A) \[A{{l}^{3+}}<M{{g}^{2+}}<N{{a}^{+}}<{{F}^{-}}\] (Increasing ionic size)
B) \[B<C<N<O\] (Increasing first ionisation energy)
C) \[I<Br<F<Cl\] (Increasing electron gain enthalpy)
D) \[Li<Na<K<Rb\] (Increasing metallic radius)
Correct Answer: B
Solution :
The order of\[I{{E}_{1}}\]of\[B,C,O\]and N is as \[B<C<P<N\] \[I{{E}_{1}}\]of\[N(1{{s}^{2}},2{{s}^{2}},2{{p}^{3}})\]is more than that of\[O\] \[(1{{s}^{2}},2{{s}^{2}},2{{p}^{4}})\]due to presence of extra stable half filled 2p-subshell in (he valence shell.
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