None of the above
    11
    478 IUPAC representation of the element of atomic number 115 is Uup. If true enter 1 else enter 0 11
    479 When Li, Na, and K are placed in decreasing order of their ionisation
    energy, the order is :
    A . Li, к, Na
    B. ( mathrm{K}, mathrm{Na}, mathrm{Li} )
    c. Na, Li, K
    D. Li, Na, K
    11
    480 Which is not anomalous pair of elements in the Mendeleev’s periodic
    table?
    ( mathbf{A} cdot A r ) and ( K )
    B. ( C o ) and ( N i )
    c. ( T e ) and ( I )
    D. ( A l ) and ( S i )
    11
    481 The atoms of elements belonging to the same group of periodic table have the
    same :
    A. number of protons
    B. number of electrons
    c. number of neutrons
    D. number of electrons in the outermost shell
    11
    482 Magnesium is present in:
    A. ascorbic acid
    B. vitamin B ( _{12} )
    c. chlorophyll
    D. haemoglobin
    11
    483 State the position of cerium ( (z=58) ) and uranium ( (z=92) ) in periodic table? 11
    484 On moving from left to right in any period valence electrons keeps on increasing and period gets over when that valence shell gets filled.
    A . True
    B. False
    11
    485 From among the elements, choose the
    following:
    ( mathrm{Cl}, mathrm{Br}, mathrm{F}, mathrm{O}, mathrm{Al}, mathrm{C}, mathrm{Li}, mathrm{Cs} ) and ( mathrm{Xe} )
    The element which shows diagonal relationship with Mg.
    11
    486 Calculate the energy required for the
    process:
    ( boldsymbol{H} boldsymbol{e}^{+}(boldsymbol{g}) rightarrow boldsymbol{H} boldsymbol{e}^{2+}(boldsymbol{g})+boldsymbol{e}^{-} )
    If the ionisation energy for the H atom in the ground state is ( 2.18 times 10^{-18} )
    J/atom.
    11
    487 Which of the following pairs has both members from the same group of the periodic table?
    A. ( N a, C a )
    в. ( N a, C l )
    c. ( C a, C l )
    D. ( C l, B r )
    11
    488 What is the name of the element with
    atomic number ( 105 ? )
    A. Dubnium
    B. Holmium
    c. Kurchatovium
    D. Nobelium
    11
    489 lonisation potential of boron is less than that of beryllium. This is because:
    A . B has ( 1 s^{2} 2 s^{2} 2 p^{1} ) configuration
    B. B has small atomic size
    c. B has higher nuclear charge
    D. B has more number of shells
    11
    490 Q. 48 Assertion (A) Electron qain enthalpy becomes less negative as we go
    down a group.
    Reason (R) Size of the atom increases on going down the group and the
    added electron would be farther from the nucleus.
    (a) Assertion and reason both are correct statements but reason is not correct
    explanation for assertion.
    (b) Assertion and reason both are correct statements and reason is correct
    explanation for assertion.
    (c) Assertion and reason both are wrong statements.
    (d) Assertion is wrong statement but reason is correct statement.
    11
    491 Which of the following pairs has both members from the same group of periodic table?
    A. ( M g, B a )
    в. ( M g, N a )
    c. ( M g, C u )
    D. ( M g, K )
    11
    492 What is the electronic arrangement of G
    ( ? )
    A. 2,2,5
    B. 2, 4, 3
    c. 2,7
    D. 2, 5, 2
    11
    493 The characteristics which remains
    same on moving down a sub-group:
    A. atomic size
    B. ionization potential
    c. valence shell electrons
    D. electronegativity
    11
    494 Assertion
    ( left[A lleft(H_{2} Oright)_{6}right]^{3+} ) is a stronger acid than
    ( left[boldsymbol{M} boldsymbol{g}left(boldsymbol{H}_{2} boldsymbol{O}right)_{6}right]^{2+} )
    Reason
    Size of ( left[A lleft(H_{2} Oright)_{6}right]^{3+} ) is smaller than
    ( left[M gleft(H_{2} Oright)_{6}right]^{2+} ) and possesses more
    effective nuclear charge.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Both Assertion and Reason are incorrect
    11
    495 The lightest gas is :
    A. nitrogen
    B. helium
    c. oxygen
    D. hydrogen
    11
    496 Which of the following statements related to the modern periodic table is incorrect?
    (a) The p-block has 6 columns because a maximum of 6 electrons can occupy
    all
    the orbitals in a p-shell
    (b) The d-block has 8 columns because
    a maximum of 8 electrons can occupy
    all the orbitals in a d-subshell
    (c) Each block contains a number of
    columns equal to the number of electrons that can occupy that subshell
    (d) The block indicates value of
    azimuthal quantum number (I) for the last subshell that received electrons
    in building up the electronic configuration
    11
    497 which of the following statements is true about effective nuclear charge?
    This question has multiple correct options
    A. ( Z_{text {eff}} ) decreases from top to bottom
    B. ( Z_{text {eff}} ) increases from top to bottom
    C. ( Z_{text {eff}} ) increases as we move from left to right in periodic table
    D. ( Z_{e f f}=Z times sigma ) (here ( sigma ) is screening constant
    11
    498 Q. 42 Among alkali metals which element do you expect to be least
    electronegative and why?
    AO
    11
    499 Q.55 Discuss and compare the trend in ionisation enthalpy of the elements of
    group 1 with those of group 17 elements.
    11
    500 Consider the following steps. ( boldsymbol{A}(boldsymbol{g}) overrightarrow{boldsymbol{E}_{1}} )
    ( boldsymbol{A}^{+}(boldsymbol{g}) underset{boldsymbol{E}_{2}}{longrightarrow} boldsymbol{A}^{2+}(boldsymbol{g}) underset{boldsymbol{E}_{3}}{longrightarrow} boldsymbol{A}^{3+}(boldsymbol{g}) ) Third
    ionization energy of ( boldsymbol{A}(boldsymbol{g}) ) is ( ? )
    A. ( E_{1}+E_{2} )
    B . ( E_{1}+E_{2}+E_{3} )
    ( mathbf{c} cdotleft(E_{1}+E_{2}+E_{3}right)^{/ 3} )
    D. ( E_{3} )
    11
    501 Q1. State the Modern Periodic Law. 11
    502 Why first ionization enthalpy of nitrogen
    is more than oxygen?
    11
    503 Assertion: Inert gases are monoatomic.
    Reason: Inert gases have stable configuration.
    A. Both assertion and reason are true and the reason is a
    correct explanation of the assertion
    B. Both assertion and reason are true but reason is not a
    correct explanation of the assertion
    C. The assertion is true but reason is false
    D. Both the assertion and reason are false
    E. The assertion is false but the reason is true
    11
    504 In the third period of the periodic table,the element having smallest size is :
    A. ( N a )
    в. ( A r )
    c. ( C l )
    D. ( s i )
    11
    505 The atomic number of a halogen element in the fourth period is ( 35 . ) If true
    enter ( 1, ) else enter 0
    11
    506 Examples of elements belonging to ( s, p, d ) or ( f- ) block are given below.
    Identify the wrong example.
    A. ( s ) -block element – Caesium
    B. ( p ) -block element – Barium
    c. ( d ) – block element – Chromium
    D. ( f ) -block element – Thorium
    11
    507 The most significant contribution towards the development of periodic table was made by:
    A. Mendeleev
    B. Avogadro
    c. Dalton
    D. Cavendish
    11
    508 In Newlands’ table, which of the
    following elements was not placed in the same group in which cobalt and
    nickel were present?
    A. Chlorine
    B. Bromine
    C. Fluorine
    D. None of the above
    11
    509 With the increase in atomic number,
    screening effect increases both in group and period.
    A. True
    B. False
    11
    510 An element with atomic number ’32’
    belongs to
    A. 4th period, VIA group
    B. 3rd period, IV A group
    c. 4 th period, IV A group
    D. 5th period, va group
    11
    511 Q4. Name different blocks of elements in the periodic table. Give general electronic configuration
    of each block.
    n
    itontie
    109
    11
    512 Mendeleev used a Sanskrit numeral
    before the names of the predicted elements. What was the term used for
    it?
    A. sasi
    B. Eka
    c. Astan
    D. Pancan
    11
    513 What is the apparent oxidation state of
    ( C ) element in the compound ( C O_{2} ? )
    ( A cdot+2 )
    B. – 2
    ( c cdot+4 )
    D. –
    ( mathrm{E} cdot+5 )
    11
    514 In the given elements, which element does not have 2 valence electrons?
    A. Ba
    B. zn
    c. Na
    D. ca
    11
    515 Which period is incomplete in the modern periodic table?
    A . ( 1 s )
    B. 2nd
    ( c cdot ) 6th
    D. 7th
    11
    516 Which of the following has the highest
    ionization energy?
    A. ( C )
    в. ( N )
    ( c cdot O )
    D. ( F )
    E . ( N e )
    11
    517 In the modern periodic table, how does the atomic size of the elements vary
    along the period and down the group? Explain.
    11
    518 The placement of elements in the Newlands’ table was compared to:
    A. weeks of a month
    B. notes of music
    c. months of a year
    D. days of a month
    11
    519 The outermost electronic configuration of the most electronegative element is:
    ( mathbf{A} cdot n s^{2} n p^{3} )
    В. ( n s^{2} n p^{6} )
    ( c cdot n s^{2} )
    D. ( n s^{2} n p^{5} )
    11
    520 Assertion
    ( boldsymbol{S} boldsymbol{c}(boldsymbol{Z}=mathbf{2 1}) ) is placed in d-block
    elements.
    Reason
    Last filling electron goes into ( 3 d- ) suborbit.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    521 A hydrogen like atom with atomic number ( Z ) is in higher excited state of quantum number ‘n’. This excited state
    atom can make a transition to the first
    excited state by successively emitting two photons of energies ( 10 mathrm{eV} ) and ( 68.2 mathrm{eV} ) respectively. Alternatively the atom from the same the same excited
    state can make a transition to the 2 nd
    excited state by emitting two photons of energies ( 4.25 mathrm{eV} ) and ( 5.95 mathrm{eV} ) respectively Calculate the value of ( z )
    11
    522 Periodic Table(Abbreviated): The
    element that will react in a 1: 1 ratio
    with (D) is:
    begin{tabular}{|c|c|c|c|c|c|}
    hline ( mathbf{z}_{mathbf{L i}} ) & & & & & ( mathbf{( D )} ) & ( mathbf{1 0} ) \
    hline & ( mathbf{( A )} ) & & & & ( mathbf{( C )} ) & & \
    hline ( mathbf{( B )} ) & ( mathbf{2 0} ) & & & & & \
    hline
    end{tabular}
    B.
    ( r )
    D
    11
    523 Which of the following statement(s) about the Modern periodic table is/are incorrect?
    (i) The elements in the Modern periodic table are arranged on the basis of their decreasing atomic number.
    (ii) The elements in the Modern periodic table are arranged on the basis of their increasing atomic number
    (iii) Isotopes are placed in an adjoining group(s) in the periodic table.
    A. (i) only
    B. (i) and (ii)
    c. (ii) and (iii)
    D. (i) and (iii)
    11
    524 Arrange the elements in increasing order of atomic radius ( mathrm{Na}, mathrm{Rb}, mathrm{K}, mathrm{Mg} )
    A. ( mathrm{Na}<mathrm{K}<mathrm{Mg}<mathrm{Rb} )
    B. ( K<N a<M g<R b )
    ( mathrm{c} cdot mathrm{Mg}<mathrm{Na}<mathrm{K}<mathrm{Rb} )
    D. ( R b<K<M g<N a )
    11
    525 09. Give the electronic configuration of the transition elements. Write their four important
    characteristics.
    Ans. The d-block elements are not
    11
    526 Given below are some elements of the
    modern periodic table:
    ( _{4} B e,_{26} F e,_{14} S i,_{19} K,_{20} C a )
    (i) Select the element that has one
    electron in the outermost shell and
    write its electronic configuration.
    (ii) Select two elements that belong to the same group. Give reason for your
    answer.
    (iii) Select two elements that belong to the same period. Which one of the two
    has bigger atomic size?
    11
    527 ( I P_{1} ) and ( I P_{2} ) of Mg are 178 and ( 348 mathrm{K} )
    cal ( m o l^{-1} . ) The enthalpy required for the reaction ( M g rightarrow M g^{2+}+2 e^{-} ) is:
    A ( . .+170 ) K.cal
    B. +526 K.cal
    c. -170 K.cal
    D . -526 K.cal
    11
    528 IUPAC symbol of atomic number 119
    A. ( U u h )
    в. Uun
    c. ( U u e )
    D. ( U u b )
    11
    529 Which of the following pair of elements follows Newland’s law of octave?
    A. ( N e, A r )
    в. ( C, N )
    c. ( N a, K )
    D. ( P, S )
    11
    530 According to classification of elements
    most of non-metals are placed in
    block
    A. ( s ) -block
    B. ( p ) – block
    c. ( d ) – block
    D. ( f ) – block
    11
    531 The period of element having three shells with three electrons in valence
    shell is:
    ( A cdot 2 )
    B. 3
    ( c cdot 4 )
    D. 5
    11
    532 Which of the following gaseous molecules is monoatomic?
    A. Chlorine
    B. Helium
    c. oxygen
    D. Nitrogen
    11
    533 Which of the following is general electron configuration of ( 4 d ) series?
    ( mathbf{A} cdot 4 s^{1+o 2} 3 d^{1+t 01} )
    B. ( 4 s^{1 t o 2} 4 d^{1+t 01} )
    ( mathbf{c} cdot 5 s^{1 t o 2} 5 d^{1 t o 10} )
    D. ( 5 s^{1 operatorname{to} 2} 4 d^{1 text { lto } 10} )
    11
    534 Which one of the following does not increase while moving down the group of the periodic table?
    A. Atomic radius
    B. Metallic character
    c. Valence electrons
    D. None of the above
    11
    535 The properties of the elements, as well as the formulae and properties of their compounds depend in a periodic manner on the atomic weights of the elements. This periodic law was given by :
    A. J.L. Meyer
    B. John A.R. Newlands
    c. Dobernier
    D. D.I. Mendeleev
    11
    536 Which of the following burns to form an
    oxide, which is gaseous at room temperature?
    A. Hydrogen
    B. Phosphorus
    c. Calcium
    D. Sulphur
    11
    537 The electronic configuration of transition elements is:
    A ( cdot n s^{1} )
    B . ( n s^{2} n p^{5} )
    c. ( n s^{2}(n-1) d^{10} )
    D . ( (n-1) d^{1-10} n s^{0}-2 )
    11
    538 Which of the following groups contains metals, non-metals and metalloids?
    A. Group 17
    B. Group 14
    c. Group 13
    D. Group 12
    11
    539 Q7. What are horizontal rows and vertical columns of the periodic table called? 11
    540 The outer most shell of a representative
    element contains ‘a’ electrons and
    penultimate shell contains ‘b’ electrons. The valency of the element will be:
    A ( cdot a+b )
    в. ( b-a )
    ( c cdot b )
    D. ( a ) or ( 8-a )
    11
    541 If Aufbau rule is not followed, ( boldsymbol{K}-mathbf{1 9} )
    will be placed in block.
    A . ( s )
    B . ( p )
    ( c cdot d )
    D. ( f )
    11
    542 Which element has the symbol ( W ? )
    A. Silver
    B. Vanadium
    c. Tin
    D. Platinum
    E . Tungsten
    11
    543 Which of the following statement (s) is/are true regarding the change:
    ( boldsymbol{C N}^{-} rightarrow boldsymbol{C N O}^{-} ? )
    This question has multiple correct options
    A. Carbon is losing two electrons per atom.
    B. The oxidation state of carbon change from +2 to +4
    c. oxidation state of nitrogen is not changing
    D. oxidation state of nitrogen changes from – 3 to –
    11
    544 Q19. The first ionization enthalpy values (in kJ mol) of group 13 elements are:
    B AL Ga In T
    801 577 579 558 589
    How would you explain this deviation from the general trend?
    1 funm to Alie due to the bigger size of A
    11
    545 Match List I and List II. 11
    546 The long form of the periodic table
    consists of ( _{-} ) horizontal rows and
    vertical columns
    A. 6 and 17
    B. 7 and 7
    c. 5 and 7
    D. 7 and 18
    11
    547 0.45 Electronic configuration of some elements is given in Column I and their
    electron gain enthalpies are given in Column II. Match the electronic
    configuration with electron gain enthalpy.
    Column !
    Column II
    (Electronic configuration) (Electron gain enthalpy/kJmol”‘
    A. 15² 25 206
    -53
    15² 25² 2p 3s’
    152 25 2p
    -141
    15 25² 2p+
    + 48
    -328
    D.
    11
    548 ( 1 mathrm{s}^{2} 2 mathrm{s}^{2} 2 mathrm{p}^{6} ) is the electron configuration
    of:
    A. nitrogen
    B. boron
    c. argon
    D. neon
    11
    549 The element with atomic number 35
    belongs to :
    A. s -block
    B. p-block
    c. d.-block
    D. f-block
    11
    550 Define electronegativity. Why standard entropy of an elementary substanceis not zero whereas standard
    enthalpy of formation is taken as zero?
    11
    551 2. 7 Among halogens, the correct order of amount of energy released in electron
    gain (electron gain enthalpy) is
    (a) F > Cl> Br>I (b) F< Cl< Br<I (c) FBr>I (d) F< Cl< Br<I
    11
    552 Which of the following match is correct?
    A. last natural element- Uub
    B. General electronic configuration of IA group – ( n s^{2} )
    C. inert gas lies in ( 2^{n d}-6^{t h} ) period
    D. Typical elements – ( 3^{r d} ) period elements
    11
    553 The atomic number of element Unq is:
    A . 102
    B. 103
    ( c cdot 104 )
    D. 105
    11
    554 Why ( B e O ) and ( A l_{2} O_{3} ) are amphoteric? 11
    555 Which of the following element belongs
    to the group ( 18 ? )
    ( mathbf{A} cdot H )
    в. ( N e )
    c. ( C l )
    D. ( F )
    11
    556 Elements with atomic number greater than 92 are called actinides.
    A. True
    B. False
    11
    557 Atom with atomic radii and
    ionisation potential tends to gain electrons
    A. large, high
    B. large, low
    c. small, low
    D. small, high
    11
    558 Assertion
    According to Mendeleev, periodic properties of elements are periodic
    function of their atomic number
    Reason
    Atomic number is equal to the number of protons.
    A. Both Assertion and Reason are correct and Reason is the correct explanation of Assertion.
    B. Both Assertion and Reason are correct, but Reason is not the correct explanation of assertion.
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    559 IP values of an element ‘X’ are 104 kJ,
    ( 200 mathrm{kJ}, 420 mathrm{kJ}, 2825 mathrm{kJ} ) per mole
    Identify the group to which the element
    belongs ?
    A . ( I A )
    в. ( I I A )
    c. ( I I I A )
    D. ( I V A )
    11
    560 Q23. How would you react to the statement that the electronegativity of Non Pauling scale is 3.0 in
    all the nitrogen compounds?
    11
    561 Which of the following species has the highest electron affinity?
    A. ( F )
    в. ( O )
    ( c cdot O )
    D. ( N a^{+} )
    11
    562 Which of the following is(are) the merit(s) of Mendeleev’s periodic table?
    A. Could also predict the properties of these unknown elements
    B. Grouping of chemically dissimilar elements.
    c. Position given to isotopes.
    D. Presence of anomalous pairs
    11
    563 Write present names of Eka-aluminium and Eka-silicon. 11
    564 Hydrogen resembles halogens as:
    A. hydrogen forms diatomic molecule
    B. it combines with metal and non-metals to form
    compounds
    C. both ( A ) and ( B )
    D. none of the above
    11
    565 Which order of relative size among the following is incorrect?
    A. ( L i<N a<K )
    в. ( C<S iA l<N a )
    D. ( F<C l<B r )
    11
    566 Element Electronegative begin{tabular}{ccc}
    ( P ) & 2.1 \
    ( H ) & 2.2 \
    ( B r ) & 2.8 \
    hline
    end{tabular} ( B^{r} ) 1
    ( O ) 3.5 If What is and
    On the basis of the electronegativity values given above, in which of the following are the bonds most polar?
    ( mathbf{A} cdot P H_{3} )
    B. ( H_{2} O )
    ( mathbf{c} cdot H B r )
    D. ( P_{4} )
    E ( . P B r_{3} )
    11
    567 In Mendeleev’s Periodic Table, why was
    there no mention of Noble gases like
    Helium, Neon and Argon?
    11
    568 Where are the transition metals in the
    periodic table?
    A. In group o
    B. In group 1
    c. In group 2
    D. In a central block from 3-12 group number
    11
    569 Q. 24 Explain why the electron gain enthalpy of fluorine is less negative than
    that of chlorine?
    inthallen
    in loon noontive than that of Cl because when an electronis
    11
    570 The last element of lanthanide series is
    A. lawrencium
    B. lutetium
    c. cerium
    D. thorium
    11
    571 ( boldsymbol{C H} equiv boldsymbol{C H} ) is more electronegative as
    compared to ( C H_{2} equiv C H_{2} ) Explain.
    11
    572 The type of elements present in group ( 1[mid A] ) is:
    A . alkal
    B. alkaline
    c. transition
    D. halogen
    11
    573 Metal ( A ) has electronic configuration of
    2,8,1 and metal ( B ) has electronic
    configuration of 2,8,2 Identify these metals:
    11
    574 The element which resembled cobalt,
    nickel and was placed in Newland’s table far away from those elements was:
    A. sodium
    B. calcium
    ( c . ) iron
    D. chlorine
    11
    575 Initially, it was believed that the atomic mass of beryllium was 13. But Mendeleev suggested that its atomic
    mass should be 9
    i) Was Mendeleev suggestion correct?
    ii) How had he reached to this
    conclusion?
    11
    576 How many valence electrons are present
    in element Q?
    11
    577 Which forms the smallest of the +1 ions?
    A. Lithium
    B. Sodium
    c. Potassium
    D. Rubidium
    E. cesium
    11
    578 Which has maximum ionisation
    potential?
    A. ( N )
    в. ( O )
    ( c cdot O^{+} )
    D. ( N a )
    11
    579 ( E C ) of ( G d(64) ) is written as:
    A ( cdot[X e]_{54} 4 f^{7} 5 d^{1} 6 s^{2} )
    В ( cdot[X e]_{54} 4 f^{8} 8 s^{2} )
    ( mathbf{c} cdot[X e]_{54} 4 f^{9} 6 s^{1} )
    D. ( [X e]_{54} 4 f^{10} )
    11
    580 14 comprehension given below is followed by some multiple choice questions.
    cach question has one correct option. Choose the correct option:
    the modern periodic table, elements are arranged in order of
    increasing atomic numbers which is related to the electronic
    configuration. Depending upon the type of orbitals receiving the last
    electron, the elements in the periodic table have been divided into four
    blocks, viz s, p, d and f.
    The modern periodic table consists of 7 periods and 18 groups. Each
    period begins with the filling of a new energy shell. In accordance with
    the Aufbau principle, the seven periods (1 to 7) have 2, 8, 8, 18, 18, 32
    and 32 elements respectively.
    The seventh period is still incomplete. To avoid the periodic table being
    too long, the two series of f-block elements, called lanthanoids and
    actinoids are placed at the bottom of the main body of the periodic
    table
    (i) The element with atomic number 57 belongs to
    (a) s-block (b) p-block (c) d-block (d) f-block
    Ane to the olomont with atomic numhar 57 holona to d
    11
    581 Atomic wt. of ( C l=35.5 ) and of ( I=127 )
    According to Doeberiner triad rule
    atomic wt. of ( boldsymbol{B r} ) will be:
    A . 80.0
    B. 162.5
    c. 81.25
    D. 91.5
    11
    582 Which of two elements among the following will display the most similar chemical properties?
    A. Aluminum and calcium
    B. Nickel and phosphorus
    c. chlorine and sulfur
    D. Carbon and sulfur
    E. Lithium and potassium
    11
    583 Element ‘X’ has twelve protons in its nucleus. To which group of the periodic table it will belong?
    ( A )
    B. 2
    ( c cdot 6 )
    D. 8
    11
    584 The correct order of ionization energies
    of ( boldsymbol{F}^{-}, boldsymbol{C l}^{-} boldsymbol{F} ) and ( boldsymbol{C l} ) is:
    A ( cdot C l<F<C l^{-}<F^{-} )
    B . ( C l^{-}<F^{-}<C l<F )
    c. ( F^{-}<C l^{-}<C l<F )
    D. ( C l^{-}<C l<F^{-}<F )
    11
    585 Q6. Write the atomic number of the element present in the third period and seventeenth group
    the periodic table.
    Ans. The element is chlorine (Cl) with atomic number (7) = 17.
    11
    586 Aluminium is diagonally related to
    A ( . L i )
    B. ( S ) i
    ( c . B e )
    D. ( B )
    11
    587 The atomic number of an element ‘y’ is
    20. The electronic configuration of the ion having inert gas configuration is:
    A .2,8,10
    B. 2,18
    c. 2,10,8
    D. 2, 8, 8
    11
    588 The number of valence electrons that
    can be present in the second element of any period is:
    A . 1
    B . 2
    ( c .5 )
    D. 7
    11
    589 Which of the following is the correct match?
    (a) Eka silicon – Ge
    (b) Eka aluminum – Ga
    (c) Eka manganese – Tr
    (d) Eka boron – Sc
    ( A cdot b, c )
    B. a, b, d
    ( c cdot a, d )
    D. All of above
    11
    590 Which of the given elements ( A, B, C, D ) and E with atomic number 2,3,7,10
    and 30 respectively belong to the same period?
    ( A cdot A, B, C )
    B. В, С, D
    c. А, D, ह
    D. B, D, E
    11
    591 Anomalous pair in Mendeleev’s periodic
    table is:
    A. ( L i, N a )
    в. ( M g, ) Аl
    c. ( C o, N i )
    D. ( B e, B )
    11
    592 Among the elements ( C a, M g, P ) and ( C l )
    the order of increasing atomic radii is:
    A. ( M g<C a<C l<P )
    в. ( C l<P<M g<C a )
    c. ( P<C l<C a<M g )
    D. ( C a<M g<P<C l )
    ( l )
    11
    593 Which of the following is not the reason
    for the higher ( boldsymbol{E} boldsymbol{A}_{1} ) of halogens?
    I) High nuclear charge
    Il) Larger atomic size
    III) Easy to get octet configuration, i.e. ( boldsymbol{n} boldsymbol{s}^{2} boldsymbol{n} boldsymbol{p}^{6} )
    IV) Half filled p-orbitals
    A. I and IV
    B. I, II and III
    c. Il and IV
    D. II and III
    11
    594 Electron gain enthalpy is positive when:
    A ( cdot O^{-} ) is formed from ( O )
    B. ( O^{2-} ) is formed from ( O^{-} )
    ( mathrm{c} cdot O^{+} ) is formed from ( O )
    D. electron affinity is always a negative value
    11
    595 From the following which is the false
    statement for the long form of the periodic table?
    A. it reflects the sequence of filling the electrons in the order of sub-energy level s, p, d and f
    B. it helps to predict the stable valency states of the elements
    c. it reflects trends in physical and chemical properties of the elements
    D. it helps to predict the relative ionic nature of the bond between any two elements
    11
    596 The element with atomic number 9
    resembles with the element having atomic number:
    ( A cdot 8 )
    B. 17
    ( c . ) 36
    D. 27
    11
    597 Assertion
    Newland’s law of octaves of elements is
    a function of their state that the
    property of every eighth element is the repetition of the first.
    Reason
    The maximum of 8 electrons can be
    accommodated in valence shell.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    598 Column-
    Column-II
    (Atomic number of elements)
    (IUPAC name)
    (A) 105
    (P) Uun
    (В) 107
    (Q) Uns
    (C) 109
    (R) Unp
    (D) 110
    (h)
    (S) Une
    The correct match for ( A, B, C, D ) are
    respectively:
    A ( . ) R, P, s,
    в. Р, R, s,
    c. R, Q, s, p
    D. Q, R, s,
    11
    599 An element ( X ) has 7 electrons in its
    shell. What is true about the element ( X )
    ( ? )
    This question has multiple correct options
    A. It belongs to period 9 of modern periodic table.
    B. Its atom contains 9 protons.
    C. It has a valency of 7
    D. It can accept an electron to acquire noble gas configuration.
    11
    600 Which of the following has the highest
    electron affinity?
    A. ( F )
    в. ( C l )
    ( c . B r )
    D. ( I )
    11
    601 What is the total number of p electrons in a single phosphorus atom in its ground state?
    ( A cdot 3 )
    B. 5
    ( c .9 )
    D. 15
    11
    602 Sub-shell electronic configuration of elements ( P, Q ) and ( R ) is given
    ( [P, Q text { and } R text { are imaginary symbols }] ) ( P=1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1} )
    ( Q=1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5} )
    ( mathrm{R}=1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2} 4 s^{2} 3 d^{1} )
    (a) One of these electronic
    configurations given above is wrong. Which is the element?
    (b) Out of ( P, Q ) and ( R ) which has the highest electronegativity?
    (c) Can ( P ) and ( Q ) join to form an ionic compound? Justify your answer
    11
    603 What is the electronic configuration of the ground state of the magnesium
    cation, ( M g^{2+} ? )
    A ( cdot 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} )
    B ( cdot 1 s^{2} 2 s^{2} 2 p^{6} 3 s )
    C ( cdot 1 s^{2} 2 s^{2} 2 p^{6} )
    D. ( 1 s^{2} 2 s^{2} 2 p^{4} 3 s^{2} )
    11
    604 In which of the following pairs, the first atom or ion is not larger than the
    second?
    A ( cdot F e^{2+}, F e^{3+} )
    в. ( O, S )
    c. ( N, O )
    D. ( C l^{-}, C l )
    11
    605 Beryllium and aluminium exhibit many properties which are similar. But, the two elements differ in:
    A. maximum covalency in compounds
    B. forming polymeric hydrides
    c. forming covalent halides
    D. exhibiting amphoteric nature in their oxides
    11
    606 The metal having highest ionisation potential is :
    A. lithium
    B. sodium
    c. potassium
    D. caesium
    11
    607 The liquid non-metal belongs to which
    group number?
    A . 15
    B. 16
    c. 17
    D. 18
    11
    608 In a group, basic nature from
    top to bottom.
    A. decreases
    B. increases
    c. constant
    D. none of these
    11
    609 5. Among the following elements, which has the least electron affinity?
    (a) Phosphorous (b) Oxygen (C) Sulphur
    (d) Nitrogen
    11
    610 Explain Pauling’s scale of electronegativity. 11
    611 Explain the appropriate reason for the following statement:
    (a)Size of ( M g^{2+} ) is less than Mg.
    (b) Electron gain enthalpy of Cl is more than that of F.
    11
    612 Difference in the number of protons of the largest element of the fourth period
    and the smallest element of the third
    period is:
    ( A )
    B. 2
    c. 20
    D. 12
    11
    613 4th period in periodic table, ends with krypton.
    A . True
    B. False
    11
    614 An element is placed in the 2 nd group and 3 rd period of the periodic table, burns in presence of oxygen to form a
    basic oxide. The electronic
    configuration of the element is
    A. ( K, M, L(2,8,2) )
    B. ( K, L, M(2,6,4) )
    c. К, М, L (4,6,2)
    D. K,L, M (2,8, 2)
    11
    615 Two elements were elected by Mendeleev for studying the properties of compounds formed by other elements with the selected elements. What were
    the selected elements?
    A. Oxygen, Nitrogen
    B. Hydrogen, Carbon
    c. Hydrogen, Oxygen
    D. Oxygen, Carbon
    11
    616 In the Doberiener’s triad, all three
    elements have similar:
    A. electronic configuration
    B. properties
    c. number of shells
    D. both A and B
    11
    617 Which of the following is incorrect statement about Mendeleev’s
    classification of elements?
    A. He could classify all the elements including noble gases
    B. He left gaps for some yet to be discovered elements
    c. He predicted the properties of some undiscovered elements
    D. There was no place for isotopes in his table
    11
    618 An element with ( Z=46 ) belongs to :
    A. 9 group
    B. 10 group
    c. 11 group
    D. 12 group
    11
    619 There are no compounds of He and Ne.
    If true enter 1 , else enter 0
    11
    620 ( P b^{4+} ) salts are better oxidizing agent agents, while ( G e^{2+} ) salts are better
    reducing agents. Explain.
    11
    621 The largest atom among the following is:
    A. sodium
    B. silicon
    c. potassium
    D. calcium
    11
    622 Element having atomic number 33 belongs to period:
    A . ( I I I )
    в. ( I V )
    ( c cdot V )
    D. ( V I )
    11
    623 The low electron affinity value of nitrogen is due to:
    A. small size
    B. high nuclear charge
    c. half-filled 2p subshell
    D. high metallic character
    11
    624 The properties which repeats repeatedly
    at a regular interval is called
    A. Diagonal properties
    B. Anomalous properties
    c. Periodic properties
    D. None
    11
    625 Which among the following is not an anomalous pair in Mendeleev’s periodic
    table?
    A . Co, Ni
    в. Te,
    c. Ar, ( k )
    D. Sc, Ga
    11
    626 4. What is the electronic configuration of the elements of group 14?
    (a) ns? np (b) nsnp (c) nsºnpº
    (d) ns2
    11
    627 The eight group of Mendeleev’s periodic table is divided into how many subgroups?
    A .2
    B. 0
    ( c cdot 4 )
    D.
    11
    628 Assertion
    According to Mendeleev, the properties of elements are a periodic function of their atomic weights.
    Reason
    Mendeleev left the gap under aluminium and a gap under silicon, and called these elements Eka-Aluminium
    and Eka-Silicon.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is correct but Reason is incorrect
    D. Both Assertion and Reason are incorrect
    11
    629 Which of the following is the correct order of chemical reactivity with water according to electrochemical series?
    A. ( K>M g>Z n>C u )
    в. ( K>M g>C u>Z n )
    c. ( C u>Z n>K>M g )
    D. ( M g>K>C u>Z n )
    11
    630 The outermost configuration of the least reactive element is:
    A ( cdot n s^{2} n p^{3} )
    B . ( n s^{2} n p^{4} )
    ( mathbf{c} cdot n s^{2} n p^{5} )
    D. ( n s^{2} n p^{6} )
    11
    631 034. Which of the following statements related to the modern periodic table is incorrect?
    (a) The p-block has six columns, because a maximum of 6 electrons can occupy all the orbitals
    in a p-subshell
    (6) The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals
    in a d-subshell
    (c) Each block contains a number of columns equal to the number of electrons that can occupy
    that subshell.
    (d) The block indicates value of azimuthal quantum number (1) for the last subshell that received
    electrons in building up the electronic configuration.
    11
    632 The number of valence electrons across
    a period and down the group:
    A. increases, same
    B. decreases, same
    c. same, increases
    D. increase, decreases
    11
    633 Carbon belongs to second period and 14
    group. Silicon belongs to third period and group 14. If atomic number of carbon is ( 6, ) the atomic number of
    silicon is :
    A. 7
    B. 14
    ( c cdot 24 )
    D. 16
    11
    634 Atomic number of a halogen element in the fourth period is ( 35 . ) If true enter 1 else enter 0 11
    635 Q. 47 Assertion (A) Boron has a smaller first ionisation enth
    beryllium.
    Reason (R) The penetration of 2s electron to the nucleus is more than
    the 2p electron hence 2p electron is more shielded by the inner core of
    electrons than the 2s electrons
    (a) Assertion and reason both are correct statements but reason is not correct
    explanation for assertion.
    (b) Assertion is correct statement but reason is wrong statement.
    (d Assertion and reason both are correct statements and reason is correct
    explanation for Assertion
    (d) Assertion and reason both are wrong statements.
    11
    636 Which of the following elements exhibit maximum outermost electrons?
    A . Na a
    в. Мв
    ( c cdot s i )
    ( D )
    11
    637
    U.
    10
    11
    30. The ionization energy of the ionized sodium atom Nal0+
    (a) 13.6 eV
    (c) (13.6/11) eV
    (b) 13.6 x 11 eV
    (d) 13.6 x (112) eV
    11
    638 Which of the following set of elements cannot be a triad?
    A. ( L i, N a, K )
    B. ( B, A l, G a )
    c. ( B e, M g, C a )
    D. ( C l, B r, I )
    11
    639 In Mendeleev periodic table few elements that are chemically similar are placed in separate 11
    640 were not given separate place in periodic table.
    A. Alkali metalss
    B. Isotopes
    c. Halogens
    D. Non-metals
    11
    641 A soft metal stored under kerosene is:
    A. sodium (Na)
    B. calcium(Ca)
    c. lithium (Li)
    D. magnesium (Mg)
    11
    642 Write the electronic configuration of the
    ( C a^{2+} ) in absence of Aufbau Principle.
    A ( cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} )
    B ( cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{3} 3 p^{3} 4 d^{3} )
    c. ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{5} 4 d^{1} )
    D. none of these
    11
    643 Which lists elements in order of
    increasing ionization energy?
    A ( . S<S^{+}<S^{-} )
    B . ( S^{+}<S^{-}<S )
    c. ( S^{-}<S<S^{+} )
    D. ( S^{+}<S<S^{-} )
    11
    644 The oxidation state of boron in
    potassium tetrafluoroborate is:
    ( A cdot+2 )
    ( B cdot+3 )
    ( c cdot+4 )
    ( D cdot-3 )
    11
    645 Which combination is odd with respect
    to oxidation number?
    ( mathbf{A} cdot H_{2} S O_{4}, H_{2} S_{2} O_{8}, K_{2} C r_{2} O_{7}, S F_{6} )
    B. ( K_{2} C r_{2} O_{7}, K_{2} C r O_{4}, C r O_{5}, C r O_{2} C l_{2} )
    ( mathbf{C} cdot N H_{3}, N H_{4}^{+}, N_{3} H, N O_{2}^{-} )
    ( mathbf{D} cdot C a H_{2}, B a H_{2}, B e H_{2}, M g H_{2} )
    11
    646 The atomic number of non transition
    element of ( 6 mathrm{d} ) series of ( ^{prime} d^{prime} ) block
    elements
    A . 112
    B. 111
    ( c .110 )
    D. 80
    11
    647 Second ionization enthalpy of Na is greater than that of Mg.
    A. True
    B. False
    11
    648 The electronic configuration of chloride
    ion is:
    ( mathbf{A} cdot 2,8,7 )
    в. 2,8,6
    c. 2,8,8
    D. 2,
    11
    649 One element has atomic weight ( 39 . ) Its electronic configuration is
    ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2}, 3 p^{6} 4 s^{1} . ) The true
    statement for that element is:
    A. more I.E
    B. transition element
    C. isotone with ( _{18} A r^{36} )
    D. stable oxide ( M_{2} O )
    11
    650 What are the electronic configuration of
    ( N a^{+} ) and ( C l^{-} ) ions?
    ( mathbf{A} cdot N a^{+}=2,8,2 ) and ( C l^{-}=2,8,7 )
    B. ( N a^{+}=2,8 ) and ( C l^{-}=2,8,8 )
    ( mathbf{C} cdot N a^{+}=2,8,2 ) and ( C l^{-}=2,8,6 )
    D. ( N a^{+}=2,8 ) and ( C l^{-}=2,8,7 )
    11
    651 Select in each pair, and one having lower ionization energy and explain the
    reason
    (a) ( I ) and ( I^{-} )
    (b) ( B r ) and ( K )
    (c) ( L i ) and
    ( boldsymbol{L} boldsymbol{i}^{+} )
    (d) ( B a ) and ( S r )
    (e) ( O ) and ( S )
    (f) ( B e )
    and ( B )
    (g) ( N ) and ( O )
    11
    652 Which of the following element is expected to have highest electron gain enthalpy:
    A ( cdot 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5} )
    B ( cdot 1 s^{2} 2 s^{2} 2 p^{3} )
    c. ( 1 s^{2} 2 s^{2} 2 p^{4} )
    D ( cdot 1 s^{2} 2 s^{2} 2 p^{5} )
    11
    653 The electron configuration for potassium in the ground state:
    A ( cdot 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} )
    B . ( 1 s^{2} 2 s^{2} p^{6} 3 s^{2} 3 p^{6} 4 s^{2} )
    C ( cdot 1 s^{2} 2 s^{2} p^{6} 3 s^{2} 3 p^{6} 4 s^{1} )
    D. ( 1 s^{2} )
    E ( cdot 1 s^{2} 2 s^{2} 2 p^{6} 3 p^{1} )
    11
    654 The oxidation state of an element in a
    particular compound can be defined as:
    A. the charge acquired by its atom on the basis of electronegative consideration from other atoms in the molecule
    B. the residual charge acquired by it s atom after removing all electronegative atoms from the molecule
    C. the valency of the most electronegative atom present in the molecule
    D. total number of electrons accepted by an atom to form a molecule
    11
    655 The correct order of ionisation energy of
    ( boldsymbol{C}, boldsymbol{N}, boldsymbol{O} & boldsymbol{F} ) is:
    A. ( F<N<C<O )
    в. ( C<N<O<F )
    c. ( C<O<N<F )
    D. ( F<O<N<C )
    11
    656 Among the following which one has largest atomic radius?
    A ( . C l )
    в. ( F )
    c. ( L i )
    D. Ne
    E . ( N a )
    11
    657 The numerical value of energy involved in the given process ( K rightarrow K^{-} ) is less
    than that of which of the following
    processes?
    ( mathbf{A} cdot K^{-} rightarrow K )
    В. ( K rightarrow K^{+} )
    c. Both (a) and (b)
    D. None of these
    11
    658 Which one is correct
    A. Oxidizing property along a period – Decreases. Down the group – Increases. Reducing property along a period – Decreases. Down the group – Increases
    B. Oxidizing property along a period – Increases. Down the group – Decreases. Reducing property along a period – Increases. Down the group – Decreases
    C. Oxidizing property along a period – Increases. Down the group – Increases. Reducing property along a period – Decreases. Down the group – Increases
    D. Oxidizing property along a period – Increases. Down the group – Decreases. Reducing property along a period – Decreases. Down the group – Increases
    11
    659 Q. 6 The statement that is not correct for periodic classification of elements is
    (a) The properties of elements are periodic function of their atomic numbers
    (b) Non-metallic elements are less in number than metallic elements
    (c) For transition elements, the 3d-orbitals are filled with electrons after 3p-orbitals
    and before 4s-orbitals
    (d) The first ionisation enthalpies of elements generally increase with increase in
    atomic number as we go along a period
    11
    660 A sudden large jump between the values of second and third ionization
    energies of an element would be associated with the
    electronic configuration of:
    A ( cdot 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{1} )
    B . ( 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{1} )
    C ( cdot 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{2} )
    D. ( 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2} )
    11
    661 The ionization potential of elements in any group decreases from top to bottom. This is due to:
    A. increase in the size of an atom
    B. increase in the atomic number
    c. increase in the screening effect
    D. both increase in the size of an atom and increase in the screening effect
    11
    662 What was Mendeleev’s basis of
    classification of elements?
    11
    663 Based on modern classification of
    periodic table atomic number increases on moving from in
    periodic table.
    A . left to right
    B. right to left
    c. straight
    D. none of these
    11
    664 The correct order of increasing atomic
    size of element ( N, F, S i & P ) is:
    ( mathbf{A} cdot N<F<S i<P )
    B ( . F<N<P<S i )
    ( mathbf{c} cdot F<N<S i<P )
    D. ( N<S i<F<P )
    11
    665 Who was the first to classify the elements into metals and non-metals?
    A. Meyer
    B. Mendeleev
    C. Lavoisier
    D. None of the above
    11
    666 The elements belonging to which group are called representative elements? This question has multiple correct options
    A. 1 and 2
    B. 3 to 12
    ( c .13 ) to 18
    D. Element lying at the bottom of periodic table
    11
    667 Lanthanoids are also called as
    A. Transition elements
    B. Rare earth elements
    c. Both A and B
    D. None of these
    11
    668 Which of the following transitions
    involves maximum amount of energy?
    ( mathbf{A} cdot M_{(s)} rightarrow M_{(g)} )
    ( mathbf{B} cdot M_{(g)} rightarrow M^{+}(g) )
    ( mathbf{c} cdot M^{+}(g) rightarrow M^{2+}(g) )
    D. ( M^{2+}(g) rightarrow M^{3+}(g) )
    11
    669 The ionisation potential of isotopes of
    an element will be:
    A. same
    B. different
    c. dependent on atomic masses
    D. dependent on the number of neutrons present in the nucleus
    11
    670 Write the electronic configuration of ( boldsymbol{K} )
    and ( N e ? )
    11
    671 Which of the following statement(s) is incorrect ?
    A . lonisation energy ( propto frac{1}{text { Screening effect }} )
    B. The first ionisation energies of Be and Mg are more than ionisation energies of B and Al respectively
    c. Atomic and ionic radii of Niobium and Tantalum are almost same
    D. Metallic and covalent radii of potassium are 2.03 , and 2.3 ( dot{A} ) respectively
    11
    672 Fifth period has elements.
    ( A cdot 18 )
    B. 32
    ( c cdot 26 )
    D. 16
    11
    673 Noble gases are stable because their valence shell contains:
    A . 2 electrons
    B. 8 electrons
    c. both ( A ) and ( B )
    D. none of the above
    11
    674 An element has atomic number 79
    Predict the group and period in which the element is placed.
    A. 2nd group, 7th period
    B. 11th group, 6th period
    C. 13th group, 6th period
    D. 12th group, 6th period
    11
    675 The atomic number of Uut is:
    ( A cdot 113 )
    B. 114
    ( c cdot 108 )
    D. 115
    11
    676 Identify the position of the elements having outer electronic configuration
    ( n s^{2} n p^{5} ) for ( n=3 )
    A. 17 th group, 3rd period
    B. 8th group, sth period
    c. 7th group, 5th period
    D. 8th group, 4th period
    11
    677 Arrange the following ions in increasing
    order of their radius:
    ( mathbf{A} cdot M n^{+7}<V^{+5}<C a^{+2}<K^{+} C l^{-}<S^{2}<P^{3-} )
    B ( cdot M n^{+7}<C a^{+2}<V^{+5}<K^{+} C l^{-}<S^{2}<P^{3-} )
    ( mathbf{c} cdot M n^{+7}<V^{+5}<C a^{+2}<K^{+} C l^{-}<P^{3-}<S^{2} )
    D. ( V^{+5}<M n^{+7}<C a^{+2}<K^{+} C l^{-}<S^{2}<P^{3-} )
    11
    678 Assertion
    SnCl ( _{2} ) is a reducing agent.
    Reason
    SnCl ( _{2} ) reduces ( F e C l_{3} ) to ( F e C l_{2} ) and
    HgCl( _{2} ) to ( H g )
    A. Both Assertion and Reason are correct and Reason is
    the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    679 Which of the following will have highest nucleophilicity?
    ( mathbf{A} cdot boldsymbol{theta} )
    ( C l )
    B. ( theta ) ( F )
    ( c . theta )
    ( C H_{3} )
    D. ( theta ) ( O H )
    11
    680 The energy of an electron in the ( 1 s )
    orbital of ( boldsymbol{H}^{-}, boldsymbol{H} e, boldsymbol{L} boldsymbol{i}^{+} ) and ( boldsymbol{B} boldsymbol{e}^{2+} )
    follows the order.
    A ( . H^{-}>H e>L i^{+}>B e^{2} )
    B . ( L i^{+}>B e^{2+}>H e>H^{-} )
    ( mathbf{c} cdot B e^{2+}>L i^{+}>H e>H )
    D. ( H^{-}>L i^{+}>H e>B e^{2} )
    11
    681 The first element of a group in many ways differs from the other heavier
    members of the group. This is due to:
    This question has multiple correct options
    A. the smaller size
    B. the high electronegativity and high ionisation potential
    c. the unavailability of d-orbitals
    D. the higher shielding effect
    11
    682 The set representing the correct order of first ionisation potential is :
    A. ( K>N a>L i )
    в. ( B e>M g>C a )
    c. ( B>C>N )
    D. ( G e>S i>C )
    11
    683 Recently (in Aug 2003 ) two new elements have been discovered with
    atomic number:
    A .113,114
    В. 114,115
    ( mathrm{c} .115,116 )
    D. 113,115
    11
    684 When burned, sulfur forms a gaseous
    product ( X ) which can be oxidised to produce a gas ( Y . ) Gas Y reacts with water to produce a product Z. Which row correctly shows the oxidation states of sulfur in ( X, Y ) and ( Z ? )
    begin{tabular}{ccccc}
    & ( mathbf{x} ) & ( mathbf{Y} ) & ( mathbf{z} ) \
    ( mathbf{A} ) & -2 & +4 & +4 \
    & & & \
    ( mathrm{B} ) & -2 & +4 & +6 \
    ( mathrm{C} ) & +4 & +6 & +4 \
    & & & \
    ( mathrm{D} ) & +4 & +6 & +6 \
    hline
    end{tabular}
    ( A cdot A )
    B. B
    ( c cdot c )
    D.
    11
    685 possess the lowest
    first ionization energy in their respective period.
    A . Alkali metals
    B. Alkaline earth metals
    c. Noble gases
    D. Halogens
    11
    686 The electronic configurations of three elements ( X, Y ) and ( Z ) are 2,( 8 ; 2,8,7 ; ) and
    2,8,2 respectively. Which of the following is correct?
    A. ( X ) is a metal
    B. ( Y ) is a metal
    ( c cdot Z ) is a non-metal
    D. ( Y ) is a non-metal and ( Z ) is a metal
    11
    687 In iron atom ( (z=26), ) the
    differentiating electron enters sublevel:
    A ( .4 d )
    B. ( 3 d )
    c. ( 4 p )
    D. ( 5 p )
    11
    688 Which of the following is(are) Dobereiner’s triads?
    (a) ( P, A s, S b )
    (b) ( mathrm{Cu}, mathrm{Ag}, mathrm{Au} )
    (c) ( mathrm{Fe}, mathrm{Co}, mathrm{Ni} )
    ( (d) S, S e, T e )
    ( A cdot ) a and ( b )
    B. b and c
    ( c . ) a and d
    D. all of the above
    11
    689 Which of the following has highest second ionization energy?
    A . ( N i )
    в. ( V )
    ( c cdot C r )
    D. ( M n )
    11
    690 Which of the following atoms should
    have the highest 1st electron affinity?
    A. ( F )
    B. ( O )
    ( c . N )
    D. ( C l )
    11
    691 Use the following system of naming elements in which first alphabets of the digits are written collectively,
    0
    2
    uni
    bi rri quad pent
    Write three-letter symbol for the elements with atomic number 106
    A . un
    B. unh
    c. uunhe
    D. unhex
    11
    692 The gradual addition of electronic shells in the noble gases causes a decrease in their
    A. ionization energy
    B. atomic radius
    c. boiling point
    D. density
    11
    693 Which element is a metal with valency
    2?
    11
    694 Q7. Which element do you think would have been named by
    (i) Lawrence Berkeley Laboratory
    (ii) Seaborg’s group?
    11
    695 The electronic configuration of an element is ( 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2} . ) The
    oxidation number of the element in its
    compounds can be:
    ( A cdot+2 )
    B. +8
    ( c cdot+1 )
    ( D )
    11
    696 The elements of the group 16 are also called:
    A. helogens
    B. noble gases
    c. chalcogens
    D. alkaline earth metals
    11
    697 Valence shell electronic configuration of
    Barium is:
    ( A cdot 5 s^{2} )
    B. ( 6 s^{2} )
    ( c cdot 5 s )
    D. ( 6 s^{text {। }} )
    11
    698 The electronegativity order increases in the order:
    A. ( mathrm{C}, mathrm{N}, mathrm{Si}, mathrm{P} )
    B. ( N, ) Si, ( C, P )
    c. ( mathrm{si}, mathrm{P}, mathrm{C}, mathrm{N} )
    D. ( P, ) Si, ( N, C )
    11
    699 Which of the following corresponds to the configuration?
    ( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} )
    A. не
    B. Na a
    c. мg
    ( D cdot A )
    11
    700 Which of the following elements are
    called representative elements?
    ( mathbf{A} cdot p ) block elements only
    B. ( s ) and ( p ) block elements only
    C. ( d ) block elements only
    D. ( s ) block elements only
    11
    701 Total number of possible shells in
    uranium atom is:
    (atomic no. ( z=92) )
    A. 7
    B.
    ( c cdot 6 )
    D. none of these
    11
    702 An element has nine positive charges in its nucleus. Its common oxidation state
    is:
    ( A cdot+7 )
    B. +5
    ( c cdot-1 )
    D. +1
    11
    703 Two elements ( X ) and ( Y ) contain only one
    electron in the outer level. Element ( X ) is
    reactive and loses electron easily while element ( Y ) is relatively unreactive and
    non-corrosive. The elements ( boldsymbol{X} ) and ( boldsymbol{Y} )
    respectively are:
    ( mathbf{A} cdot C s ) and ( L i )
    B. ( R b ) and ( N a )
    c. ( L i ) and ( C u )
    D. ( A g ) and ( A u )
    11
    704 lonization potential in a period is lowest
    for:
    A. halogens
    B. inert gases
    c. alkali metals
    D. alkaline earth elements
    11
    705 Eka – silicon is a :
    A. metal
    B. non-metal
    c. metalloid
    D. none of the above
    11
    706 As you go down in a group, the alkali metals become:
    A. brighter
    B. hotter
    c. more reactive
    D. less reactive
    11
    707 Which of the following is the property of
    a group?
    A. The elements in the same group have similar outer electronic configuration.
    B. Their atomic size increases on moving down the group
    C. Their melting and boiling points changes in a regular manner
    D. All of the above
    11
    708 Which of the following has ( 2^{n d} I P< )
    ( 1^{s t} ) IP?
    A. ( M g )
    в. ( N e )
    ( c . c )
    D. None
    11
    709 The element having the least number of electron shells is :
    A. ( L )
    B.
    c. Na
    D. cs
    11
    710 The modern periodic table has been evolved through the early attempts of Dobereiner, Newland and Mendeleev.
    List one advantage and one limitation of all the three attempts.
    11
    711 Which is not correct in case of ( B e ) and
    ( A l ? )
    A. Both are rendered passive by conc. ( H N O_{3} )
    B. Carbides of both give methane on hydrolysis
    C. Both give hydroxides which are basic
    D. Both give covalent chlorides
    11
    712 Which of the following has largest
    radius?
    A ( cdot 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2} )
    B ( cdot 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{1} )
    C ( cdot 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{3} )
    D. ( 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{5} )
    11
    713 The elements with atomic numbers
    ( mathbf{9}, mathbf{1 7}, mathbf{3 5}, mathbf{5 3}, mathbf{8 5} ) are all :
    A . noble gases
    B. halogens
    c. heavy metals
    D. light metals
    11
    714 The number of completed transitional series in the periodic table is / are:
    A . 2
    B. 3
    ( c cdot 4 )
    ( D )
    11
    715 2. 11 The formation of oxide ion 02- (g), from oxygen atom requires first an
    exothermic and then an endothermic step as shown below
    0 (g) + 0- (g); AH = – 141 kJ mol-1
    0 (g) + 02 (g); AH = + 780 kJ mol-1
    Thus, process of formation of 02- in gas phase is unfavourable even
    though 02- is isoelectronic with neon. It is due to the fact that
    (a) oxygen is more electronegative
    (b) addition of electron in oxygen results in larger size of the ion
    (c) electron repulsion outweighs the stability gained by achieving noble gas
    configuration
    (d) Oion has comparatively smaller size than oxygen atom
    11
    716 If
    ( A, B ) and ( C ) are the three elements of
    Dobereiner’s triad, and atomic weights of ( A ) and ( B ) are 7 and ( 15, ) respectively then the atomic weight of ( C ) is :
    ( A cdot 1 )
    B. 11
    ( c cdot 23 )
    D. 25
    11
    717 Q10. What is screening or shielding effect? How does it influence the ionization enthalpy?
    ahalle chiold the electrons
    11
    718 No. of elements in 1st period are:
    ( A cdot 2 )
    B. 6
    ( c cdot 8 )
    D. 18
    11
    719 Which of the following is the most stable oxidation state of aluminium?
    A . -1
    B. +1
    ( c cdot+2 )
    D. +3
    11
    720 037. Which of the following statements is incorrect in relation to ionization enthalpy!
    (a) ionization enthalpy increases for each successive electron.
    (b) The greatest increase in ionization enthalpy is experienced on removal of electrons from
    core noble gas configuration.
    (c) End of valence electrons is marked by a big jump in ionization enthalpy.
    (d) Removal of electron from orbitals bearing lower n value is easier than from orbital having
    higher n value.
    at
    11
    721 An element ( X ) has IE and EA respectively 275 and ( 1450 k J ) mole ( ^{-1} ). The
    electronegativity of element according to Mullikan scale is ?
    A . 2.4
    в. 2.8
    ( c .3 .20 )
    ( D cdot 4.0 )
    11
    722 The atomic numbers of Lanthanides are
    from:
    A 57 to 71 1
    B. 90 to 103
    ( c .21 ) to 30
    D. 39 to 48
    11
    723 Diagonal relationship is shown between:
    A. ( C ) and ( N )
    B. ( B ) and ( M g )
    c. ( B ) and ( S i )
    D. ( B e ) and ( A l )
    11
    724 Arrange the following in order of increasing reducing property.
    ( N a H, M g H_{2} ) and ( H_{2} O )
    11
    725 An element has atomic number ( 16 . ) It
    will belong to which period of the periodic table?
    ( A cdot 2 )
    B. 3
    ( c cdot 4 )
    D. 5
    11
    726 Which amongst the following can lose 2 electrons to acquire the configuration of argon?
    A. ( N )
    в. ( M g )
    ( c . C a )
    D. ( B e )
    11
    727 The ionisation enthalpy of ( H e^{+} ) ion is
    ( 19.60 times 10^{-18} J ) atom ( ^{-1} . ) The ionisation
    enthalpy of ( L i^{2+} ) ion will be:
    A. ( 84.2 times 10^{-18} ) Jatom( ^{-1} )
    B. ( 44.10 times 10^{-18} ) Jatom ( ^{-1} )
    c. ( 63.20 times 10^{-18} ) Jatom ( ^{-1} )
    D. ( 21.20 times 10^{-18} ) Jatom ( ^{-1} )
    E ( .2 .17 times 10^{-19} mathrm{Jatom}^{-1} )
    11
    728 What is the IUPAC name of an element
    with atomic number 107
    11
    729 Which of the following species has same number of unpaired electrons?
    This question has multiple correct options
    A ( cdot C r^{3} )
    B. ( M n^{2+} )
    ( mathrm{c} cdot F e^{3} )
    D. ( C u^{2} )
    11
    730 A nuclide of an alkaline earth metal
    undergoes radioactive decay by emission of three ( alpha ) -particle in
    succession. The group of the periodic table to which the resulting daughter element would belong is
    A. Group 14
    B. Group 16
    c. Group 4
    D. Group 6
    11
    731 Which of the following elements position’s was not justified in Mendeleev’s periodic table?
    A. Hydrogen
    B. Lithium
    c. Sodium
    D. Potassium
    11
    732 Which element was not known when
    Mendeleev gave his classification?
    A. Germanium
    B. Gallium
    c. Scandium
    D. All of the above
    11
    733 Q. 40 How does the metallic and non-metallic character vary on moving from
    left to right in a period?
    11
    734 State Modern periodic law. 11
    735 What is valency? Write valency of
    hydrogen.
    11
    736 ( N a, M g ) and ( A l ) are the elements of the
    ( 3^{r d} ) period of the Modern Periodic Table having group number 1,2 and 13 respectively. Which one of these elements has the
    (a) highest valency,
    (b) largest atomic radius, and (c)
    maximum chemical reactivity? Justify
    your answer starting the reason for each.
    11
    737 The ( X-X ) bond length is ( 1.00 dot{A} ) and ( C-C ) bond length is 1.54 A. If
    electronegativities of ‘ ( X^{prime} ) and ‘ ( C^{prime} ) are 3.0
    and 2.0 respectively, the ( C-X ) bond
    length is likely to be:
    A. 1.27 an a
    в. 1.18 ( dot{A} )
    c. ( 1.08 AA )
    D. ( 1.28 dot{A} )
    11
    738 Which one of the alkaline earth metals
    shows some anomalous behaviour and
    has same electronegativity as aluminium?
    A. sr
    в. са
    c. Ва
    D. Be
    11
    739 toppr
    Q Type your question
    virtually all or the transıtion metals form dipositive ( (2+) ) cations, along with
    one or more other forms. For example,
    titanium forms ( boldsymbol{T} boldsymbol{i}^{2+} ) ad ( boldsymbol{T} boldsymbol{i}^{4+}, ) and
    cobalt forms ( C o^{2+} ) and ( C o^{3+} )
    The principal exceptions to this
    predominance of cations with a ( 2^{+} )
    charge are scandium and yttrium,
    which form only tripositive cations.
    ( S c^{3+} ) and ( Y^{3+}, ) and copper and silver
    which form cations with a single
    positive charge. ( C u^{+} ) and ( A g^{+} )
    [While copper also forms dipositive
    ( C u^{2+}, ) silver exhibits the single positive
    state essentially exclusively.]
    Which of the following offers a
    POSSIBLE explanation for the existence
    of ( C u^{+} ) and ( A g^{+} ? )
    A. Mendeleev placed copper and silver in Group IB on his original periodic table because they formed compounds with the same combining ratios as elements in Group ( 1 A )
    B. Elemental copper and silver have a single valence electron, which is lost in cation formation
    C. Copper and silver have higher ionization energies than the other transition metals in their respective periods, so are unable to lose more than one electron.
    D. The loss of one electron gives copper and silver noble gas configurations.
    11
    740 The name of the element having atomic number ( 100, ) was adopted in the honour of :
    A. Alfred Nobel
    B. Enrico Fermi
    c. Dmitri Mendeleev
    D. Albert Einstein
    11
    741 ( X ) is an element of the modern periodic table. It is surrounded by elements
    having the atomic numbers 17,34,36
    and ( mathbf{5 3} )
    (i) What is the atomic number of ( X ? )
    (ii) Predict its position in the periodic table.
    (iii) Which among these do not belong to the same period?
    11
    742 Why was there no zero four in the original Mendeleefs Periodic Table? 11
    743 Assertion
    Separation of lanthanides is very
    difficult.
    Reason
    Lanthanides differ only with electronic
    configuration in antipen ultimate shell.
    A. Both Assertion and Reason are correct and Reason is
    the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is correct but Reason is incorrect
    D. Both Assertion and Reason are incorrect
    11
    744 Predict block, group and period of ( boldsymbol{S b} )
    A. Block-p, Period- ( -5, ) Group- 15
    B. Block-p, Period-5, Group-14
    c. Block-s, Period- – 5 , Group- 13
    D. Block- ( s ), Period-5, Group- 11
    11
    745 Which of the following statements is
    not true about Dobereiner’s law of
    triads?
    A. The law was applicable to all known elements
    B. Nitrogen family does not obey the law of triads
    C. Dobereiner’s classification was not very useful
    D. The atomic mass of the central element of each triadd was merely the arithmetic mean of of the atomic masses of other two elements
    11
    746 The most electronegative element
    belongs to:
    A. group 1
    B. group 18
    c. group 17
    D. group 15
    11
    747 Which element has a dicey position in the modern periodic table?
    A. Hydrogen
    B. Helium
    c. Argon
    D. Neon
    11
    748 5. An element X which occurs in the first short period has
    an outer electronic structure s2p1. What are the formula
    and acid-base character of its oxides?
    (a) X0z, basic (b) X,Oz, basic
    (c) X,0,, amphoteric (d) XO,, basic
    11
    749 Noble gases are placed extremely left in the periodic table.
    A . True
    B. False
    11
    750 Which atoms should have smaller value
    of ( (boldsymbol{I} boldsymbol{E})_{1} ? )
    (a) Oxygen or sulphur
    (b) Nitrogen or phosphorus
    ( begin{array}{ll}text { A } cdot text { (a) } S(b) & Pend{array} )
    B. (a) ( O ) (b) ( P )
    c. (a) ( S ) (b) ( N )
    D. Noneofthese
    11
    751 The group number, number of valence electrons, and valency of an element with the atomic number 15
    respectively, of ( boldsymbol{P}, ) are:
    ( mathbf{A} cdot 16,5 ) and 2
    B. 16,6 and 3
    c. 15,5 andb 3
    D. 15,6 and 2
    11
    752 ( ln C u X_{2}, X ) belongs to which group?
    A. group IA
    B. group IIA
    c. group IIIA
    D. group VIA
    E. group VIIA
    11
    753 Describe the main features of
    Mendeleev’s Periodic Table.
    11
    754 In the second period, Li to Ne identify the element
    (a) Most reactive element
    (b) Most non-reactive non-metal
    (c) Largest atomic radius
    (d) With valency equal to 4
    11
    755 The number of elements known in
    Mendeleev’s presented periodic table is:
    ( mathbf{A} cdot 50 )
    B. 90
    c. 63
    D. 102
    11
    756 01 (
    )
    20 Pu.
    Q25. Would you expect the first ionization enthalpies of two isotopes of the same element to be the
    same or different? Justify your answer.
    11
    757 Assertion
    ( H_{2} S ) is more acidic than ( H_{2} O )
    Reason
    ( H-S ) bond is more polar than ( H-O )
    bond.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is correct but Reason is incorrect
    D. Both Assertion and Reason are incorrect
    11
    758 Match the atomic number of the
    transuranium element (in List I) with
    their IUPAC representation in (List II).
    11
    759 In Mendeleev’s periodic table, gaps were left for the element to be discovered
    later on, which of the following elements found a place on the periodic table later
    on:
    A. germanium
    B. chlorine
    c. silicon
    D. oxygen
    11
    760 Which of the following acid is
    strongest?
    ( mathbf{A} cdot H F )
    в. ( H_{2} ) 0
    c. ( N H_{3} )
    D. ( C H_{4} )
    11
    761 In Mendeleev table, the triad of VIII group is :
    ( A cdot ) Ru, Rh, Pd
    B. Cu, Ag, Au
    c. ( N, ) О, ( F )
    D. TI, Pb, Bi
    11
    762 Outermost shell cannot have more than
    electrons.
    A .2
    B. 4
    ( c cdot 6 )
    ( D )
    11
    763 Hydrolysis of urea is an example of
    A. Homogenious reaction
    B. heterogenious reaction
    C. Biomolecular reaction
    D. Both a and b
    11
    764 o seven du wu que
    118. What element has the atom whose K, L, and M shells and 4s subshell
    are filled completely and 4p subshell is half-filled?
    11
    765 Column II give the group to which element in column I belong, match
    them correctly.
    11
    766 The properties of the elements, as well as the formulae and properties of their compounds depend in a periodic manner on the atomic weights of the elements. This periodic law was given by :
    A. J. Lothar Meyer
    B. John A. R. Newlands
    c. Dobernier
    D. D.I. Mendleev
    11
    767 Which among the following elements has the largest atomic radii?
    A. ( N a )
    в. ( M g )
    c. ( K )
    D. ( C a )
    11
    768 According to the Newlands’ law of octaves, the properties of fluorine are similar to those of
    A. hydrogen
    B. lithium
    c. sodium
    D. potassium
    11
    769 The law of triads was given by :
    A. Dobereiner
    B. Lewis
    c. Mendeleev
    D. Dalton
    11
    770 The correct order of atomic radii is :
    ( mathbf{A} cdot C e>S m>Y b>L u )
    в. ( S m>C e>L u>Y b )
    c. ( L u>Y b>S m>C e )
    ( mathrm{D} cdot S m>Y b>C e>L u )
    11
    771 In periodic table, the period number
    indicates the number of:
    A. neutrons
    B. protons
    c. electrons
    D. none of the above
    11
    772 The type of elements present in group 18[0] are :
    A . alkal
    B. alkaline
    c. transition
    D. noble gases
    11
    773 What is the valency of potassium with atomic number ( 19 ? )
    ( mathbf{A} cdot mathbf{0} )
    B.
    ( c cdot 2 )
    ( D )
    11
    774 Select correct statement(s):
    This question has multiple correct options
    A. ( C e, P r ) and ( N d ) are ( f ) -block elements
    B. ( C u, P d ) and ( N i ) are d-block elements
    ( mathbf{c} cdot C uleft([A r] 3 d^{10} 4 s^{1}right) ) and ( Kleft([A r] 4 s^{1}right) ) have been placed in sblock.
    D. ( S i, G e ) and ( A s ) are metalloids
    11
    775 The element eka-silicon predicted by Mendeleev is :
    A . Ge
    в. Ga
    ( c cdot A )
    ( D cdot s )
    11
    776 When ( L ) is heated with iron metal, it
    forms a compound ( F e L . ) What chemical term would you use to describe the change undergone by ( L ? )
    11
    777 Which among the following elements
    has largest atomic size?
    ( A cdot B )
    в. А।
    ( c cdot ) Ga
    D. In
    11
    778 Atomic size of ( N e>F e )
    A. True
    B. False
    11
    779 Q38. Considering the elements B, AI, Mg and K. the correct order of their metallic character is:
    (a) B > Al > Mg > K (6) Al > Mg > B > K (c) Me > Al > K> B (d) K> Mg > Al > B
    11
    780 The arrangement of elements in a group of three is known as 11
    781 Which of the following elements never show positive oxidation number?
    A.
    B. Fe
    ( c cdot ) Ga
    ( D )
    11
    782 There are …….. periods in the Modern Periodic Table.
    A. 7
    B. 18
    ( c cdot 9 )
    ( D )
    11
    783 Consider the following statements.
    (I) Rutherford’s name was associated
    with the development of periodic table.
    (II) A metal M having electronic configuration ( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1} )
    is d-block element.
    (III) Diamond is an element.
    (IV) The electronic configuration of the most electronegative element is ( 1 s^{2} 2 s^{2} 2 p^{5} )
    The correct statements are:
    A. ।, ॥।, IV
    B. ।, ॥, ॥ा, IV
    c. ॥, IV
    D. I, III, IV
    11
    784 LS 650
    Q18. What are the various factors due to which the ionization enthalpy of the main group elements
    tends to decrease down the group?
    11
    785 Which of the following will have
    maximum electron affinity?
    ( mathbf{A} cdot 1 s^{2} 2 s^{2} 2 p^{5} )
    B ( cdot 1 s^{2} 2 s^{2} 2 p^{6} )
    ( mathbf{C} cdot 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5} )
    D. ( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} )
    11
    786 The most electronegative element of period-3 is :
    A . ( A r )
    B. ( S )
    ( c cdot s i )
    D. ( C l )
    11
    787 At the time of Newlands, how many elements were known?
    ( mathbf{A} cdot 50 )
    B. 52
    c. 54
    D. 56
    11
    788 Upto which element, the law of octaves
    was applicable?
    A. oxygen
    B. Calcium
    c. cobalt
    D. Potassium
    11
    789 Pentavalence in phosphorus is more stable when compared to that of nitrogen even though they belong to same group is due to:
    A. reactivity of phosphorus
    B. inert nature of nitrogen
    c. hydrogen and sulphurous acid
    D. large size of phosphorus atom
    11
    790 26 Identify the group and valency of the element having atomic number
    119. Also predict the outermost electronic configuration and write the
    general formula of its oxide.
    11
    791 Which of the following reasons corresponds to decrease in IP value
    from top to bottom in a group?
    A. Decrease in screening effect
    B. Increase in atomic number
    c. Increase in screening effect
    D. Decrease in nuclear charge
    11
    792 State the electronic configuration for Boron ( [p=5, n=6] )
    A . 2,3
    B. 5, 10
    c. 5,12
    D. 5,1
    11
    793 Law of octaves stated:
    A. every eighth element had properties similar to the first element
    B. every third element had properties similar to the first element
    C. the properties of the middle element were in between the other two members
    D. the properties of the elements were repeated after regular intervals of 3,4 or 8 elements
    11
    794 Let us suppose that you have discovered a new element of the atomic
    number ( 162, ) which you choose to name
    khalidium (Kh). Assume that the
    normal order of filling of orbitals still prevails in the eighth period.

    The new type of orbital used in Kh that
    is not used in any known atom is:
    ( A cdot h )
    B.
    ( c cdot f )
    D.

    11
    795 The pair with minimum difference in electronegativity is
    A . F, C
    в. с, н
    c. ( P, H )
    D. Na, cs
    11
    796 The amount of energy when a million atoms of iodine are completely
    converted into ( I^{-} ) ions in the vapor
    state according to the equation, ( boldsymbol{I}_{(g)}+boldsymbol{e}^{-} rightarrow boldsymbol{I}_{(g)}^{-} ) is ( 4.9 times 10^{-13} mathrm{J} . ) What
    would be the electron gain enthalpy of
    iodine in terms of ( k J ) mol ( ^{-1} ) and ( e V ) per
    atom?
    ( mathbf{A} cdot 295,3.06 )
    в. -295,-3.06
    C .439,5.09
    D. -356,-7.08
    11
    797 ( P b O_{2} ) is a reducing agent.
    A. True
    B. False
    11
    798 Which of the following element would lose an electron easily?
    ( mathbf{A} cdot M g )
    в. ( N a )
    c. ( K )
    D. ( C a )
    11
    799 In ( S ) and ( P ) -block elements the oxidation
    state changes by 2 units. But in transition elements, it changes by 1 unit
    of
    1. Explain.
    11
    800 Atomic wt. of ( P ) is 31 and ( S b ) is 120 . What
    will be the atomic wt. of As, as per Dobernier triad rule?
    A . 151
    B. 75.5
    c. 89.5
    D. Unpredictable
    11
    801 The structure of sodium atom is shown
    in the figure given above. Identify the
    correct statement.
    An atomic sodium
    ( A . ) is a non-metal
    B. reacts vigorously with wate
    ( c . ) is stored in oil to avoid contact with moisture
    D. all of the above
    11
    802 Which of the following statement(s)
    is/are correct about the modern
    periodic table?

    This question has multiple correct options
    A. It consists of ( s, p, d ) and ( f ) blocks
    B. The energy levels filling order in 6 th period is ( 6 s, 4 f, 5 d ) and ( 6 p )
    C . III ( B ) group does not contain maximum number of elements
    D. It consists only metals

    11
    803 The group number of element with atomic number 7 in the periodic table
    is:
    ( A cdot 2 )
    B. 18
    c. 15
    D. 14
    11
    804 State Dobereiner’s Triads giving one
    example.
    11
    805 The first I.P. values in electron volts of
    nitrogen and oxygen atoms are respectively given by :
    A ( .14 .6,13.6 )
    в. 13.6,14.6
    c. 13.6,13.6
    D. 14.6,14.6
    11
    806 Q30. Assign the position of the element having outer electronic configuration,
    (1) ns np for n = 3 (ii) (n-1) {ns for n = 4 and (iii) (n -2) f (1 – 1) dns for
    n = 6 in the periodic table?
    11
    807 Choose the option which describes best this statement:
    “The modern periodic table is based upon”.
    A. Atomic mass of the elements
    B. Number of neutrons in the nucleus
    c. Number of isotopes of an element
    D. Oxidation states
    E. Number of protons in the nucleus
    11
    808 Assertion
    Li and ( M g ) shows diagonal relationship.
    Reason
    Li and ( M g ) are diagonal to each other in the Periodic table.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    809 Pauling scale Linus Pauling: Phenomenon of electronegativity Relative electronegativities of two atoms in a molecule
    ( boldsymbol{E} boldsymbol{N}(boldsymbol{X})-boldsymbol{E} boldsymbol{N}(boldsymbol{Y})=mathbf{0 . 1 0 2}(triangle mathbf{1} / 2) . mathbf{1} )
    0.02 is conversion factor between ( k J )
    and eV is:
    11
    810 Which of the following is non-existing?
    A. ( mathrm{H}_{2} )
    в. ( mathrm{O}_{2} )
    c. ( mathrm{N}_{2} )
    D. He ( _{2} )
    11
    811 Phosphorus has oxidation state of +3 in:
    A. phosphorus acid
    B. orthophosphoric acid
    c. metaphosphoric acid
    D. pyrophosphoric acid
    11
    812 The elements in the middle of the
    periodic table are called:
    A. metalloids
    B. transition elements
    c. rare earth element
    D. noble gases
    11
    813 What relation about elements did
    Dobereiner want to establish?
    11
    814 In terms of energy 1 u is equal to?
    begin{tabular}{l}
    A. ( 100 J ) \
    hline
    end{tabular}
    B. ( 931.1 k c a l )
    c. ( 931.1 mathrm{MeV} )
    D. ( 10^{7} ) erg
    11
    815 Which among the following elements is metalloid?
    A. Berellium
    B. Barium
    c. Boron
    D. Bismuth
    11
    816 Which of the following elements is oxidised by fluorine and not by
    chlorine?
    A. Sodium
    B. Aluminum
    c. sulphur
    D. oxygen
    11
    817 The correct order of variation in the
    sizes of atoms is:
    A. ( B e>C>F>N e )
    в. ( N e>F>C>B e )
    c. ( N e>B e>C>F )
    D. ( F>N e>B e>C )
    11
    818 sily as compared to
    Q6. Explain why chlorine can be converted into chloride ion more easily as com
    ion from fluorine?
    Ans. Flectron main anth
    Chi more negative than that of
    11
    819 Total number of inert gases among the following is :
    ( mathrm{H}, mathrm{He}, mathrm{Ne}, mathrm{F}, mathrm{Ar}, mathrm{Kr}, mathrm{K} )
    A . 1
    B. 2
    ( c cdot 3 )
    D. 4
    11
    820 State any three demerits of Mendeleev’s
    periodic table.
    11
    821 Considering the elements ( F, C I, O ) and ( N ) the correct order of their chemical
    reactivity in terms of oxidizing property is:
    ( (a) F>C mid>0>N )
    ( (b) F>0>C l>N )
    ( (c) C mid>F>0>N )
    ( (d) O>F>N>C l )
    11
    822 06. An anion A*has 18 electrons. Write the atomic number of A. 11
    823 The effective nuclear charge for the outermost electron of oxygen atom is
    A . 4.55
    B. 5.35
    ( c cdot 6.68 )
    D. None of these
    11
    824 Question 6. Why is the highest oxidation state of a metal exhibited in its
    oxide or fluoride only?
    Consider high electronegativity of Fand O.
    11
    825 Choose the incorrect statement about
    effective nuclear charge.
    A. ( Z_{e f f}=Z-sigma(sigma text { is Slater’s screening constant }) )
    B. ( Z_{text {eff}} ) increases as we move across the period
    C. ( Z_{text {eff}} ) decreases from top to bottom in a group
    D. ( Z_{text {eff}} ) is constant or almost constant for f-block elements
    11
    826 Assertion
    Compounds of ( boldsymbol{H} boldsymbol{g}^{2+} ) ions having an ionic radius of 116 pm are more covalent in character than those of
    ( C a^{2+} ) ions with almost identical size
    ( 114 p m) ) and the same charge.
    Reason
    For two ions of the same size and
    charge, one with an ( (boldsymbol{n}-mathbf{1}) boldsymbol{d}^{10} boldsymbol{n s}^{mathbf{0}} )
    electronic configuration will be more
    polarizing than a cation with an ( (n- )
    1) ( s^{2}(n-1) p^{6} n s^{0} ) electronic
    configuration.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion.
    B. Both Assertion and Reason are correct, but Reason is not the correct explanation for Assertion.
    C. Assertion is correct, but Reason is incorrect
    D. Assertion is incorrect, but Reason is correct.
    11
    827 The Russian chemist Dmitri Mendeleev
    is generally credited with organizing the chemical elements into a
    comprehensive periodic table in large part due to the fact that he was able to
    use his table to predict the existence of elements, like gallium, that were not known at the time ( (1872), ) but were discovered later.

    Which is the best explanation for why Mendeleev was unable to predict the existence of the noble gases (group 18
    )?
    A. Noble gases are not found on Earth
    B. Noble gases are stable and very unreactive, and therefore, have few observable properties
    c. Noble gases are synthetic elements and do not occu
    D. Noble gases are very reactive and do not exist as stable elements

    11
    828 In ground state, all the elements of group 13 of the periodic table are having same number of :
    A . nuclear particles
    B. occupied principal energy levels
    c. electrons
    D. valence electrons
    E . neutrons
    11
    829 ( (I E)_{1} ) of Be is greater than that of B but
    ( (I E)_{2} ) of ( (B) ) is greater than that of Be.If
    true enter 1 , else 0 .
    11
    830 Which element has the symbol ( S b ? )
    A. Arsenic
    B. Antimony
    c. Lead
    D. Seaborgium
    E. Silver
    11
    831 When ammonium vanadate is heated
    with oxalic acid solution, a substance ( mathbf{Z} )
    is formed. A sample of Z was treated
    with ( K M n O_{4} ) solution in hot acidic
    solution. The resulting liquid was
    reduced with ( S O_{2}, ) the excess ( S O_{2} )
    boiled off and the liquid again titrated
    with same ( K M n O_{4} . ) The ratio of
    volumes of ( K M n O_{4} ) used in the two
    titrations was ( 5: 1 . ) What is the
    oxidation state of vanadium in
    substance Z? Given than ( K M n O_{4} )
    oxidize all oxidation state of vanadium
    to vanadium (+5) and ( S O_{2} ) reduces
    ( V(+5) ) to ( V(+4) )
    11
    832 Which of the following statement is
    correct?
    This question has multiple correct options
    A . oxidizing power order: ( operatorname{SiCl}_{4}<operatorname{SnCl}_{4}

    R b B r>K B r>N a B r>L i B r )
    c. The ionic character of lead(II) halides decrease with the increase in atomic no. of halogen
    D. The oxidation state of ( T l ) in ( T l I_{3} ) is +3

    11
    833 Isobars have same mass numbers
    becausetheir nuclei contain
    equalnumber of
    A. protons
    B. electrons
    c. neutrons
    D. nucleons
    11
    834 The correct order of stability of ( boldsymbol{A l}^{+}, boldsymbol{A l}^{+mathbf{2}}, boldsymbol{A l}^{+mathbf{3}} mathbf{i s} )
    A ( cdot A l^{+3}>A l^{+2}>A l^{+} )
    B. ( A l^{+2}>A l^{+3}>A l^{+} )
    c. ( A l^{+2}A l^{+} )
    D. ( A l^{+3}>A l^{+}>A l^{+} )
    11
    835 7. Which of the following atoms has the lowest ionisation
    potential?
    (a) 0
    (b) 4N
    (c) 133 Cs too lonit (d) to Ar (AIEEE 2003)
    11
    836 ( 2^{n} d ) separation energy of an electron in
    H atom?
    A. 27.2 ev
    B. 1.51 ev
    c. 3.4 ev
    D. 13.6 ev
    11
    837 ( c )
    Using the information ab bove, complete
    the following

    Metal atoms tend to have a maximum
    of electrons in the
    outermost energy level

    11
    838 The number of elements in each of the
    inner transition series is :
    ( A cdot 2 )
    B. 8
    c. 10
    ( D cdot 14 )
    11
    839 Refer to the Periodic table and
    identify the halogen element in the fifth
    period among following.
    A . ( I )
    в. ( C l )
    ( c . B r )
    D. None of these
    11
    840 In the Modern Periodic Table, calcium (atomic number 20 ) is surrounded by elements with atomic numbers
    12,19,21 and ( 38 . ) Which of these have physical and chemical properties resembling calcium?
    11
    841 Find the ratio of the following: ( (operatorname{Max}(mathrm{M}) ) ( +operatorname{Max}(mathrm{N})) /(operatorname{Max}(mathrm{K})+operatorname{Max}(mathrm{L})) ) where
    Max denotes the maximum number of
    electrons. ( K, L, M, N ) represent the shells.
    A . 4
    B. 5
    ( c .6 )
    ( D .7 )
    11
    842 Arrange the following elements in increasing order of their atomic radii ( boldsymbol{L} boldsymbol{i}, boldsymbol{B} boldsymbol{e}, boldsymbol{F}, boldsymbol{N} )
    A. ( N<F<B e<L i )
    B. ( F<N<L i<B e )
    c. ( F<B e<N<L i )
    D. ( F<N<B e<L i )
    11
    843 List the different scales of
    electronegativity and briefly describe the theoretical basis behind each.
    11
    844 In the given square ( P, Q, R, S ) with atomic number is written are
    metalloids. About this the 4 statements
    are given below. Select the correct
    option of the true statements.
    (a) Element after square ( P ) is a non-
    metal
    (b) Square ( R ) represents metalloid
    (c) Element just before square ( R ) is a metalloid
    ( (d) ) Element just before square ( S ) is a non-metal
    ( A cdot(a),(b) ) and ( (c) )
    в. ( (a),(b) ) and ( (d) )
    c. ( (b) ) and ( (c) )
    D. ( (a),(b),(c) ) and ( (d) )
    11
    845 Increase in nuclear charge of an atom decreases the tendency of the atom to loose electrons.
    A. True
    B. False
    11
    846 An element has atomic number 19
    Where would you expect this element in
    the periodic table and why?
    11
    847 M(g) + I.E. → M (g) + e
    013. The electronic configuration of an element is 1s 2s 2p 3s 3p 4s”. Locate the element in the
    periodic table.
    11
    848 What would be the IUPAC name of
    element with a atomic number ( 120 ? )
    A. Unbinilium
    B. Unnilhexium
    c. Unnilseptium
    D. Ununnilium
    11
    849 In a period, elements are arranged
    strictly in a sequence of:
    A. decreasing charge in the nucleus
    B. increasing charge in the nucleus
    C. constant charge in the nucleus
    D. equal charge in the nucleus
    11
    850 In which of the following period a maximum number of 32 elements are
    present? This question has multiple correct options
    ( mathbf{A} cdot 4^{t h} )
    B. ( 6^{text {th }} )
    ( c cdot 3^{r d} )
    D. ( 7^{t h} )
    11
    851 S-block elements are:
    A. Elements of group I-A and III-B.
    B. Elements of group I-A and II-A.
    C. Elements of group I-A and I-B.
    D. Elements of group I-A and II-B.
    11
    852 Q. 30 Choose the correct order of atomic radii of fluorine and neon (in pm) out
    of the options given below and justify your answer.
    (a) 72,160 (b) 160, 160 (c) 72, 72 (d) 160, 72
    11
    853 An element M belongs to the group 1 and period 3 of the modern periodic table. Out of the following statement, which is
    the true about ‘M’?
    A. It forms an acidic oxide having formula ( M_{2} O_{3} )
    B. It is a non-metal
    c. It is highly electro positive in nature
    D. It has a valency of three
    11
    854 Which element among those listed below, has the greatest electronegativity?
    A . In
    B. ( I )
    c. ( S b )
    D. ( T e )
    E . ( S n )
    11
    855 Boron is diagonally related to:
    A. boron
    B. aluminium
    c. magnesium
    D. silicon
    11
    856 Transition elements are also known as
    ( mathbf{A} cdot d- ) block elements
    B. ( f ) – block elements
    c. ( s ) – block elements
    D. None of these
    11
    857 Which group element has greater tendency to form positive ions than elements of group IIA?
    A . IA
    B. IVA
    ( c cdot v B )
    D. None of these
    11
    858 Write the correct alternatives:
    According to Mendeleev’s periodic law, properties of elements are periodic
    function of their.
    A. Atomic number
    B. Atomic masses
    c. Densities
    D. Boiling points
    11
    859 Three elements ( A, B ) and ( C ) belong to
    the same group of the modern periodic table such that the difference in atomic
    weight of ( A ) and ( B ) is equal to the
    difference in atomic weight of ( B ) and ( C ) The sum of atomic weights of elements ( A ) and ( C ) is 46 and that of ( A ) and ( B ) is 30
    Identify elements ( A, B ) and ( C . )
    11
    860 State Newlands law of Octaves. 11
    861 Q. 22 Ionic radii vary in
    (a) inverse proportion to the effective nuclear charge
    (b) inverse proportion to the square of effective nuclear charge
    (c) direct proportion to the screening effect
    (d) direct proportion to the square of screening effect
    11
    862 Electro negativity is expressed in
    Scale.
    A. paulings
    B. sorensens
    c. rutherford
    D. none of these
    11
    863 Energy required for the ionisation reactions are shown:
    ( boldsymbol{N a}(boldsymbol{g}) stackrel{+E_{1}}{rightarrow} boldsymbol{N} boldsymbol{a}^{+}(boldsymbol{g}) )
    ( M g(g) stackrel{+E_{2}}{rightarrow} M g^{+}(g) ) and
    ( boldsymbol{N} boldsymbol{a}^{+}(boldsymbol{g}) stackrel{+boldsymbol{E}_{3}}{rightarrow} boldsymbol{N} boldsymbol{a}^{2+}(boldsymbol{g}) )
    Then the correct order of absorbed
    energy is :
    A. ( E_{1}>E_{2}>E_{3} )
    в. ( E_{3}>E_{1}>E_{2} )
    c. ( E_{2}>E_{3}>E_{1} )
    D. ( E_{3}>E_{2}>E_{1} )
    11
    864 Example of noble gas is
    A. Helium
    B. Argon
    c. xenon
    D. all of these
    11
    865 The horizontal rows in Mendleev’s table
    were called :
    A. groups
    B. rows
    c. periods
    D. none of the above
    11
    866 After the classification of elements
    study of elements
    become
    A. difficult
    B. easy
    c. both ( A ) and ( B )
    D. None of these
    11
    867 Equivalent weight of ( B r_{2} ) is 96 in the following disproportionation reaction:
    ( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{B} boldsymbol{r}^{-}+boldsymbol{H}_{2} boldsymbol{O}+? )
    (oxidized product) The oxidation state of Br in the oxidized product is ( (mathrm{Br}=80) )
    11
    868 The first periodic law stated by
    Mendeleev was:
    A. there is no correlation in the properties and atomic weights of the elements
    B. the properties of the elements are a periodic function of their atomic numbers
    C. the properties of the elements are a periodic function of their atomic weights
    D. the properties of the elements are a periodic function of their empirical formula
    11
    869 An ion is an atom with an electric
    charge due to a loss or gain of an electron.
    Which of the following is the electron configuration of a ground state of the most common alkali metal ion?
    ( mathbf{A} cdot 1 s^{2} 2 s^{2} )
    B. ( 1 s^{2} 2 s^{text {। }} )
    C ( cdot 1 s^{2} 2 s^{2} 2 p^{6} )
    D. ( 1 s^{2} 2 s^{2} 2 p^{6} s s^{2} 3 p^{6} 3 d )
    11
    870 Consider the following statements and arrange in the order of true/false as given in the codes. ( S_{1}: ) Long form of periodic table completely helps in predicting the
    oxidation state of elements.
    ( S_{2}: ) Metallic and covalent radii of potassium are 203 pm and 230 pm respectively.
    ( boldsymbol{S}_{3}: ) Formation of ( boldsymbol{S} boldsymbol{e}^{2-} ) and ( boldsymbol{A} boldsymbol{r}^{-}, ) both
    the absorption of energy.
    A . FFT
    в. गाग
    c. ( pi mathrm{F} )
    D. TFT
    11
    871 Assertion
    Formal charges help in selection of the lowest energy structure from a number of possible lewis structure.
    Reason
    show +1 formal charge on central 0 marked 1.
    A. Both Assertion and Reason are true and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are true but Reason is not the correct explanation for Assertion
    c. Assertion is true statement but Reason is false
    D. Both Assertion and Reason are false statement.
    11
    872 Which will have graded property
    particular to ( boldsymbol{E} cdot boldsymbol{C} cdot boldsymbol{1} boldsymbol{s}^{2} boldsymbol{2} boldsymbol{s}^{2} boldsymbol{2} boldsymbol{p}^{6} boldsymbol{3} boldsymbol{s}^{2} boldsymbol{3} boldsymbol{p}^{boldsymbol{6}} boldsymbol{4} boldsymbol{s}^{1} ) ?
    ( mathbf{A} cdot[A r] 3 d^{10} 4 s^{1} )
    B . ( [K r] 4 d^{10} 5 s^{1} )
    c. ( [K r] 5 s^{1} )
    D. all of these
    11
    873 The ionization enthalpies, ( (I E)_{1} ) and
    the ( (I E)_{2} ) in ( mathrm{kJ} mathrm{mol}^{-1} ) of a few elements designated by Roman numerals are shown below:
    ( begin{array}{lll}text { Element } & (I E)_{1} & (I E)_{2} \ text { A } & text { 2372 } & 5251 \ text { B } & 520 & 7300 \ text { c } & 900 & text { 1760 } \ text { D } & text { 1680 } & text { 3380 }end{array} )
    Which of the above elements form a
    stable binary halide of the formula
    [
    boldsymbol{M} boldsymbol{X}_{2} ?
    ]
    A. ( A )
    в. ( B )
    c. ( C )
    D. ( D )
    11
    874 Who is the founder of the law of triads? 11
    875 Which of the following general electronic configuration for transition
    elements is NOT correct?
    This question has multiple correct options
    A ( cdot(n+1) s^{1-2} n d^{1-30} )
    B . ( left.n s^{1-2}(n-1) d^{1-10} text { (Where } n=2,3,4, ldots ldotsright) )
    C. ( n s^{1-2}(n-1) s^{2} p^{6} d^{1-10} )
    D ( cdot(n-1) d^{1-10} n s^{0-2} )
    11
    876 The group number of the element with
    atomic number 37 is:
    11
    877 Which of the following elements have
    the lowest value of ( I E_{1} ? )
    A ( . P b )
    в. ( S n )
    ( c . s i )
    D. ( C )
    11
    878 An element X has 7 electrons in its shell. What is true about the element ( x )
    ( ? )
    I. It belongs to period 9 of modern periodic table.
    II. Its atom contains 9 protons.
    III. It has a valency of 1
    IV. Its atoms can accept an electron to acquire noble gas configuration.
    ( A cdot(1) ) and (11)
    B. (II), (III), (IV)
    c. (III) and (IV)
    D. (II) and (IV)
    11
    879 In Mendeleev’s periodic table, the elements were arranged in the increasing order of their atomic
    masses. However, cobalt with atomic
    mass of 58.93 amu was placed before nickel having an atomic mass of 58.69 amu. Reason for the same is that:
    A. the elements with similar size can be grouped togethe
    B. the elements with different properties can be grouped together
    c. the elements with similar properties can not be grouped together
    D. the elements with similar properties can be grouped together
    11
    880 Q3. Give reasons:
    sodium is lower than that of magnesium whereas IE, of sodium is higher
    than that of magnesium.
    (ii) Noble gases have positive value of electron gain enthalpy.
    that of sodium. For these
    11
    881 Which group elements of the modern periodic table were placed along with alkali metals in Mendeleeff table?
    ( A cdot 1 B )
    B. ॥ в
    ( c cdot | A )
    D. IA
    11
    882 Arrange the following in the ilncreasing hydrated ion size: ( boldsymbol{C} boldsymbol{s}_{boldsymbol{a q}}^{+}<boldsymbol{R} boldsymbol{b}_{boldsymbol{a q}}^{+}< )
    ( boldsymbol{K}_{a q}^{+}<boldsymbol{N} boldsymbol{a}_{a q}^{+} )
    If true enter 1 , else enter 0 .
    ( A )
    11
    883 Complete the electronic configuration
    of a chloride ion.
    ( mathbf{1} s^{2} )
    11
    884 If an element ( X ) is placed in group ( 14, ) the formula its chloride is:
    A. ( X C l )
    в. ( X C l_{2} )
    c. ( x C l_{3} )
    D. ( X C l_{4} )
    11
    885 The electronic configuration, ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6}, 3 d^{9} ) represents a
    A. Metal atoms
    B. non metals atom
    c. non-metallic anionic
    D. metallic cation
    11
    886 The second I.P. for alkali metals shows a
    jump while the third I.P. for alkaline earth metal shows a jump. Explain.
    11
    887 Which element has the symbol Ti?
    A. Tin
    B. Leadd
    c. Titanium
    D. Thallium
    E. Technetium
    11
    888 For the properties mentioned, the correct trend for the different species
    is :
    A. inert pair effect – ( A l>G a>I n )
    B. first ionization enthalpy ( -B>A l>T l )
    C . strength as Lewis acid – ( B C l_{3}>A l C l_{3}>G a C l_{3} )
    D. oxidising property ( -A l^{+3}>I n^{+3}>T l^{+3} )
    11
    889 SUSO
    Q. 23 An element belongs to 3rd period and group 13 of the
    Which of the following properties will be shown by the element?
    (a) Good conductor of electricity (b) Liquid, metallic
    (c) Solid, metallic
    (d) Solid, non-metallic
    11
    890 Q. 43 Match the correct atomic radius with the element.
    Element Atomic radius (pm)
    74
    Be
    88
    111
    OZ
    Thinking Process
    11
    891 An atom with an electron configuration of ( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4} ) will probably exhibit an oxidation state of:
    ( A cdot+2 )
    в. -2
    ( c cdot+3 )
    D. –
    ( E cdot+5 )
    11
    892 Which element has the highest electronegativity?
    A. ( K )
    в. ( C a )
    c. ( B r )
    D. ( K r )
    E. ( Z n )
    11
    893 POUC
    TUICUUILUL LUI QUUUC LLLLEEN
    Q2. Why is ionization enthalpy of nitrogen greater than that of oxygen
    11
    894 The energy needed to remove one electron from unipositive ion is abbreviated as:
    ( mathbf{A} cdot 1^{s t} I cdot P )
    B. ( 3^{r d} ) I.P.
    ( mathbf{c} cdot 2^{n d} I . P )
    D. ( 1^{s t} ) E.A.
    11
    895 The valency of element with atomic
    number 10 is:
    A . 0
    B.
    ( c cdot 2 )
    ( D )
    11
    896 How does ionization enthalpy vary in a group and a period? 11
    897 The atomicity of a noble gas is:
    ( A cdot 2 )
    B.
    ( c cdot 0 )
    D.
    11
    898 The diagram represents an atom ‘X!
    Answer the following.

    Atom ‘X’ will lose electrons to become
    ( boldsymbol{X}^{1+} )
    A. True
    B. False

    11
    899 The element ( X ) with electronic
    configuration 2,8,8,2 belongs to
    A ( cdot 2^{n d} ) Period
    B. ( 3^{r d} ) Period
    ( mathbf{c} cdot 4^{t h} ) Period
    D. ( 5^{text {th}} )period
    11
    900 In Period 3 of the Periodic Table, element
    B is placed to the left of element A. On the basis of this information, choose
    the correct word from the brackets of
    complete the following statement.
    (i) The element B would have(lower/higher) metallic character
    than ( A )
    (ii) The element A would probably have(lesser/higher) electron affinity than B.
    (iii) The element A would have(greater/smaller) atomic size than
    B.
    11
    901 Assuming that 113 elements are there in the periodic table now, what would be the group and period to which newly added element belongs?
    A. IVA group, 7th period.
    B. VIA group, 7th period.
    c. va group, 7th period.
    D. VIIA group, 6th period.
    11
    902 The breaking of which of the following
    bond is most endothermic?
    A ( . F-F )
    в. ( C l- ) Сl
    c. ( B r-B r )
    ( mathbf{D} cdot I-I )
    11
    903 0. 16 Which of the following sequences contain atomic numbers of only
    representative elements?
    (a) 3, 33, 53, 87
    (b) 2, 10, 22, 36
    (c) 7, 17, 25, 37, 48
    (d) 9, 35, 51, 88
    11
    904 What type of bond is formed, if the atoms involved has electronegativity difference as ( 2 ? )
    A. Metallic
    B. Covalent
    c. lonic
    D. Polar covalent
    E. Hydrogen bonding
    11
    905 A paste of substance ( A ) is used to
    decorate the ceiling of your home.
    Write the reaction of substance ( A ) with
    ( boldsymbol{H}_{2} boldsymbol{O} )
    11
    906 Arrange the following in the increasing strength: ( S<C l<N<O<F )
    if true enter 1 , else enter 0 .
    11
    907 In the long form of periodic table, elements are arranged in the increasing order of :
    A. atomic mass
    B. atomic number
    C. mass number
    D. metallic character.
    11
    908 Which group elements are the most reactive among the non-metals?
    A . 15 th
    B. 16th
    c. 17 th
    D. 18th
    11
    909 What were the limitations of Newlands’
    classification?
    A. It was applicable only for lighter elements
    B. He adjusted two elements on the same place
    C. The pattern was only observed up to calcium
    D. All of the above
    11
    910 Which of the following statements are
    correct?
    A. The second ionization enthalpy of oxygen element is greater than that of the fluorine element.
    B. The first ionization enthalpy of phosphorus is greater than that of aluminium.
    C. The first ionization enthalpy of aluminum is slightly greater than that of gallium.
    D. The first ionization enthalpy of ( B ) is less than that of Be.
    11
    911 When you move from left to right across a period, or row, of the periodic table which one decreases?
    A. Reactivity
    B. Ionization energy
    c. Electron affinity
    D. Number of valence electrons
    E. Atomic radius
    11
    912 Screening effect of inner shells decreases the effective nuclear charge. The order of screening effect of subshells is ( s>p>d>f ) State whether the given statement is
    true or false.
    A. True
    B. False
    11
    913 Pickout among the following:
    ( mathrm{LI}^{-}, mathrm{Be}^{-}, mathrm{C}^{-}, ) species which is least
    stable?
    11
    914 Which pair of atomic numbers represents s-block elements?
    A . 7, 15
    B. 6, 12
    c. 9,17
    D. 3, 12
    11
    915 What is the symbol of atomic number
    ( 117 ? )
    A. Uus
    B. Uns
    c. uno
    D. uut
    11
    916 The group number of the element with
    atomic number 96 is 3
    If true enter 1 , else enter 0 .
    11
    917 The IIA group metal ion having ( 6 s^{2}, 6 p^{6} ) as outer electron configuration is:
    A ( cdot C a^{2} )
    в. ( S a^{2} )
    ( c cdot B a^{2} )
    D. ( R a^{2} )
    11
    918 The major constituent of freshly obtained molasses is:
    A. sucrose
    B. fructose
    c. glucose
    D. methanol
    11
    919 Representative elements belong to:
    A. ( s ) -and ( p ) – block
    B. ( d- ) block
    c. ( d ) and f block
    D. ( f ) – block
    11
    920 What are the main feature of
    Mendeleev’s periodic table?
    11
    921 The first ionization energy for ( N a ) is ( 495 k J / m o l )
    The BEST estimate for sodium’s second
    ionization energy would be
    A. ( 367 k J / ) mol
    в. ( 584 k J / m o l )
    c. ( 690 k J / ) mol
    D. ( 4560 k J / ) mol
    11
    922 An element has 12 neutrons in its
    nucleus. To which group of the periodic table it will belong?
    ( A )
    B. 2
    ( c cdot 6 )
    D. Impossible to predict
    11
    923 A type of ion found in sodium acetate
    is :
    A ( . x^{+} )
    B. ( X^{2+} )
    ( c cdot X^{3+} )
    D. ( X O_{3}^{2-} )
    E ( cdot X O_{4}^{2-} )
    11
    924 Stability of ions of ( G e, S n ) and ( P d ) will be in the order:
    This question has multiple correct options
    A. ( G e^{2+}<S n^{2+}

    S n^{4+}>P b^{4+} )
    ( mathrm{c} cdot S n^{4+}>S n^{2} )
    ( D cdot P b^{2+}>P b^{4} )

    11
    925 Elements which occupied the position in the Lother Meyer curve, on the peaks,
    were:
    A. alkali metals
    B. highly electropositive elements
    c. elements having large atomic volume
    D. all of the above
    11
    926 What were the criteria used by Mendeleev in creating his period. Why do you think the noble gases are placed
    in a separate group?
    11
    927 Paulings values of electronegativities are dependent upon:
    A. ionisation potentials
    B. bond energies
    c. electron affinities
    D. atomic radii
    11
    928 Name the following metals:
    A metal present in period ( 3, ) group 1 of the periodic table
    11
    929 The highest ionization energy is exhibited by:
    A. halogens
    B. alkaline earth metals
    c. transition metals
    D. noble gas
    11
    930 How many valence electrons are present in Eka – aluminium?
    A.
    B. 2
    ( c cdot 3 )
    ( D )
    11
    931 Statement I: Atomic radius generally increases as you move across the periodic table from left to right. Statement II: The atomic number is
    increasing from left to right as you move across the periodic table
    A. Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement
    B. Both Statement I and Statement II are correct, but Statement II is not the correct explanation of Statement I.
    c. Statement lis correct, but Statement II is incorrect
    D. Statement I is incorrect, but Statement II is correct
    11
    932 The high ionistion potential of magnesium compared with aluminium is due to:
    A. filled orbitals in magnesium
    B. high nuclear charge in magnesium
    c. low radius of magnesium atom
    D. low effective nuclear charge in magnesium
    11
    933 Q1. Discuss the main features of long form of the periodic table. What are the advantages of long
    form of periodic table?
    die boble.
    11
    934 The value of ( square_{e q}^{infty} ) for ( N H_{4} C l, ) NaOH and NaCl are respectively, 149.74,248.1 and ( 126.4 Omega^{-1} c m^{2} e q u i v^{-1} . ) The value of ( square_{e q}^{infty} )
    of ( N H_{4} O H ) is
    A . 371.44
    B. 271.44
    ( c cdot 71.44 )
    D. Cannot be predicted from given data
    11
    935 In modern periodic table, if two elements have the same number of
    valence electrons, then they belong to
    the same:
    A. group
    B. period
    c. part
    D. none of the above
    11
    936
    1.312
    IU J MUI.
    Q16. Among the second period elements, the actual ionization enthalpies are in the order:
    Li<B< Be <C<O<N<F< Ne
    Explain why
    (i) Be has higher 4, H, than B?
    (ii) O has lower 4 H, than N and F?
    rbital while in
    11
    937 Question 36. Arrange the following in the order of property indicated for
    each set :
    (1) F2, Cl2, Br, 1-increasing bond dissociation enthalpy.
    (ii) HF, HCI, HBr, HEIncreasing acid strength.
    (ii) NH3, PH3, AsHz, SbH3, BiHz-increasing base strength.
    (1) F has small size; except it bond dissociation enthalpy decreases from
    Cl to l.
    (ii) From F to I, acid strength increases as H X bond distance increases.
    (iii) From N to Bi, basic strength decreases due to decrease in electron
    density.
    11
    938 Which of the following sequence contains atomic number of only
    representative elements?
    A. 55,12,48,53
    в. 13,33,54,80
    c. 3,33,53,87
    D. 22,33,55,66
    11
    939 Three elements ( X, Y ) and ( Z ) form a Dobereiner triad. The ratio of the atomic
    weight of ( X ) to that of ( Z ) is 7: 25
    If the sum of the atomic weights of ( x ) and ( Z ) is 160 , find the atomic weights of ( X, Y ) and ( Z )
    A ( . x rightarrow 35, Y rightarrow 80, Z rightarrow 125 )
    в. ( x rightarrow 125, Y rightarrow 80, z rightarrow 35 )
    c. ( x rightarrow 80, Y rightarrow 35, Z rightarrow 125 )
    D. ( x rightarrow 80, Y rightarrow 125, z rightarrow 35 )
    11
    940 What is the IUPAC symbol for Mendelevium?
    A. Md
    в. мп
    c. ме
    D. Mv
    11
    941 An atom has the symbol ( p ) ( q ) Which value determines the position of the element in the periodic table?
    A .
    B. 9
    ( c cdot p-q )
    D. p+q
    11
    942 Which of the following triads does not follow Dobereiner’s law of triads?
    A. ( mathrm{Li}, mathrm{Na}, mathrm{K} )
    B. Ca, Sr, Ba
    c. вe, мg, са
    D. Cu, Ag, Au
    11
    943 The atomic weights of Be were
    corrected by Mendeleev using the
    formula:
    ( mathbf{A} cdot sqrt{v}=a(z-b) )
    B. ( m v r=frac{n h}{2 pi} )
    C. atomic weight = equivalent weight ( times ) valency
    D. equivalent weight = atomic weight ( times ) valency
    11
    944 Noble gases belongs to group of periodic table.
    A. VII A
    B. VIII A
    c. VIII B
    D. VIA
    11
    945 What is meant by periodicity in properties of elements with reference to the periodic table? 11
    946 Which among the following element has largest atomic size?
    A.
    B.
    c. As
    D. sb
    11
    947 An element ( Z ) has atomic number 16 .
    Answer the following questions on ( Z ) :
    What kind of a compound is this?
    11
    948 Which of these choices is not a family of elements?
    A. Halogen
    B. Metal
    c. Inert Gas
    D. Fire extinguishers
    11
    949 All the elements in a group in the periodic table have similar:
    A. atomic weights
    B. number of valence electrons
    c. mass number
    D. atomic number
    11
    950 The number of periods present in the long form of the periodic table are:
    ( mathbf{A} cdot mathbf{6} )
    B. 7
    c. 8
    D. 18
    11
    951 0.39 Although fluorine is more electronegative than oxygen,
    of oxygen to stabilise higher oxidation states exceeds that
    Why?
    multiple bond with
    11
    952 Gradual addition of electronic shell in
    the noble gases causes a decrease in their?
    A. Ionization energy
    B. Atomic radius
    c. Boiling point
    D. Density
    11
    953 The correct order of atomic size of Na,
    Be and Mg is:
    ( A cdot B e>M g>N a )
    в. ( mathrm{Na}>mathrm{Mg}>mathrm{Be} )
    c. ( mathrm{Mg}>mathrm{Na}>mathrm{Be} )
    D. ( N a=M g>B e )
    11
    954 Q5. In terms of period and group where will you locate the element with z = 114?
    Ans Period 7 and
    1
    11
    955 The vertical columns in Mendeleev’s
    table were called:
    A. verticals
    B. periods
    c. columns
    D. groups
    11
    956 According to Mendeleev’s periodic table, one element whose atomic mass is
    greater than that of nickel is placed
    before Nickel. Name the element:
    A. copper
    B. Iron
    c. zinc
    D. cobal
    11
    957 The Inner Transition elements are
    classified as
    A. Lanthanides and Actinides
    B. Metals and Non-metals
    c. Both A and B
    D. None of these
    11
    958 LUDIL. TI U JUICK LU IU Wu Classily elenlerlis LO BOUP E
    Q3. What is the basic difference in approach between Mendeleev’s Periodic Law and the Modern
    Periodic Law?
    TILHA
    ondolo’s Periodic Law and Modern
    11
    959 For ( B e, Z_{e f f}=1.95 ) and for ( boldsymbol{B} boldsymbol{e}^{boldsymbol{x}+}, boldsymbol{Z}_{boldsymbol{e f f}}=mathbf{2 . 3 0 .} ) Hence, ion is:
    ( mathbf{A} cdot B e^{+} )
    в. ( B e^{2} )
    ( mathbf{c} cdot B e^{3+} )
    D. ( B e )
    11
    960 Give the names and atomic numbers of
    the first and last members of the
    lanthanide series.
    11
    961 In terms of period and group where would you locate the element with ( z= )
    ( 114 ? )
    11
    962 Which of the following give the correct increasing order of the atomic radii of
    ( boldsymbol{O}, boldsymbol{F}, boldsymbol{a} boldsymbol{n} boldsymbol{N} ? )
    A. ( O, F, N )
    в. ( N, F, O )
    c. ( O, N, F )
    D. ( F, O, N )
    11
    963 Identify the elements in the Periodic Table:
    A: Which shows diagonal relationship to ( B e )
    B: Which shows diagonal relationship to
    ( L i )
    A. ( A: A l, B: M g )
    в. ( A: S i, B: M g )
    c. ( A: M g, B: A l )
    D. ( A: A l, B: S i )
    11
    964 Q24. Describe the theory associated with the radius of an atom as it:
    (a) gains an electron (b) loses an electron?
    11
    965 The ionization potential ( left(I_{1}right) ) of nitrogen ( (Z=7) ) is more than oxygen ( (Z=8) )
    This is explained by :
    A. Hunds rule
    B. Excitation rule
    c. Pauli principle
    D. Aufbau principle
    11
    966 In which period of the periodic table,will an element, be found whose
    differentiating electron is a ( 4 mathrm{d} ) electron?
    11
    967 Is Fe, Co, Ni are Dobereiner triad? 11
    968 Which of the following elements does not belong to p-block?
    A . sr
    B. Po
    c. As
    D. Ga
    11
    969 Following question is based on ( S c(Z= )
    21).
    For any ( 1 s ) electron, ( Z^{*} ) (effective
    nuclear charge) is :
    A . 21.0
    B. 20.65
    c. 16.85
    D. 9.75
    11
    970 An element which is an essential
    constituent of all organic compounds
    belongs to :
    A. group 1
    B. group 14
    c. group 15
    D. group 16
    11
    971 Assertion
    The first ionization energy of Be is
    greater than that B.
    Reason
    2p orbital is lower in energy than 2 s.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    972 Na, Mg and Al are the elements having one, two and three valence electrons
    respectively. Which of these elements
    (i) has the largest atomic radius, (ii) is least reactive? Justify your answer
    stating reason for each.
    11
    973 The ( I P_{1} ) value of potassium is less than
    the ( I P_{1} ) value of sodium. This is due to:
    A. large size of potassium atom
    B. small size of potassium atom
    c. low density of potassium
    D. univalent nature of potassium
    11
    974 An element ( A ) combines with oxygen to
    form an oxide ( A O . ) Find the group to
    which the element ( boldsymbol{A} ) belongs.
    A . ( I A )
    в. ( I I A )
    c . III ( A )
    D. IVA
    11
    975 Select the correct statement(s) among
    the following.
    a. Electron gain enthapy of ( A s ) is more
    negative than ( C l )
    b. (+3) oxidation state are shown by ( boldsymbol{S} boldsymbol{b} )
    and ( B i ) both
    c. ( boldsymbol{P} ) is more electronegative than ( boldsymbol{N} )
    ( A cdot a, b ) and ( c )
    B. b only
    c. a and bonly
    D. b and conly
    11
    976 What s the basis of triad formation of
    elements?
    11
    977 The first element of actinide series is :
    A. thorium
    B. cerium
    c. lanthanum
    D. actinium
    11
    978 With respect to oxygen maximum oxidation state is shown
    by
    A. Halogen family
    B. Oxygen family
    c. Nitrogen family
    D. Boron family
    11
    979 The last element in period 2 is lithium
    A. True
    B. False
    11
    980 8. The energy needed to remove a single electron (most loosely bound) from an isolated
    gaseous atom is called
    (a) ionisation energy
    (b) electronegativity
    (C) kinetic energy
    (d) electron affinity
    11
    981 John Newland arranged the element starting with hydrogen and ending at
    A. cerium
    B. calcium
    c. thorium
    D. rubidium
    11
    982 Differentiating electron in inner transition elements enters the
    orbital.(s/p/d/f)
    11
    983 The elements of one period are given below in order from left to right
    ( boldsymbol{L} boldsymbol{i}, boldsymbol{B} boldsymbol{e}, boldsymbol{B}, boldsymbol{C}, boldsymbol{O}, boldsymbol{F}, boldsymbol{N} boldsymbol{e} )
    Which is the missing element?
    A . Na a
    B.
    c. ( c 1 )
    ( D )
    11
    984 Predict the position of the elements
    which form the largest cation and the
    smallest anion in the modern periodic
    table.
    11
    985 Example of Dobereiner’s triad is
    A. ( L i, ) Al ( , C a )
    в. ( L i, N a, K )
    c. ( L i, K, N a )
    D. ( K, A l, C a )
    11
    986 An element with electronic
    arrangement as 2,8,18,1 will exhibit which of the following stable oxidation states?
    A. +2 and +4
    B. +1 and +2
    ( mathbf{c} cdot+2 operatorname{to}+7 )
    D. +1 only
    11
    987 Which of the following pairs has both elements from the same group?
    A. ( M g, R a )
    в. ( M n, C l )
    c. ( M g, C u )
    D. ( M g, C l )
    11
    988 Which amongst the following is not an alkaline earth metal?
    ( A cdot ) Mg
    B. Ba
    ( c . F r )
    D. sr
    11
    989 If the same element is forming oxides in different oxidation states, then, which
    of the following statement is incorrect? This question has multiple correct options
    A. Oxide will be neutral in nature in which element is in its highest oxidation state
    B. Oxide will be highly acidic in nature in which element is in its highest oxidation state
    c. oxide will be amphoteric in nature in which element is in its highest oxidation state
    D. oxide will be highly basic in nature in which element is in its highest oxidation state
    11
    990 What is the name for the horizontal
    rows of the periodic table?
    A. Groups
    B. Periods
    c. Families
    D. sets
    11
    991 Which element is considered
    radioactive among the options given below?
    A. Sodium
    B. Gold
    c. Thorium
    D. Neon
    11
    992 An element in period-3 which has zero electron affinity is:
    A. neon
    B. sulphur
    c. sodium
    D. argon
    11
    993 The number of metals from the
    following:
    ( boldsymbol{A} boldsymbol{s}, boldsymbol{F} boldsymbol{e}, boldsymbol{X} boldsymbol{e}, boldsymbol{L} boldsymbol{i}, boldsymbol{B}, boldsymbol{C l}, boldsymbol{B} boldsymbol{a}, boldsymbol{P}, boldsymbol{I}, boldsymbol{S} boldsymbol{i} )
    11
    994 The electronegativites of the following
    elements ( H, O, F, S ) and ( C l ) increase in
    the order:
    A. ( H<O<F<S<C l )
    в. ( S<H<C l<O<F )
    c. ( H<S<O<C l<F )
    D. ( H<S<C l<O<F )
    11
    995 An element A has atomic number 7. It
    will have properties similar to the element with the atomic number:
    A. 85
    B. 57
    ( c cdot 26 )
    D. 51
    11
    996 Mendeleev’s Periodic Table was
    published in a in 1872.
    A. German journal
    B. US journal
    c. Russian journal
    D. None of the above
    11
    997 Considering their electrons affinities, it is possible for alkali metals to form an
    anion like ( mathrm{M}^{-} ) where M represents an
    alkali metal. If true enter 1 , else enter 0 .
    11
    998 PU
    6. In halogens, which of the following increases from iodine to fluorine?
    (a) Bond length
    (b) Electronegativity
    (@) The ionization energy of the element
    (d) Oxidizing power
    nilalatiansbih
    11
    999 Which of the following statements are true about the modern form of the
    periodic table?
    A. Properties of the elements are the periodic functions of their atomic number
    B. There are 7 periods
    c. There are 18 numbered groups
    D. All of the above
    11
    1000 Why is there a gradual increase in the
    ionisation energy from ( L i ) to ( N e ? )
    A. Increase in atomic size
    B. Decrease in nuclear charge
    c. Atomic size remains same
    D. Increase in nuclear charge
    11
    1001 Match list I (atomic number of the
    elements) with list II (position in the periodic table) and select the correct
    answer using the codes given below the
    lists.
    begin{tabular}{c|cc|c}
    & List I & & List II \
    A. & 52 & 1. & s-block \
    B & 56 & 2. & p-block \
    c. & 57 & 3. & d-block \
    D. & 60 & 4. & f-block
    end{tabular}
    A. ( A-2, B-1, C-3, D-4 )
    B. ( A-2, B-1, C-4, D-3 )
    ( c )
    ( A-1, B-2, C-3, D-4 )
    D. ( A-1, B-2, C-4, D-3 )
    11
    1002 The number of electrons in the valence
    shell of group 1 elements.
    ( mathbf{A} cdot mathbf{1} )
    B. 2
    ( c cdot 3 )
    ( D )
    11
    1003 Which of the following is a defect in the Mendleev’s periodic table?
    A. Prediction of new elements
    B. Doubtful atomic weights
    c. Anomalous position of hydrogen
    D. Non-systematic study of elements
    11
    1004 Which element has the highest first ionization potential?
    A .
    B. Ne
    c. не
    D.
    E. ( L )
    11
    1005 Which of the following sets of elements follows Newland’s octave rule?
    A. ( B e, M g, C a )
    в. ( N a, K, R b )
    c. ( F, C l, B r )
    D. ( B, A l, G a )
    11
    1006 Arrange the following as per the
    instructions given in the brackets:
    ( N a, K, C l, S, S i ) (increasing order of ionization energy)
    11
    1007 A, ( B, C ) are three elements with atomic
    numbers, Z-1, Z and Z+1 respectively. B is an inert gas. Identify the elements having same valence shell.
    ( A cdot A, B )
    B. В, с
    c. ( A, C )
    D. A, B, C
    11
    1008 From among the elements, choose the
    following:
    ( mathrm{Cl}, mathrm{Br}, mathrm{F}, mathrm{O}, mathrm{Al}, mathrm{C}, mathrm{Li}, mathrm{Cs} ) and ( mathrm{Xe} )
    The element which belongs to zero
    group.
    11
    1009 Metal which emits photo-electrons very easily is :
    ( A cdot A )
    B.
    ( c cdot c s )
    D. cu
    11
    1010 All the elements of the same group have similar ( _{text {一一一一一一一一 }} ) properties. 11
    1011 Correct the mistakes, if any in the
    following statement.
    ¡) Second period is a short period. It contains only two elements.
    ii) Group 18 elements are called Halogen family.
    11
    1012 In which group all the elements do not have same number of valence
    electrons?
    A. zero
    B. first
    c. second
    D. seventh
    11
    1013 An element ( X ) combines with oxygen to
    form an oxide ( X_{2} O . ) This oxide is
    electrically conducting.
    (i) How many electrons would be there in the outermost shell of the element ( boldsymbol{X} )
    (ii) To which group of the periodic table does the element ( X ) belong.
    (iii) Write the formula of the compound
    which is formed when ( X ) reacts with
    chlorine.
    11
    1014 Which of the following are the demerits
    of Mendeleev periodic table?
    This question has multiple correct options
    A. No proper position for hydrogen is given.
    B. Grouping of chemically dissimilar elements.
    C. Position given to isotopes.
    D. Presence of anomalous pairs.
    11
    1015 Total no. of compound which are not
    possible? ( boldsymbol{P} boldsymbol{C} boldsymbol{I}_{5}, boldsymbol{N} boldsymbol{C} boldsymbol{I}_{5}, boldsymbol{O} boldsymbol{F}_{4}, boldsymbol{O} boldsymbol{F}_{2}, boldsymbol{S} boldsymbol{F}_{4} )
    ( boldsymbol{S} boldsymbol{F}_{6}, boldsymbol{P H}_{5}, boldsymbol{X} boldsymbol{e} boldsymbol{H}_{4}, boldsymbol{X} boldsymbol{e} boldsymbol{F}_{4}, boldsymbol{I} boldsymbol{F}_{7}, boldsymbol{I} boldsymbol{H}_{5} )
    ( boldsymbol{P B r}_{6}^{-}, boldsymbol{C l F}_{3} )
    11
    1016 Identify the correct order of solubility in aqueous medium:
    A ( cdot C u S>Z n S>N a_{2} S )
    в. ( Z n S>N a_{2} S>C u S )
    c. ( N a_{2} S>C u S>Z n S )
    D. ( N a_{2} S>Z n S>C u S )
    11
    1017 You will find metals on the extreme
    right side of the periodic table.
    A. True
    B. False
    11
    1018 The property which regularly increases down the group in the periodic table is:
    A. ionisation energy
    B. electronegativity
    c. reducing nature
    D. electron affinity
    11
    1019 Which group in p-block elements shows highest positive oxidation state?
    A . 16
    B. 17
    c. 18
    D. 15
    11
    1020 The law of octaves was proposed by :
    A. Newlands
    B. Dobereiner
    c. Lavoisier
    D. Mendeleev
    11
    1021 0.15 Those elements impart colour to th
    elements impart colour to the flame on heating in it, the atoms of
    which require low energy for the ionisation (i.e., absorb energy in the
    visible region of spectrum). The elements of which of the following
    groups will impart colour to the flame ?
    (a) 2
    (b) 13
    (c) 1
    (d) 17
    11
    1022 In Mendeleev’s periodic table, the gap
    was not left for one of the following elements. This element is:
    A. potassium
    B. beryllium
    c. germanium
    D. scandium
    11
    1023 Q. 35 How would you explain the fact that the first ionisation enthalpy of
    sodium is lower than that of magnesium but its second ionisation
    enthalpy is higher than that of magnesium?
    11
    1024 Which of the following is not a periodic property for the elements?
    A. Electronegativity
    B. Atomic size
    c. occurrence in nature
    D. lonization energy
    11
    1025 The tendency of a bonded atom in a molecule to lose or repel the electron density of a shared pair of electrons is
    called:
    A. electro negativity
    B. electropositivity
    c. electroneutrality
    D. none of these
    11
    1026 Nitrogen ( (z=7) ) is the element of group V of the periodic table. Which of the following is the atomic number of the next element in the group?
    ( A cdot 9 )
    B. 14
    c. 15
    D. 17
    11
    1027 The atomic number of an element that
    belongs to the IVA (or 14) group and 4th period is:
    A . 32
    B. 30
    ( c cdot 34 )
    D. 36
    11
    1028 Find the number of an element(s) which
    is/are present in group-II. ( boldsymbol{B} boldsymbol{a}, boldsymbol{K}, boldsymbol{C} boldsymbol{a}, boldsymbol{C} boldsymbol{s}, boldsymbol{R} boldsymbol{b}, boldsymbol{n} )
    11
    1029 The number of ionization energies
    carbon can have are:
    A . 1
    B. 2
    ( c cdot 4 )
    ( D )
    11
    1030 lonic mobility of ( mathrm{Li}^{+} ) is greater than that
    of ( mathrm{Na}^{+} )
    A. True
    B. False
    11
    1031 ( ^{35} C l ) and ( ^{37} C l ) are the two isotopes of
    chlorine, in the ratio 3: 1 respectively. If
    the isotope ratio is reversed the average atomic mass of chlorine will be:
    ( mathbf{A} cdot 35.0 u )
    B. ( 35.5 u )
    c. ( 36.0 u )
    D. 36.5 ( u )
    11
    1032 021. Would you expect the second electron gain enthalpy of O as positive, more negative or less
    negative than the first? Justify your answer.
    11
    1033 Give a reason for the following. lonisation potential increases across a period, from left to right. 11
    1034 The dominant factor in determining the IE of the elements on moving down the groups is its:
    A. atomic radius
    B. effective nuclear charge
    c. Both (a) and (b)
    D. None of the above
    11
    1035 An element belongs to the 3 rd period and Group II of the periodic table.
    Name of the element is
    A. magnesium
    B. sodium
    c. aluminium
    D. calcium
    11
    1036 lonization Energy ( (boldsymbol{k} boldsymbol{J} / boldsymbol{m} boldsymbol{o l}) )
    First
    [
    896
    ]
    Secon
    [
    1,752
    ]
    Third
    [
    14,807
    ]
    Fourth
    [
    17,948
    ]
    The table above shows the first four
    ionization energies of an element. This element is located in which group of the
    periodic table?
    A. Group 1
    B. Group 2
    C . Group 3
    D. Group 4
    11
    1037 The only non-metal which is liquid at
    ordinary temperature is ( B r_{2} )
    A. True
    B. False
    11
    1038 Number of elements in Lanthanide
    family is:
    11
    1039 Out of the following outer electronic configurations of atoms, the highest oxidation state is achieved by which one?
    A ( cdot(n-1) d^{8} n s^{2} )
    B . ( (n-1) d^{5} n s^{2} )
    c. ( (n-1) d^{3} n s^{2} )
    D・ ( (n-1) d^{5} n s^{1} )
    11
    1040 Which statement describes positive
    ions?
    A. Positive ions have more electrons than neutrons
    B. Positive ions have more protons than neutrons
    C. Positive ions have more electrons than protons
    D. Positive ions have more protons than electrons
    11
    1041 Which of the following pair represents elements of same group?
    A . Q, R
    B. P,Q
    ( c cdot P, s )
    D. Q,
    11
    1042 Q1. Give the name and atomic number of the inert gas atom in which the total number of
    d-electrons is equal to the difference between the numbers of total p and total s-electrons.
    10
    11
    1043 Q1. Arrange the following as stated: (i) N,, ,, F, C1, (Increasing order of bond dissociation
    energy) (ii) F, CI, Br, I (Increasing order of electron gain enthalpy) (iii) ,,N,,C,, , (Increasing
    order of bond length).
    11
    1044 38 Explain the deviation in ionisation enthalpy of some elements from the
    general trend by using given figure.
    2500+
    2000+
    (2080) Ne,
    lonisation enthalpy
    A H/kJ mol
    (1681) FA
    1500
    (1402) N
    (1314)
    1000+
    (899) Bex (1086)
    B (801)
    5007 (520) Li/
    0 1 2 3 4 5 6 7 8 9
    Atomic number of elements –
    10
    11
    1045 The total number of elements in the
    group ( I B ) is:
    A . 4
    B. 5
    ( c .7 )
    D. 9
    11
    1046 An element R belongs to IVA(14) group and 3rd period in the periodic table. Arrange the elements that are placed below ‘R’ in increasing order of atomic size.
    A. ( G e>S n>P b )
    B. ( A s>S b>B i )
    c. ( G e<S n<P b )
    D. ( A s<S b<B i )
    11
    1047 Which of the following are transition
    elements?
    ( mathrm{K}, mathrm{Mn}, mathrm{Ca}, mathrm{Cs}, mathrm{Fe}, mathrm{Cu}, mathrm{Pb} )
    11
    1048 Who proposed the law of traids? 11
    1049 Write the electronic configuration of
    Sr ( ^{2+} ) in absence of Aufbau Principle.
    ( mathbf{A} cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{10}, 4 s^{2} 4 p^{5} 4 d^{1} )
    B. ( 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{10}, 4 s^{2} 4 p^{3} 4 d^{3} )
    C ( cdot 1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{10}, 4 s^{2} 4 p^{6} )
    D. None of these
    11
    1050 The three elements ( A, B ) and ( C ) with
    similar properties have atomic masses
    ( x, Y ) and ( z ) respectively. The mass of ( Y ) is approximately equal to the average mass of ( X ) and ( Z . ) Such an
    arrangement of elements called as:
    A. Dobereiner triad
    B. Mendeleev triad
    c. Modern triad
    D. none of the above
    11
    1051 Which of the following is a highly polar bond?
    A ( . O-H )
    в. ( N-H )
    c. ( H-C l )
    D. ( H-F )
    11
    1052 How many electrons does oxygen have in its outermost shell? 11
    1053 Write the general outer electronic configuration of ( s, p, d ) and ( f ) block elements. 11
    1054 Which of the following sulphates has the highest solubility in water?
    A ( . . M g S O_{4} )
    в. ( B a S O_{4} )
    ( mathrm{c} cdot mathrm{CaSO}_{4} )
    D. ( B e S O_{4} )
    11
    1055 Which of the following elements has lowest electronegativity?
    A. ( N a )
    в. ( M g )
    c. ( A l )
    D. ( S ) i
    11
    1056 Which of the following sets belongs to
    the same period:
    A. ( L i, N a, K )
    в. ( L i, M g, C a )
    c. ( N i, C u, Z n )
    D. ( F, C l, B r )
    11
    1057 Identify the correct match(es) in the
    following table:
    ( begin{array}{ll}text { Element } & text { Column A } \ text { Sodium } & text { Non-metal } \ text { Sulphur } & text { Lanthanide } \ text { Manganese } & text { Metal } \ text { Cerium } & text { Transition metal }end{array} )
    A. Sodium- Metal
    B. Sulphur- Non metal
    c. Manganese- Transition metal
    D. all of these
    11
    1058 Q. 14 Which of the following elements can show covalencey greater
    (a) Be
    (b) P
    (d) B
    W covalencey greater than 4?
    (c) S
    11
    1059 Which of the following statements is
    not correct for the periodic
    classification of elements?
    A. The properties of elements are the periodic functions of their atomic numbers.
    B. Non – metallic elements are lesser in number than
    metalic elements
    C. The first ionization energies of elements along a period do not vary in regular manner with increase in atomic number
    D. For transition elements, the d-sub shells are filled with electrons monotonically with increase in atomic number.
    11
    1060 Write the electronic configuration of Elements with an electron sextet, e.g.
    ( boldsymbol{O}, boldsymbol{S}, boldsymbol{e t c} )
    11
    1061 Statement 1: For an element with an
    atomic number of ( 17, ) the most probable
    oxidation number is +1
    Statement 2: The outer energy level of the halogen family has a tendency to add one electron to itself
    A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1
    B. Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.
    c. statement 1 is correct but Statement 2 is not correct
    D. Statement 1 is not correct but Statement 2 is correct
    E. Both the Statement 1 and Statement 2 are not correct.
    11
    1062 Which of the following has the highest electronegativity?
    A . Na a
    B. cl
    ( c cdot k )
    ( D )
    11
    1063 The single-bonded metallic radius of Na is 157 pm. What is the reasonable estimate of the radius of Na assuming that the increment between radii of
    different magnitudes is 60 pm?
    ( A cdot 97 mathrm{pm} )
    B. 95 pm
    ( c cdot 93 p m )
    D. 99 pm
    11
    1064 True or False
    VI A group elements are known as
    chalcogens.
    11
    1065 The correct statement among the following is:

    This question has multiple correct options
    A. the first ionization potential of ( A ) l is less than the first ionization potential of Mg
    B. the second ionization potential of Mg is greater than the second ionization potential of ( mathrm{Na} )
    C. the first ionization potential of Na is less than the first ionization potential of Mg
    D. the third ionization potential of Mg is greater than the third ionization potential of Al

    11
    1066 Why was the basis of classification of
    elements changed from the atomic
    mass to the atomic number?
    11
    1067 On moving down the group, the
    tendency to gain electrons:
    A. decreases
    B. increases
    C. increases and then decreases
    D. decreases and then increases
    11
    1068 The element with highest electronegativity value is :
    A. carbon
    B. Chlorine
    c. Fluorine
    D. oxygen
    11
    1069 The increasing order of reactivity among group 1 element is ( L i<N a< )
    ( R bC I>B r>I . ) Explain?
    11
    1070 Which of the following statements are
    correct about Mendeleev’s periodic table?
    i) It is based on increasing order of
    atomic numbers.
    ii) Mendeleev corrected the atomic
    weight of some elements like Be, In etc.
    iii) ( left(boldsymbol{A} boldsymbol{r}, boldsymbol{H}_{2}right),left(boldsymbol{C o}, boldsymbol{C l}_{2}right),left(boldsymbol{T} boldsymbol{e}, boldsymbol{F}_{2}right) ) are
    three inverted pairs.
    iv) It is based on increasing order of atomic weights.
    A. only (i) correct
    B. (ii) and (iv) are correct
    c. only (iii) correct
    D. (i) and (iv) are correct
    11
    1071 The elements ( A ) and ( B ) obey
    Newland’s law of octave. How many
    elements are there between ( A ) and ( B ? )
    A. 7
    B. 8
    ( c .5 )
    D. 6
    11
    1072 According to Dobereiner in Triads, atomic weight of the centre element is equal to 1st and 3rd
    elements in that triads.
    A. Geometric Mean
    B. Arithmetic Mean
    c. Harmonic Mean
    D. None of these
    11
    1073 Which of the following indicates the correct order of variation in atomic
    size?
    A. ( B e>C>F>N e )
    в. ( B e>C>F<N e )
    c. ( B e<C<F<N e )
    D. ( F<N e<B e<C )
    ( C )
    11
    1074 The most stable oxidation state of
    Thallium is:
    ( A cdot+1 )
    B. +3
    ( c cdot+4 )
    D. +6
    11
    1075 Which of the following has zero electronegativity?
    A . ( A r )
    B. ( S ) i
    c. ( N )
    D. ( F )
    11
    1076 Q11. Define electron gain enthalpy. What are its units? 11
    1077 The atomic number of the element next
    to bromine (atomic no 35 ) in the same
    group is:
    A . 43
    B. 50
    ( c .56 )
    D. 53
    11
    1078 The first attempt to classify elements systemically was made by :
    A. Mendeleev
    B. Newland
    c. Lother Meyer
    D. Dobereiner
    11
    1079 (a) What are isotopes?
    (b) State modern periodic law.
    (c) Name two noble gas.
    11
    1080 Q Type your question
    Why may be members of the same family, it does mean that they will behave in similar ways.

    The same things can be said about elements in a group (“family”) on the periodic table. For example, fluorine and iodine are members of the halogen family, but their physical properties are different, as shown in the table below.
    Melting Point ( quad ) Boiling Point Element ( quadleft(^{circ} Cright) )
    ( left(^{circ} Cright) )
    Fluorine
    [
    220
    ]
    ( begin{array}{ll}text { lodine } & +118 \ & +184end{array} )
    What of the following is the BEST explanation for these differences in melting and boiling point?
    This question has multiple correct options
    A. Fluorine has a higher value for electronegativity than iodine
    B. The covalent bond in the fluorine molecule is stronger than the covalent bond in the iodine molecule
    C. lodine molecules are larger and more polarizable than fluorine molecules
    D. Fluorine is a nonpolar molecule, but iodine is a polar molecule

    11
    1081 An element ( X ) belongs to group III-A and 4 th period in the periodic table. Find out
    the atomic numbers of ( X ) and the
    element which is placed just below ( boldsymbol{X} ) in the periodic table.
    11
    1082 Eka-aluminium forms chloride of the
    type :
    A ( cdot E_{2} C l )
    в. ( E C l_{3} )
    ( mathbf{c} cdot E_{2} C l_{3} )
    D. ( E_{3} C l_{4} )
    11
    1083 The correct order of the second
    ionisation potential of carbon, nitrogen, oxygen and fluorine is :
    A. ( C>N>O>F )
    в. ( O>N>F>C )
    с. ( O>F>N>C )
    11
    1084 Q5. Elements A, B, C and D have atomic numbers 12, 19, 29, and 36 respectively. On the basis of
    electronic configuration, write to which group of the periodic table each element belongs.
    11
    1085 Which of the following compound has no existence?
    A. ( mathrm{CF}_{4} )
    B. ( mathrm{XeF}_{4} )
    ( mathrm{c} cdot mathrm{KrF}_{4} )
    D. HeF ( _{4} )
    11
    1086 ( H_{2} O ) is a liquid but ( H_{2} S ) is a gas.
    Explain why?
    11
    1087 Which will be the third element among
    the given elements to complete given Doberiener triad?
    (Atomic mass of Be ( 9 ; ) Na ( 23 ; ) Mg ( 24 ; ) si 28; Cl 35; Ca 40)
    ( mathrm{Be},_{-}-_{-}, mathrm{Ca} )
    11
    1088 ldentify the noble gas in the ( 4^{t h} ) period. 11
    1089 . 4 The first ionisation enthalpies of Na, Mg, Al and Si are in the order
    (a) Na Al Mg > Al > Si
    (c) Na < Mg < Al Mg > Al < Si
    Ans.(a) Follow the following stens to sobre ou unh nrohlo
    11
    1090 consist of atoms that have valence electrons in a ( boldsymbol{d}- )
    subshell.
    A. Alkali metals
    B. Alkaline earth metals
    c. Transition metals
    D. Halogens
    11
    1091 The atomic number of elements ( A, B ) and ( C ) are ( (Z-1), Z ) and ( (Z+1) ) respectively. B is an inert gas (not helium). Which element among ( A, B ) and
    C has the highest ionization energy? Why?
    11
    1092 Which of the following sequence is correct for decreasing order of ionic
    radius?
    A ( cdot S e^{-2}, I^{-}, B r^{-}, O^{-2}, F^{-} )
    B . ( I^{-}, S e^{-2}, O^{-2}, B r^{-}, F^{-} )
    c. ( S e^{-2}, I^{-}, B r^{-}, F^{-}, O^{-2} )
    D. ( I^{-}, S e^{-2}, B r^{-}, O^{-2}, F^{-} )
    11
    1093 Which of the following will have the most negative electron gain enthalphy and which the least negative?
    ( A cdot F, C )
    в. С।,
    c. ( mathrm{Cl} ),
    D. CL,
    11
    1094 The chemistry of lithium is very similar to that of magnesium even though they are placed in different groups. Its reason is that:
    A. both are found together in nature
    B. both have nearly the same size
    c. both have similar electronic configurations
    D. the ratio of their charge to size is nearly the same
    11
    1095 Arrange following oxides in increasing
    acidic nature.
    ( boldsymbol{L} boldsymbol{i}_{2} boldsymbol{O}, boldsymbol{B} boldsymbol{e} boldsymbol{O}, boldsymbol{B}_{2} boldsymbol{O}_{3} )
    A. ( L i_{2} O<B e O<B_{2} O_{3} )
    в. ( B e O<L i_{2} O<B_{2} O_{3} )
    c. ( L i_{2} O<B_{2} O_{3}<B e O )
    D. None of these
    11
    1096 Actinides belong to which period?
    A .4
    B. 5
    ( c .6 )
    D.
    11
    1097 The element having electronic configuration ( [boldsymbol{K} boldsymbol{r}] boldsymbol{4} boldsymbol{d}^{10} boldsymbol{4} boldsymbol{f}^{14} boldsymbol{5} boldsymbol{s}^{2} boldsymbol{5} boldsymbol{p}^{6} boldsymbol{5} boldsymbol{d}^{1} boldsymbol{6} boldsymbol{s}^{2} ) belongs to
    A. s-block
    B. p-block
    c. d-block
    D. f-block
    11
    1098 In long form of periodic table, the total number of periods is:
    A. 5
    B. 7
    ( c cdot 8 )
    D.
    11
    1099 The shielding constant ‘ ( sigma^{prime} ) for ( _{7} N ) atom
    is :
    A . 3.10
    B. 3.40
    c. 3.80
    D. 4.20
    11
    1100 Assertion
    ( F ) -atom has less electron affinity than
    ( C l^{-} ) atom.
    Reason
    Additional electrons are repelled more
    effectively by ( 3 p ) electrons in ( C l ) atom than by ( 2 p ) electrons in ( F ) -atom.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    1101 Of the following, the wrong statement is:
    A. the first ionization potential of ( A ) l is less than the first ionization potential of Mg.
    B. the second ionization potential of Mg is greater than the second ionization potential of ( mathrm{Na} )
    C. the first ionization potential of Na is less than the first ionization potential of Mg.
    D. the third ionization potential of Mg is greater than the third ionization potential of Mg.
    11
    1102 Less amount of energy is required to
    remove ‘s’ electron than ‘p’ electron.
    A. True
    B. False
    11
    1103 begin{tabular}{ll|l}
    & ( mathbf{X} ) & ( mathbf{Y} ) \
    & & \
    Normal & 2,8,7 & \
    Electronic & & 2,8,2 \
    Configuration & Dissolves in & Very low \
    Nature of & water and & solubility in \
    oxide & turns blue & water. \
    & litmus red & Dissolves in \
    & & hydrochloric \
    Tendency for & acid \
    oxidising & Tends to & Tends to act \
    and reducing & oxidise & as a \
    reactions & elements & reducing \
    Electrical and & and & agent \
    thermal & compounds & Good \
    conductivity & Very poor & Electrical \
    & electrical & conductor \
    & conductor & Good \
    & Poor thermal & Thermal \
    & conductivity & conductor \
    Tendency to & & \
    form & No tendency & \
    alloys and & to form & Forms alloys \
    amalgums & alloys &
    end{tabular} Using the information above, complete
    the following

    Non-metallic elements tend to be electricity

    11
    1104 The halogens (group 17 elements):
    A. have an electronic configuration of a noble gas
    B. are highly electropositive character
    C. show variable oxidation state of -1,+1,+3,+5 and +7 in
    their various compounds
    D. forms a volatile, covalent hydrides HX in which the halogen (X) shows an oxidation state of +1
    11
    1105 Which of the following sets of atomic masses do not correspond to Dobernier traid?
    This question has multiple correct options
    A .7,23,39
    в. 20,38,56
    c. 47,91,178
    D. 54,95,183
    11
    1106 Which is the correct in the following?
    A ( . ) Radius of ( C l ) is ( 0.99 AA ), while that of ( C l^{+} ) ion is 1.54 A.
    B. Radius of ( C l ) atoms is 0.99 , ( hat{A} ), while that of ( N a ) atom is 1.54 月.
    C. Radius of ( C l ) atoms is 0.99 , a , while that of ( C l^{-} ) ion is ( 0.81 A )
    D. Radius of ( N a ) atoms is 0.95 , ( dot{A} ), while that of ( N a^{+} ) ion is ( 1.54 AA )
    11
    1107 Nobel gases were included in Mendeleev’s periodic table in the:
    A. 1 st group
    B. 7th group
    c. 8 th group
    D. none of these
    11
    1108 The stability of cation in dihalides of
    Si, Ge, Sn and Pb increases in the
    sequence is:
    A ( cdot G e X_{2}<operatorname{Si} X_{2}<S n X_{2}<P b X_{2} )
    B. ( operatorname{SiX}_{2}<operatorname{GeX}_{2}<operatorname{Pb} X_{2}<operatorname{SnX}_{2} )
    c. ( operatorname{six}_{2}<operatorname{Ge} X_{2}<operatorname{Sn} X_{2}<operatorname{Pb} X_{2} )
    D. ( P b X_{2}<operatorname{Sn} X_{2}<G e X_{2}<operatorname{Si} X_{2} )
    11
    1109 Where would you locate the element
    with electronic configuration 2,8 in the modem period table?
    A. Group 8
    B. Group 2
    c. Group 10
    D. Group 18
    11
    1110 The electronic configuration of ( boldsymbol{H} e ) is 2
    and that of oxygen is
    11
    1111 Which of the following is the general electronic configuration in the valence
    shell of elements of a group ( -16 ? )
    A ( cdot n s^{2} n p^{3} )
    В. ( n s^{2} n p^{4} )
    c. ( n s^{2} n p^{6} )
    D. ( n s^{2} n p^{5} )
    11
    1112 If the second I.P of calcium is 275.12
    kcals ( m o l^{-1}, ) then, the equation that
    represents this ionization can
    be written as:
    A ( cdot C a_{(S)}^{+} rightarrow C a_{(S)}^{3+}+2 e^{-}-275.12 ) kcals
    B. ( C a_{(S)}^{+} rightarrow C a_{(S)}^{3+}+2 e^{-}+275.12 ) kcals
    c. ( C a_{(S)}^{+} rightarrow C a_{(S)}^{2++}+e^{-}+275.12 ) kcals
    D. ( C a_{(S)}^{+} rightarrow C a_{(S)}^{2+1}+e^{-}-275.12 ) kcals
    11
    1113 Assertion
    The first IE of ( B e ) is greater than that of
    ( boldsymbol{B} )
    Reason
    ( 2 p ) -orbital is lower in energy than ( 2 s )
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect but Reason is correct
    11
    1114 How does the electronic configuration of an atom relate to its position in the Modern Periodic Table? 11
    1115 Which of the following is true regarding
    periodicity of elements?
    A. Elements of same group are characterized by same valence shell electronic configuration.
    B. The most electropositive elements are positioned on right hand side of the Modern periodic Table
    C. On going from Li of F there would be decrease in ionization energy
    D. reducing property of elements increases from Na to Cl in 3 rd period elements.
    11
    1116 What were the two criteria used by Mendeleev in creating his Periodic Table? 11
    1117 The diagram represents an atom ‘X’. Answer the following.
    f atom ‘X’ has 1 electron in its outer
    shell, is it a non-metal.
    A. True
    B. False
    11
    1118 As you move from top to bottom on the periodic table, what generally happens to the atomic radius?
    A. It decreases
    B. It decreases, then increases
    c. It remains constant
    D. It increases, then decreases
    E. It increases
    11
    1119 A paste of substance ( A ) is used to
    decorate the ceiling of your home. State the name of the product in the
    above reaction.
    11
    1120 Symbol of palladium is:
    A. ( P )
    в. ( P o )
    c. ( P d )
    D. ( P h )
    11
    1121 In which one of the following pairs the radius of the second species is greater than that of the first?
    A. ( N a, M g )
    B. ( O^{2-}, N^{3-} )
    c. ( L i^{+}, B e^{2+} )
    D. ( B a^{2+}, S r^{2+} )
    11
    1122 Maximum work in periodic table related with atomic number was done by:
    A. Mendeleev
    B. Aston
    c. Mosley
    D. Newland
    11
    1123 Assertion
    First period of periodic table is the shortest period.
    Reason
    K shell can accommodate a maximum
    of two electrons
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    c. Assertion is correct but Reason is incorrect
    D. Assertion is incorrect, but reason is correct.
    11
    1124 lonization potential values of an element ( X ) are 104 kJ, 200 kJ, 420 kJ
    2825 kJ per mole. Identify the group to which the element belongs?
    A. ( I A )
    в. ( I I A )
    c. ( I I I A )
    D. ( I V A )
    11
    1125 Which of the following is the correct set
    of elements to Dobereiner’s triads?
    A. Li-7, Na – 23, K -39
    B. Br-80, CI-35.5,1-127
    c. Fe ( -55.85, ) Ni ( -58.71, ) Co -58.93
    D. All of these
    11
    1126 First long period contains elements.
    A . 8
    B. 18
    ( c .32 )
    ( D )
    11
    1127 Atomic number of an element ( X ) is 16
    its group number will be :
    A . 14
    B . 15
    c. 16
    D. 17
    11
    1128 Electronic configuration of Gd(64) is
    written as: ( [boldsymbol{X} boldsymbol{e}]_{54} boldsymbol{4} boldsymbol{f}^{x} boldsymbol{5} boldsymbol{d}^{1} boldsymbol{6} boldsymbol{s}^{2}, ) then
    the value of ( x ) is ( 7 . ) If true enter 1 , else
    enter 0
    11
    1129 Be, ( M g, C a, S r, B a ) are group 2 metals. Which of these will form ions
    most readily?
    A. ( B e )
    в. ( M g )
    ( c cdot S r )
    D. ( B a )
    11
    1130 Which of the following is not s-block element?
    В. ( 1 s^{2} 2 s^{2} 2 p^{1} )
    c. ( 1 s^{2} 2 s^{1} 2 p^{1} )
    D・ ( [A r] 4 s^{1} 4 p^{1} )
    11
    1131 elements (i.e., s and
    of representative
    NO
    0.33 First member of each group of representative elements
    p-block elements) shows anomalous behaviour. Illustrate w
    examples.
    nntntiin niomonts tie s- and p-block elements)
    11
    1132 Atomic numbers of few elements are
    given below. Which of the pairs belongs
    to s-block?
    A . 7,14
    B. 3,20
    c. 8,15
    D. 9,17
    11
    1133 The elements posses stable electronic
    configuration are called as
    A. Transition metals
    B. Non-transition metals
    c. Noble gases
    D. None of these
    11
    1134 Identify the correct sets of entries that
    are rightly matched.

    Column A
    ( B )
    (A) Bridge elements Elements of group IA-VIIA
    (B) Representative elements
    (b) 2nd-
    period elements
    (C) Typical elements
    (c) 7 th-
    period elements
    (D) Transition elements
    (d) ( 3 r d- )
    period elements
    (E) Transuranic elements
    (e) Present
    in 4 th, 5 th and 6 th periods
    ( mathbf{A} cdot A-b, B-a, C-d, D-e, E-c )
    B . ( A-c, B-a, C-b, D-d, E-e )
    c. ( A-a, B-c, C-d, D-e, E-b )
    D. ( A-c, B-e, C-d, D-b, E-a )

    11
    1135 The period of element with atomic number 20 in the periodic table is :
    ( mathbf{A} cdot mathbf{1} )
    B. 2
    ( c cdot 3 )
    ( D )
    11
    1136 The modern periodic table is most ( _{text {一一一一一一一一一 }} ) form of periodic
    table.
    A . insignificant
    B. Significant
    c. Both A and B
    D. None of these
    11
    1137 2. Which of the following oxides is neutral?
    (a) Sno
    (b) CO
    (c) A1,
    (d) Na,o
    11
    1138 Significance of classification of
    periodic table is to
    A. predict the blocks of elements
    B. predicts the groups of elements
    c. both A and B
    D. none of these
    11
    1139 Modern periodic table has
    periods.
    A. 7
    B. 8
    ( c cdot 6 )
    ( D )
    11
    1140 Electronic configuration ( boldsymbol{O} ) is:
    A ( cdot[H e] 2 s^{2} 2 p^{4} )
    B . ( [H e] 2 s^{3} 2 p^{4} )
    ( mathbf{c} cdot[H e] 2 s^{2} 2 p^{5} )
    D cdot ( [H e] 3 s^{2} 2 p^{4} )
    11
    1141 The chemical properties of the elements of matter have been found to repeat is regular patterns. This pattern can be
    seen in the arrangement of atoms in the:
    A. nutrition table
    B. calculus table
    c. periodic table
    D. chemical table
    11
    1142 Atomic number ( _{-1-}-_{-1} ) by one unit on moving from right to left.
    A. increases
    B. decreases
    c. remains the same
    D. None of the above
    11
    1143 An element ‘X’ with atomic number 114
    has recently been discovered. Its IUPAC name is:
    A. Eka-lead
    B. Ununfortium
    c. Ununquadium
    D. Bohrium
    11
    1144 The chemical formula of the oxide of
    Eka – aluminium is:
    A. ( G a O )
    в. ( G a O_{2} )
    c. ( G a_{2} O_{2} )
    D. ( G e_{2} O_{3} )
    11
    1145 The unit of electron affinity is:
    A. kcal/mole
    B. erg-sec
    ( c cdot A^{c} )
    D. no unit
    11
    1146 Which one of the following is least
    chemically reactive?
    ( A cdot A r )
    B.
    ( c cdot s )
    D. Ti
    E.
    11
    1147 Which of the following group bear maximum number of elements?
    ( mathbf{A} cdot 3^{r d} ) group
    B. ( 2^{n d} ) group
    c. ( 18^{text {th }} ) group
    D. ( 13^{text {th }} ) group
    11
    1148 Arrange the following elements in terms of increasing first ionization energy:
    ( boldsymbol{G} boldsymbol{a}, boldsymbol{B} boldsymbol{a}, boldsymbol{R} boldsymbol{u}, boldsymbol{F}, boldsymbol{N} )
    A. ( B a<R u<G a<N<F )
    в. ( G a<B a<R u<F<N )
    c. ( R u<B a<G a<N<F )
    D. None of the above
    11
    1149 Atomic number 56 belongs to which
    block ?
    ( A )
    B. ( p )
    ( c cdot d )
    D. ( f )
    11
    1150 Two elements A and B have the
    following configuration: ( boldsymbol{A}: mathbf{2}, mathbf{7} ; boldsymbol{B} )
    ( 2,8,7 . ) Both of them belong to:
    A. the same group and are chemically similar
    B. different groups but are chemically similar
    C. the same group but are chemically dissimilar
    D. the same period and are chemically similar
    11
    1151 The diagram shows some parts of the
    periodic table with few elements.
    Identify the set of two elements which
    combine together to form a covalent
    compound with a formula of the type
    ( boldsymbol{X} boldsymbol{Y}_{3} )
    A ( cdot 2 ) and 3
    B. 4 and 6
    ( c .5 ) and 7
    D. 1 and 7
    11
    1152 The classification of elements in
    the modern periodic table is based on
    their:
    A. increasing order of their atomic number
    B. atomic weight
    c. atomic volume
    D. equivalent weight
    11
    1153 ( 4^{t h} ) period ends with :
    A . argon
    B. neon
    c. krypton
    D. radon
    11
    1154 Element P has atomic number 19. To
    which group does P belongs to?
    ( mathbf{A} cdot mathbf{1} )
    B. 2
    ( c cdot 17 )
    ( D cdot 16 )
    11
    1155 Which of the following statement about Mendeleev’s periodic table is incorrect?
    A. He leftgaps for some elements which were discovered later and correctly predicted the properties of them
    B. Inert gases could be placed in a new group without disturbing the existing order
    C. He arranged the elements according to the properties of elements
    D. The properties of the elements are the periodic function of their atomic numbers
    11
    1156 Among cellulose, polyvinyl chloride, nylon and natural rubber, in which of the polymer intermolecular force of attraction is weakest?
    A. Nylon
    B. Polyvinyl chloride
    c. cellulose
    D. Natural rubber
    11
    1157 Which of the following elements shown as pairs with their atomic numbers
    belong to the same period?
    A. ( Z=19 ) and ( z=38 )
    B. ( Z=12 ) and ( Z=17 )
    C ( . quad Z=11 ) and ( Z=21 )
    D. ( z=16 ) and ( z=35 )
    11
    1158 DU
    ) CU
    012. Define ionisation enthalpy.
    11
    1159 Out of sodium, chlorine and silicon
    which one is metalloid?
    11
    1160 The long form of the periodic table is
    based on :
    A. number of electrons
    B. mass of the atoms
    c. electronegativity
    D. shape of the atom
    11
    1161 Compared to the first ionization potential, the value of second ionization potential of an element is:
    A. Negligible
    B. Smaller
    c. Greater
    D. Double
    11
    1162 Q17. Define electronegativity. How does it differ from electron gain enthalpy? 11
    1163 Anything that influences the valence electrons will affect the chemistry of the element. Nuclear mass effects
    chemistry of valence electrons.
    A. True
    B. False
    11
    1164 Which is inert gas?
    ( A cdot 1 )
    B. 2
    ( c cdot 3 )
    D. 4
    11
    1165 Assertion
    Newland’s law of octaves of elements is
    a function of their state that the
    property of every eighth element is the repetition of the first.
    Reason
    In order to fit new elements into his
    table Newland adjusted two elements in the same colum.
    A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion.
    B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
    C. Assertion is correct but Reason is incorrect.
    D. Assertion is incorrect but Reason is correct.
    11
    1166 The electronic configuration with the highest ionization enthalpy is:
    A ( cdot[N e] 3 s^{2} 3 p^{1} )
    B ( cdot[A r] 3 d^{10} 4 s^{2} 4 p^{3} )
    ( mathbf{c} cdot[N e] 3 s^{2} 3 p^{3} )
    D. ( [N e] 3 s^{2} 3 p^{2} )
    11
    1167 The screening effect of ( boldsymbol{d} ) electrons is:
    A. much less than ( s ) -electrons
    B. much more than ( s ) -electrons
    c. equal to ( s ) -electrons
    D. equal to ( p ) -electrons
    11
    1168 Which of the following statements is true regarding the typical element belonging to ( 1^{s t} ) group of ( p ) – block elements?

    This question has multiple correct options
    A. The element forms amphoteric oxide
    B. The element forms a sulphate of formula ( M_{2}left(S O_{4}right)_{3} )
    c. The element shows variable valency
    D. The element is a metalloid

    11
    1169 The modern periodic table explains the periodicity of the properties of the elements and relates them to their:
    A. Charge
    B. Electron number
    c. Electronic configuration
    D. Atomic mass
    11
    1170 Which element among those listed below, has the lowest electronegativity?
    A ( . M g )
    в. ( C a )
    ( c . B a )
    D. ( S r )
    E . ( B e )
    11

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