Chemistry

1. The properties of the elements are periodic function of their atomic numbers. This statement was given by:
(a) Bohr
(b) Mendeleev
(c) Dobereiner
(d) Moseley
2. Which of the following statements is not correct?
(a) Long form of periodic table is based on atomic numbers and aufbau principle.
(b) Long form of periodic table consists of seven horizontal rows and eighteen vertical columns.
(c) Long form of periodic table was presented by Bohr.
(d) Lanthanides and actinides actually belong to third vertical column of long form of periodic table.
3. Column I —- Column II
(A) Law of triads 1. New land
(B) Law of octaves 2. Mendeleev
(C) Periodic law 3. Moseley
(D) Modified periodic law 4. Dobereiner
The correct match of contents in Column I with those of Column II is :
A B C D
(a) 1 2 3 4
(b) 4 3 2 1
(c) 1 3 4 2
(d) 4 1 2 3
4. Eka-aluminium and eka-silicon are known as :
(a) aluminium and silicon
(b) gallium and germanium
(c) scandium and titanium
(d) stable isotopes of aluminium and silicon
5. The statement that is not correct for periodic classification of elements is:
(a) the properties of the elements are periodic function of their atomic numbers
(b) non-metallic elements are less in number than metallic elements
(c) 63 elements were known when Mendeleev presented the periodic table
(d) for transition elements, the 3d-orbitals are filled with electrons after 3orbitals and before 4s-orbitals
6. The transition elements have a characteristic electronic configuration which can be represented as:
(a) (n-2)S2p6d1-10(n-1)S2 p6ns2
(b) (n-2)S2p6d1-10(n-1)S2p6d1 or 2 ns1
(c) (n-1) S2 p6 d10 ns2 np6 nd1-10
d) (n-1) S2 p6 d1-10 ns1 or 2
7. Which one of the following statements is not correct for modern Mendeleev’s periodic table?
(a) It consists of nine groups
(b) It consists of seven periods
(c) Each group has equal number of elements
(d) Each period except first period starts with the element of alkali group and ends with an element of zero group
8. The first member of lanthanide series is :
(a) lanthanum
(b) cerium
(c) caesium
(d) thorium
9. The elements in which electrons are progressively filled in 4f-orbitals are called:
(a) lanthanoids
(b) actinoids
(c) noble metals
(d) chalcogens
10. (i) Total inner-transition elements are 28.
(ii) Total of-block elements are 40.
(iii) Except hydrogen, all non-metals belong to block series.
(iv) All the members of the actinide series are man-made (synthetic).
The correct statements are:
(a)(i)and(iv)
(b) (i), (ii) and (iii)
(c) (iii) and (iv)
(d) all
11 . Which of the elements whose atomic numbers are given below, cannot be accommodated in the present set up of the long form of periodic table?
(a) 107
(b) 118
(c) 126
(d) 102
12 . The elements which occupy their positions in periodic table just after the members of zero group are:
(a) metals
(b) gases
(c) radioactive
(d) alkali metals
13. An element having electronic configuration [Ar] 3dP2 ,4s2belongs to:
(a) d-block
(b) f-block
(c) s-block
(d) block
14. The electronic configuration of most electropositive element is:
(a) [Xe] 6s2
(b) [Xe] 6s1
(c) [Kr] 5s1
(d) [Kr] 5s2
15. An element ‘X’ with atomic number 114 has recently been discovered. The name of this element is :
(a) eka lead
(b) flerovium
(c) ununfortium
(d) bohrium
16. An element which belongs to third period and group 15 has electronic configuration:
(a) 1s2 , 2s2 2p6 , 3s2 3p3
(b) 1s2 , 2s2 2p3
(c) 1s2 , 2s2 2p6 , 3s2, 3p4
(d) none of these
17. The electronic configuration of gadolinium (At. No. 64) is:
(a) [Xe] 4f3, 5d5, 6S2
(b) [Xe] 4f7, 5d2, 6s1
(c) [Xe]4f7 , 5d1 ,6S2
(d) [Xe] 4f8, 5d0,6S2
18. d-block elements in long form of periodic table are placed:
(a) on the extreme left
(b) on the extreme right
(c) at the bottom
(d) in the middle
19. The element having electronic configuration [Rn] 5fP1414 6dP2 7S2 belongs to:
(a) d-block
(b) s-block
(c) block
(d) f-block
20. The formula of the binary compound formed by the element ‘X’ with atomic number 120 and sulphur is:
(a) X2S
b) XS2
X3S
XS
Europium belongs to:
(a) s-block
(b) block
(c) d-block
(d) f-block
The element of 4th period of the periodic table having maximum number of unpaired electrons in its ground state is:
(a) 20Ca
(b) 30Zn
(c) 24Cr
(d) 28Ni
Which one of the following ions is paramagnetic?
(a) Ag+
(b) Fe2+
(c) K+
(d) Mg2+
Mark the group which has maximum number of elements in Mendeleev’s periodic table:
(a) I
(b) II
(c) III
(d) IV
Diagonal relationship in periodic table is shown by elements of…… and …… periods.
(a) I and II
(b) II and III
(c) III and IV
(d) I and III
An element (X) which occurs in the second period has an outer electronic configuration S2 p1—what is the formula and nature of its oxide?
(a) XO3, basic
(b) X2O3, acidic
(c) X2O3, basic
(d) XO2, acidic
In extended form of the periodic table, one of the following does not having appropriate position:
(a) inner-transition elements
(b) transition metals
(c) noble gases
(d) chalcogens
The most predominantly electrovalent compounds will be obtained from the combination of elements belonging to:
(a) I and VII groups
(b) II and VI groups
(c) III and V groups
(d) none of these
The screening effect of d-electrons is:
(a) much less than s-electrons
(b) much more than s-electrons
(c) equal to s-electrons
(d) equal to electrons
30. The first ionisation enthalpies of Na, Mg, Al and Si are in the order of:
(a) Na < Mg > Al Mg > Al > Si
(c) Na < Mg < Al > Si
(d) Na > Mg > Al < Si 31. Ionisation enthalpy of K would numerically the same as: (a) Electronegativity of K+
(b) Electron gain enthalpy of K+
(c) Electron gain enthalpy of Ar
(d) Ionisation enthalpy of Ca
32. The electronegativity of the following elements increases in the order of:
(a) C, N, Si, P
(b) N, Si, C, P
(c) Si,P,C,N
(d) P,Si,N,C
33. Match List-I with List-II and select the correct answer :
List-I (At. No.)—- List-II (Block)
(A) 43 (1) s-block
(B) 35 (2)block
(C) 38 (3) f-block
(D) 60 (4)d-block
A-2,B-1,C-3,D-4
A-1,B-2,C-3,D-4
A-4,B-3,C-2,D-1
A-3,B-2,C-1,D-4
34. Identify the block in the periodic table in which the elements have nearly similar electro negativities :
(a) s-block
(b) p-block
(c) f-block
(d) d-block
35. Which of the following is not arranged in the correct sequence?
(a) MO,M2O3, MO2, M2O5 — decreasing basic nature
(b) Sc, V, Cr, Mn — increasing number of oxidation states
(c) d5 ,d3 ,d1 ,d4 — increasing magnetic moment
(d) Mn2+, Fe2+, Cr2+, Co2+ — decreasing stability
36. The electronic configuration of four elements are :
(i) [Xe] 6s1
(ii)[Xe]4f14 5d1, 6S2
(iii) [Ne] 3s2 3p5
(iv) [Ar] 3d7 4s2
(a) (i) is a strong reducing agent
(b) (iv) shows variable oxidation states
(c) (iii) has maximum electron gain enthalpy
(d) (ii) is a d-block element
37. In the periodic table which one of the following trends is not correct across the period?
(a) Electronegative to electropositive
(b) Metallic to non-metallic
(c) Reducing to oxidising
(d) Base to acid forming
38. The ions O 2-, F, Na+, Mg 2+ and Al3+ are isoelectronic. Their ionic radii show:
(a) an increase from O 2- to F and then decrease from Na+ to Al 3+
(b) a decrease from O-2 to F and then increase from Na+ to Al3+
(c) a significant increase from O 2- to Al3+
(d) a significant decrease from -2 to Al3+
In the descending order of a vertical group in the periodic table, which of the following would be true?
(i) Electro negativity decreases
(ii) Ionisation enthalpy decreases
(iii) All the atoms have the same number of valence electrons
(iv) Metallic character decreases and the basic nature of their oxides decreases
(a) (ii), (iii) and (iv)
(b) (i), (ii) and (iv)
(c) (i), (iii) and (iv)
(d) (i), (ii) and (iii)
Atomic and ionic radii are expressed in:
(a) mm
(b) angstrom units
(c) cm
(d) nm
Which one of the following grouping represent a collection of isoelectronic species? (At. numbers, Cs = 55 and Br = 35)
N 3-, F, Na+
(b) Ca2+, Cs+, Br
(c) Be, Al3+, Cl
(d) Na+, Ca2+, Mg2+
The formation of O 2-(g) starting from O(g) is endothermic by 639 kJ mol-1 If electron gain enthalpy of O(g) is -141 kJ mol-1 , the second electron gain enthalpy of oxygen would be:
(a) – 780 kJ mol-1
+780Kj.mol-1
(c) + 498 kJ mol-1
(d) – 498 kJ mol-1
Which of the following elements has the maximum electron gain enthalpy?
(a) Oxygen
(b) Chlorine
(c) Fluorine
(d) Nitrogen
The set representing the correct order of first ionisation enthalpy is:
(a) K>Na>Li
(b) Be>Mg>Ca
(c) B > C > N
(d) Ge > Si > C
If we go from Li to F in the second period, there would be a decrease in:
(a) atomic mass
(b) atomic radii
(c) ionisation enthalpy
(d) electronegativity
The correct order of atomic or ionic size is:
(a)N < Li < B (b) Ca 2+ < S 2- < Cl
(c) Na + < Mg 2+ < Cl
(d) Cl < Mg < Ca The correct order of atomic radii or ionic radii is: (a) Na < Be < B (b) F < O 2- < N 3-
(c)Na < Li 3+ < Fe 2+ < Fe 4+
48. Which of the following is the smallest cation ?
(a) Na+
(b) Mg2+
(c) Al3+
(d) Ca2+
49. Which of the following statements is wrong?
(a) In a period of normal elements, the atomic radii decreases from left to right
(b) Cation is always smaller in size than normal atom
(c) In a period of normal elements, the atomic radii increases from left to right
(d) Anion is always larger in size than normal atom
50. Transition metals are characterised by the properties except:
(a) variable valency
(b) coloured compounds
(c) high melting and boiling points
(d) no tendency to form complexes
51. The ionisation enthalpy 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
52. The ionic radius of a cation is always:
(a) less than atomic radius
(b) more than atomic radius
(c) equal to atomic radius
(d) cannot be predicted
53. The maximum ionisation enthalpy in a period is shown by.
(a) halogens
(b) alkali metals
(c) chalcogens
(d) inert gases
54. Which of the following statements is incorrect?
(a) Among all the elements, fluorine has the highest electron gain enthalpy
(b) Among all the elements, helium has the highest ionisation enthalpy
(c) Elements of groups 1,2,13,14,15,16and 17are called representative elements
(d) All the af-block elements are metallic in nature
55. Lowest ionisation enthalpy in periods is shown by:
(a) inert gases
(b) halogens
(c) alkali metals
(d) alkaline earth metals
56. The elements with atomic numbers 10, 18, 36, 54 and 86 are all:
(a) light metals
(b) inert gases
(c) halogens
(d) rare-earths
57. Among the following, the highest ionisation energy is shown by :
[Ne] 3s2 3p3
[Ar] 3d10 4s2 4p3
(c) [Ar] 3d10 4s2 4p4
(d) [Ne] 3s2 3p4
58. Which of the following atoms has the largest atomic radius?
(a) Cs
(b) Ba
(c) Pb
(d) Cu
59. Electron gain enthalpy of:
(a) carbon is higher than oxygen
(b) sulphur is lesser than oxygen
(c) iodine is higher than bromine
(d) chlorine is higher than fluorine
60. The correct order of relative stability of half filled and completely filled shells is :
(a) p3 < d5 < d 10 < p6
(b) d5>p3>d10>p6
(c) p3 < d10 < d 5 6
(d) d5 < P3 < d10 < p6
61. An element has successive ionisation enthalpies as 800 (first), 2427, 3658,25024, 32824 kJ mol -1. To which group of the periodic table does this element belong?
(a) 16
(b) 15
(c) 13
(d) 14
62. The valency shell of element A contains 3 electrons while the valency shell of element B contains 6 electrons. If A combines with B, the probable formula of the compound formed will be:
(a) AB2
(b) A2B
(c) A2B3
(d) A3 B 2
63. The electronic configuration of four elements are given below. Which element does not belong to the same family as others?
(a) [Xe]4f14 5d10 6S2
(b) [Kr]4d10 5s2
(c) [Ne] 3s2 3p2
(d) [Ar]3d10 4s2
64. The most non-metallic element among the following is:
(a) 1s2, 2s2 2p6
(b) 1s2, 2s2 2p5
(c) 1s2,2s2 2p4
(d) 1s2, 2s2 2p3
65. The atomic numbers of the other elements which lie in the same group as the ninth element in the periodic table are:
(a) 18,32,54,86
(b) 8, 18, 36, 84
(c) 8,16,34,52
(d) 17,35,53,85
66. Which of the following has lowest ionisation energy?
(a) Sulphur
(b) Oxygen
(c) Fluorine
(d) Nitrogen
67. Atoms of which of the following groups lose electrons most easily?
(a) Li, Na, K
(b) Cl, Br, I
(c) O, S, Se
(d) N, P, As
68. The electronic configuration of an element is 1s2,2s2 2p6,3s2 3p5. The atomic numbers of the elements just above and below this element and the group number (extended form) to which these belong are respectively:
(a) 9, 25 (Group number 17)
(b) 9, 35 (Group number 17)
(c) 9, 25 (Group number 7)
(d) 9, 35 (Group number 7)
69. Which of the following element has highest metallic character?
Element — I.E.
(a)-419 kJ mol-1
(b)Q—737 kJ mol-1
(c)R–590 kJ mol-1
(d) S —370 kJ mol-1
70. Electron gain enthalpies of O, F, S and Cl are in the order:
(a) O < S < Cl < F (b) S < O < Cl < F (c) O < S < F –orbitals are more stable
(c) nitrogen atom is small
(d) more penetration effect
73. Lanthanide contraction explains:
(a) density of the series
(b) atomic volume of the series
(c) chemical activity of the series
(d) size of the atoms of the series
74. The outermost electronic configuration of the most electronegative element is:
(a) ns2 np3
(b) ns2 np4
(c) ns2 np5
(d) ns2 np6
75. Which one is not correct order of electronegativity?
(a) F > Cl > Br > I
(b) Si > Al > Mg > Na
(c) Cl > S > P > Si
(d) None of these
76. The electronic configuration of the element which is just above the element with atomic number 43 in the same periodic group is:
(a) 1s2,2s2,2p6,3s2,3p6,3d5,4s2
(b) 1s2,2s2,2p6,3s2,3p6,3d10,4s2,4p5
(c) 1s2,2s2,2p6,3s2,3p6,3d6,4s1
(d)1s2,2s2,2p6,3s2,3p6,3d10,4s1,4p6
77. The statement that is not correct for the periodic classification of elements is:
(a) The properties of elements are periodic functions of their atomic numbers.
(b) Non-metallic elements are lesser in number than metallic elements.
(c) The first ionisation energies of the elements along the periods do not vary in a regular manner with the increase in atomic number.
(d) For transition elements the d-subshells are filled with electrons monotonically with increase in atomic number.
78. Among the following, the element which is not liquid at room temperature (30 0 C) is:
(a) Ga
(b) Ge
(c) Cs
(d) Br
79. Which of the block of elements does belong to inert gases?
(a) s-block
(b) p-block
(c) d-block
(d) f-block
80. Which of the following elements has the lowest ionisation enthalpy?
(a) Na
(b) K
(c) Mg
(d) Al
81. Which one of the following is smallest in size?
(a) Na+
(b) O 2-
(c) N 3-
(d) F
82. Which of the following has the lowest ionisation enthalpy?
(a) 4s1
(b) 3d2
(c) 3p6
(d) 2p6
83. Of the following elements, which one has the highest electronegativity?
(a) I
(b) Br
(c) Cl
(d) F
84. The element with positive value of electron gain enthalpy is:
(a) hydrogen
(b) oxygen
(c) lithium
(d) neon
85. Among the following outermost configurations of transition metals which shows the highest oxidation state, is:
(a) 3d3 , 4s2
(b) 3d5,4s1
(c) 3d5,4s2
(d) 3d6,4s2
86. Which of the following ions has the lowest magnetic moment?
(a) Cu2+
(b) Ni2+
(c) Co3+
(d) Fe2+
87. Which of the following have no unit?
(a) Electron gain enthalpy
(b) Electronegativity
(c) Ionisation enthalpy
(d) Atomic radii
88. The order of electron gain enthalpy of B, C, N and O is:
(a)O>C>N>B
(b)B>N>C>O
(c)O>B>C>N
(d) O > C> B > N
89. Which of the following set of ions represents a collection of isoelectronic species?
(a) Ba2+, Sr2+, K+, Ca2+
(b) K+, Cl , Ca2+, Sc3+
(c) N 3-, O 2-,F, S 2-
(d) Li +, Na +, Mg2+, Ca2+
90. Aluminium is diagonally related to:
(a) Li
(b) Si
(c) Be
(d) B
91. In the sixth period of the extended form of periodic table, the orbitals are filled as:
(a) 6s, 5f, 6d, 6p
(b) 5s. Sp, 5d, 6p
(c) 6s, 6p, 6d, 6f
(d) 6s, 4f, 5d, 6p
92. Gradual addition of electronic shells in the noble gases causes a decrease in their:
(a) ionisation enthalpy
(b) atomic radius
(c) boiling point
(d) density
93. Which one of the following belongs to representative group of elements in the periodic table?
(a) Lanthanum
(b) Argon
(c) Chromium
(d) Aluminium
94. An element of atomic number 29 belongs to:
(a) s-block
(b)p-block
(c)d-block
(d) f-block
95. A trend common to both groups 1 and 17 elements in the periodic table as atomic number increases is:
(a) increase in oxidising nature
(b) increase in atomic radius
(c) increase in maximum valency
(d) increase in reactivity with water
96. Which of the following has largest radius?
(a) O 2-
(b) Mg2+
(c) Na +
(d) F
97. Which one is the correct order of the size of the iodine species?
(a) I > I+ > I
(b) I > I > I +
(c) I+ >I > I
(d) I > I> I +
98. Which of the following configurations represents atoms of element having a large difference between first and the second ionisation energy?
(a) 1s2, 2s2, 2p4
(b) 1s2, 2s2, 2p6
(c) 1s2, 2s2,2p6, 3s1
(d) 1s2, 2s2,2p6, 3s2
99. In which of the following arrangements, the order is not according to the property indicated against it?
(a) Al3+ < Mg2+ < Na + < F increasing ionic size
(b) B < C < N < O increasing first ionisatioii enthalpy (c) I < Br < F < Cl increasing electron gain enthalpy_ (with negative sign) (d) Li < Na < K < Rb increasing metallic radius 100. The electronic configurations of four elements are given below. Arrange these elements in the correct order of magnitude (without sign) of their electron gain enthalpy:
(i)2s2,2p5
(ii) 3s2,3p5
(iii) 2s2,2p4
(iv) 3s2,3p4
Select the correct answer:
i, ii, iii, iv
ii, i, iv, iii
iii, iv, ii, i
iii, iv, i, ii
101. In the long form of the periodic table, all the non-metals are placed with:
(a) 5-block
(b) p-block
(c) d-block
(d) f-block
102. The lanthanide contraction is responsible for the fact that:
(a) Zr and Y have about the same radius
(b) Zr and Nb have similar oxidation state
(c) Zr and Hf have about the same radius
(d) Zr and Zn have the same oxidation state
103. Of cobalt and zinc salts, which are attracted in magneticfield?
(a) Cobalt salts
(b) Zinc salts
(c) Both
(d) None
104. The electronic configuration of an element is 1s2, 2s2 2p6, 3s2 3p3. What is the atomic number of the element which is just below the above element in the periodic table?
(a) 34
(b) 49
(c) 33
(d) 31
105. Element X belongs to 4th period. It contains 18 and 1 electrons in the penultimate and ultimate orbit. The X should be:
(a) normal element
(b) transition element
(c) inert gas
(d) inner-transition element
106. Electron gain enthalpy of X would be equal to:
(a) electron affinity of X
(b) ionisation potential of X
(c) ionisation potential of X
(d) none of the above
107. Pauling’s electronegativity scale is based on experimental value of:
(a) atomic radii
(b) bond lengths
(c) ionic radii
(d) bond energies
108. Most of the man-made synthetic elements occur:
(a) in actinide series
(b) in lanthanide series
(c) in coinage metals
(d) in alkaline earth metals
109. Which is the largest stable atom?
(a) V
(b) Na
(c) Al
(d) Pb
110. Which of the following is strongest base?
(a) Be(OH)2
(b) Mg(OH)2
(c) A1(OH)3
(d) Si(OH)4
111. Which has largest atomic size?
(a) Al
(b) Al2+
(c) Al3+
(d) Al +
112. Which one of the following indicate the correct order of atomic size?
(a)Be>C>F>Ne
(b)Ne>Be>C>F
(c) Be < C < F < Ne (d) F < Ne < Be < C 113. Which of the following is not correct ? (a) N3 > O 2- > F : Ionic radii
(b)s>p>d : Ionisation energy
(c) Cl > F > Br : Electron gain enthalpy
(d) P > N > O : Electronegativity
114. The incorrect statement among the following is:
(a) The first ionisation potential of Al is less than the first ionisation potential of Mg
(b) The second ionisation potential of Mg is greater than the second ionisation potential of Na
(c) The first ionisation potential of Na is less than the first ionisation potential of Mg
(d) The third ionisation potential of Mg is greater than third ionisation potential of Al
115. Which of the following orders is wrong?
(a) NH3 < PH3 < AsH3 – Acidic
(b) Li < Be < B < C – IE1
(c) Al2O3 < MgO < Na2O < K2O – Basic
(d) Li+ < Na + < K+ < Cs + — Ionic radius
116. An element has successive ionisation energies as 940, 2080, 3090, 4140, 7030, 7870, 16000 and 19500 kJ mol”1. To which group of the periodic table does this element belong?
(a) 16
(b) 15
(c) 14
(d) 17
117. Two elements whose electronegativities are 1.2 and 3.0, the bond formed between them would be:
(a) ionic
(b) covalent
(c) coordinate
(d) metallic
118. Chloride ion and potassium ion are isoelectronic. Then:
(a) their sizes are same
(b) Cl ion is bigger than K+ ion
(c) K+ ion is relatively bigger
(d) their sizes depend on other cation and anion
119. Identify the least stable ion amongst the following:
(a) Li
(b) Be
(c) B
(d) C
120. Increasing order of electron gain enthalpy is:
(a) N < O < Cl < Al (b) O < N < Al< Cl (c) Al< N < O < Cl (d) Cl< N < O < Al 121. Which of the following sets is of coinage metals? (a) Cu, Ag, Au (b) Zn, Cd, Hg (c) Au, Ag, Zn (d) Li, Na, K 122. According to modern periodic law, variations in the properties of elements is related to their: (a) atomic weights (b) nuclear weights (c) atomic numbers (d) neutron-proton ratios 123. Which of the following has maximum ionisation enthalpy? (a) K (b) Na (c) Mg (d) Be 124. The reduction in atomic size with increase in atomic numbers is characteristic of elements of: (a) radioactive series (b) high atomic masses (c) d-block (d) f-block 125. General electronic configuration of outermost and penultimate shell is (n - 1) S2 (n -1)p6(n – 1)d x ns2. If n = 4 and x = 5, then number of protons in the nucleus will be:
(a) > 25
(b) < 24 (c) 25 (d) 30 126. Increasing order of density is: (a) Li < K < Na < Rb 1, 3d10 3d5
(b) 4s2, 3d10 3dP4
(c)4s1,3dP9 3dP4
(d) 4s1,3d10 3dP6
128. Identify the wrong statement in the following:
(a) Amongst isoelectronic species, the smaller the positive charge on the cation, smaller is the ionic radius.
(b) Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius.
(c) Atomic radius of the elements increases as one moves down the first group of the peroidic table.
(d) Atomic radius of the elements decreases as one moves across from left to right in the second period of the periodic table.
129. With which of the following electronic configuration an atom has the lowest ionisation enthalpy?
(a) 1s2,2s2 2p3
(b) 1s2, 2s2 2p6, 3s1
(c) 1s2, 2s2 2p6
(d) 1s2, 2s2 2p5
130. In which one of the following pairs the radius of the second species is greater than that of the first?
(a)Na,Mg
(b) O 2-,N 3-
(c) Li +, Be2+
(d) Ba2+, Sr2+
131. Which of the following is a favourable factor for cation formation?
(a) High electronegativiry
(b) High electron gain enthalpy
(c) Low ionisation enthalpy
(d) Smaller atomic radius
132. The electronic configuration of the atom having maximum difference in first and second ionisation energies is:
(a) 1s2,2s2 2p6, 3s1
(b) 1s2, 2s2 2p6, 3s2
(c) 1s2,2s2 2p1
(d) 1s2, 2s2 2p6, 3s2 3p3
133. Which of the following has lowest ionisation energy?
(a) Oxygen
(b) Nitrogen
(c) Fluorine
(d) Sulphur
134. The electronic configuration of the element with maximum electron affinity is:
(a) 1s2,2s2 2p3
(b) 1s2, 2s2 2p5
(c) 1s2,2s2 2p6, 3s2 3p5
(d) 1s2, 2s2 2p6, 3s2 3p3
135. The first ionisation energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?
(a) Lesser effective nuclear charge of oxygen than nitrogen
(b) Lesser atomic size of oxygen than nitrogen
(c) Greater inter-electron repulsion between two electrons in the same orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen
(d) Greater effective nuclear charge of oxygen than nitrogen
136. Column I —– Column II
(A) He (i) High electron gain enthalpy
(B) Cl (ii) Most electropositive element
(C) Ca (iii) Strongest reducing agent
(D) Li (iv) Highest ionisation energy
The correct match of contents in Column I with those in Column II is:
(a) A—(iii), B—(i), C—(ii), D—(iv)
(b) A-(iv), B—(iii), C—(ii), D-(i)
(c) A—(ii), B—(iv), C—(i), D—(iii)
(e) A-(iv), B—(i), C—(ii), D-(iii)
137. In the descending order of a vertical group of normal elements in the periodic table, which of following would be true?
(i) Electronegativity decreases
(ii) Ionisation enthalpy decreases
(iii) All atoms have same number of valence electrons
(iv) Metallic character decreases
Mark the correct alternative :
(a) (ii), (iii) and (iv)
(b) (i), (ii) and (iv)
(c) (i), (ii) and (iii)
(d) (i), (iii) and (iv)
138. The correct order of increasing electron affinity of halogens is:
(a)F2
< SiO2 < SnO2 < PbO2 : increasing oxidising power
(b) HF < HCl < HBr < HI: increasing acid strength (c) NH3 < PH3 < AsH3 < SbH3: increasing basic strength
(d) B < C < O < N: increasing first ionisation energy 140. The set representing the correct order of ionic radius is: (a) Li + > Be2+ > Na + > Mg2+
(b) Na + > Li + > Mg2+ > Be2+
(c) Li + > Na + > Mg 2+ > Be2+
(d)Mg 2+>Be 2+>Li +>Na +
141. The correct order of ionisation energy of C, N, O, F is :
(a)F+ is 19.6 x 10 -18 J atom 1. The energy of the first stationary state (n = 1) of Li 2+ is:
(a) 8.82 x 10 7 J atom-1
(b) 4.41 x 10 -16 J atom-1
(c) – 4.41 x10-17 J atom-1
(d) -2.2 x 10P15 J atom-1
143. The correct sequence which shows decreasing order of the ionic radii of the elements is:
(a) O 2- > F > Na + > Mg2+ > Al3+
(b) Al 3+ > Mg 2+ > Na + > F > O 2-
(c) Na + > Mg 2+ > Al 3+ > O 2- > F
(d) Na + > F > Mg2+ > O 2-> Al 3+
144. The second ionisation energy is maximum for:
(a) aluminium
(b) boron
(c) magnesium
(d) beryllium
145. Second ionisation energies of Li, Be and B are in order of:
(a) Li > Be > B
(b) Li > B > Be
(c) Be > Li > B
(d) B > Be > Li
146. In a periodic table, the basic character of oxides:
(a) increases from left to right and decreases from top to bottom
(b) decreases from right to left and increases from top to bottom
(c) decreases from left to right and increases from top to bottom
(d) decreases from right to left and decreases from top to bottom
147. Which of the following orders regarding ionization energy is correct?
(a)N>O>F
(b)N<00F
148. The diagonal partner of element Bis:
(a) Li
(b) Al
(c) Si
(d) Mg
149. The first (δiH1) and second (δiH2) ionisation enthalpies (in kJ mol-1) and the electron gain enthalpy (δeg H) in kJ mol-1 of elements I, II, III, IV and V are given below:
Element —-(δiH1)– (δiH2)—- (δeg H)
I—- 520— 7300—– -60
II— 419 —3051—– -48
III —1681 —3374—- -328
IV— 1008 — 1846 —– -295
V— 2372 — 5251—– +48
The most reactive metal and least reactive non-metal of these are respectively:
(a) I and V
(b)Vandll
(c) II and V
(d) IV and V
150. The electron affinity values of elements A,B,C and D are respectively -135, -60, -200 and -348 kJ mol-1. The outer electronic configuration of B is:
(a) 3s2 3p5
(b) 3s2 3p4
(c) 3s2 3p3
(d) 3s2 3p2
151. If n = 6, the correct sequence of filling of electrons will be:
(a) ns ——> (n – 2)f——> (n – 1)d——> np
(b) ns ——> (n – 1)d——> (n – 2)f——> np
(c) ns ——> (n – 2)f——> np——> (n – 1)d
(d) ns ——> np ——> (n – 1)d——»(n- 2)f
152. Which one of the following orders represents the correct sequence of increasing basic nature of the given oxides?
(a) Al2O3 < MgO < Na2O < K2O
(b) MgO < K2O < Al2O3 < Na2O
(c) Na2O < K2O < MgO < Al2O3
(d) K2O < Na2O < Al2O3 < MgO 153. The correct order of decreasing electronegativity values among the elements beryllium (I), oxygen (II), nitrogen (III) and magnesium (IV) is: (a) (II) > (III) > (I) > (IV)
(b) (III) > (IV) > (II) > (I)
(c) (I) > (II) > (III) > (IV)
(d) (I) > (II) > (IV) > (III)
154. The correct decreasing order of first ionisation enthalpies of five elements of the second period is:
(a) Be > B > C > N > F
(b) N > F > C > B > Be
(c) F>N>C>Be>B
(d) N>F>B>C >Be
155. Generally, the first ionisation energy increases along a period but there are some exceptions. The one which is NOT an exception is:
(a) Na and Mg
(b) Be and B
(c) N and O
(d) Mg and Al
156. The increasing order of ionic radii of the given isoelectronic species is:
(a) S 2-, Cl Ca2+, K
(b) Ca 2+, K +, Cl , S 2-
(c) KP +, SP 2-, Ca2+, Cl
(d) Cl, Ca 2+, K +, S 2-
157. Which of the following is correct?
(a) Radius of Ca 2+ < Cl < S 2-
(b) Radius of Cl < S2 < Ca 2+
(c) Radius of S 2- = Cl = Ca 2+
(d) Radius of S 2- < Cl < Ca2+
158. The correct order of electronegativities of N, O, F and P is:
(a) F > N > P > O
(b) F> O>P>N
(c)F>O>N>P
(d)N>O>F>P
159. Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, Se, S and Ar?
(a) Ca < Ba < S < Se < Ar (b) Ca < S < Ba < Se < Ar (c) S < Se < Ca < Ba < Ar (d) Ba < Ca < Se < S < Ar 160. The first ionization potential of Na is 5.1 eV. The value of electron gain enthalpy of Na+ will be: (a) + 2.55 eV (b) - 2.55 eV (c)-5.1eV (d) - 10.22 eV 161. Which of the following noble gases has the highest positive electron gain enthalpy value? (a) He (b) Kr (c) Ar (d) Ne 162. Among the elements B, Mg, Al and K, the correct order of increasing metallic character is: (a) B < Al< Mg < K (b) B < Mg < Al< K (c) Mg< B < Al< K (d) Mg< Al-1
(b) 575 kJ mol-1
(c) 801 kJ mol-1
(d) 419 kJ mol-1
164. The correct arrangement for the ions in the increasing order of their radii is:
(a) Na +, Cl ,Ca 2+
(b) Ca 2+, K +, S 2-
(c) Na +, Al 3+,Be 2+
(d) Cl ,F ,S 2-