corresponding monovalent cation of the respective atom. For $I E_{2}$, electronic configuration of
$C^{+}, N^{+}, O^{+}$ and $F^{+}$ -ions which are as follows. $C^{+}=2 s^{2}, 2 p 1$
$N^{+}=2 s^{2}, 2 p^{2}$
$O^{+}=2 s^{2}, 2 p^{3}$
$F^{+}=2 s^{2}, 2 p^{4}$
$\because O^{+}$ is half-filed configuration, obviously it is most stable and greater ionisation energy than
$F^{+}$ as well as $N^{+}$.
The ionisation energy of an element depends upon its size as. Hence, correct order will be, $O>$ $F>N>C$
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$(a)\,\,B\,\,\,\,\,\,\,\,\,\,(b)\,\,Mg\,\,\,\,\,\,\,\,\,\,\,\,(c)\,\,Li\,\,\,\,\,\,\,\,\,\,\,\,(d)\,\,Al\,\,\,\,\,\,\,\,\,\,\,(e)\,\,K$
$'X'$ cannot be