Question

List IList II(A) N, F, O, Li(P) Increasing order of |EA|(B) F, N, Si, Mg, Rb(Q) Increasing order of IE1(C) K, Na, Al, Mg(R) Increasing order of IE2(D) N, B, O, Cl(S) Incresing order of radius Which of the following is the only CORRECT combination?

A
A-S; B-R; C-P; D-Q
B
A-S; B-Q; C-Q; D-P
C
A-R; B-S; C-Q; D-P
D
A-P; B-Q; C-R; D-S

Solution

The correct option is C A-R; B-S; C-Q; D-P(A) Ionisation energy increases from left to right in a period due to increase in effective nuclear charge which bound the outermost electrons strongly. However, due to noble gas configuration of (Li+:1s2) , it has the highest second ionization energy followed by (O+:2s22p3) which has half filled electronic configration.  Hence, IE2 for the given elements follows the order: N<F<O<Li (B) On moving along the group from top to bottom atomic radius increases and while moving left to right in a preriod it decreases. Hence the radius follows the order: F<N<Si<Mg<Rb (C) Ionisation energy decreases down the group due to increase in number of shells and increases as we move from left to right. However due to filled electronic configuration of Mg, its IE will be greater than Al. K<Na<Al<Mg (D) EA refers the amount of energy released when an electron is added to a neutral atom. Electron affinity increases as we move from left to right along a period. However, due to half filled configuration, N has the least EA. So correct order of electron affinity will be: N<B<O<Cl  Chemistry

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