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Question

Match the increasing orders given in column I with the property(ies) given in column II.

Column I Column II
(A) Na+<F−<O2−<N3− (p) electronegativity
(B) Li+ < Na+ < K+ < Rb+ < Cs+ (q) Ionisation energy
(C) O<S<F<Cl (r) Size
(D) Cl−<K+<Ca2+<Sc3+ (s) Electron affinity

A
(A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
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B
(A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
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C
(A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
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D
(A-r) ; (B-q) ; (C-s) ; (D-p, q, s)
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Solution

The correct option is C (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
(A-r) ; (B-q,r) ; (C-s) ; (D-p, q, s, t)
(A-r) For isoelectronic species, the ionic size decreases with increase in nuclear charge. correct order of anionic size is Na+<F<O2<N3
(B- r) Number of atomic shells increases, ionic size increases.
correct cationic size is Li+ < Na+ < K+ < Rb+ < Cs+
(C-s) Correct order ; as Cl has less inter electronic repulsions than F due to bigger size of 3p- subshell so, the correct order of electron affinity is O<S<F<Cl
(D- p,q,s)
Cl<K+<Ca2+<Sc3+
Oxidation state increases, the electronegativity increases. For isoelectronic species ionisation energy and electron affinity increases with increasing nuclear charge.

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