$\begin{matrix} List I & List II (A) N, F, O, Li & (P) Increasing order of |EA| (B) F, N, Si, Mg, Rb & (Q) Increasing order of {IE}_{1} (C) K, Na, Al, Mg & {(R) Increasing order of IE}_{2} (D) N, B, O, Cl & (S) Incresing order of radius \end{matrix}$
Which of the following is the only CORRECT combination?

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

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

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

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

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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 $(L i^{+} : 1 s^{2})$ , it has the highest second ionization energy followed by $(O^{+} : 2 s^{2} 2 p^{3})$ which has half filled electronic configration. Hence, $I E_{2}$ for the given elements follows the order: $N < F < O < L i$

(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: $F < N < S i < M g < R b$

(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 $M g$ , its IE will be greater than $A l$ .
$K < N a < A l < M g$

(D) $E A$ 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: $N < B < O < C l$

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Similar questions

Q. Among the following, the isoelectronic species is/ are:
(i)

O^{2 -}, F^{-}, N a^{+}, M g^{2 +}

(ii)

N a^{+}, M g^{+}, A l^{3 +}, F^{-}

(iii)

N^{3 -}, O^{2 -}, F^{-}, N e

Q. The correct order of atomic radii for the following isoelectronic species

F^{-}, O^{2 -}, N a^{+}, M g^{2 +}

is:

Question 17
Arrange the following elements in the order of their decreasing metallic character
Na, Si, Cl, Mg, Al

(a) Cl > Si >Al > Mg >Na
(b) Na >Mg >Al >Si > Cl
(c) Na > Al > Mg > Cl > Si
(d) Al > Na> Si > Ca> Mg

The first ionistation enthalpies of Na, Mg, Al, and Si are in the order
(a) Na< Mg > Al < Si (b) Na> Mg > Al > Si
(c) Na< Mg< Al< Si (d) Na> Mg> Al < Si

A water contains the following dissolved ions.
$[N a^{+}] = 56 m g / L; [C a^{2 +}] = 40 m g / L;$
$[M g^{2 +}] = 30 m g / L; [A l^{3 +}] = 3 m g / L;$
$[H C O_{3}^{-}] = 190 m g / L; [C l^{-}] = 165 m g / L;$
Water $p H$ is $7$ .
Atomic weights:
$C a = 40, M g = 24, A l = 27, H = 1, C = 12, O = 16, N a = 23, C l = 35.5$

The non-carbonate hardness of the sample in $m g / L$ as $C a C O_{3}$ is

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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?