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(B) The ionization energy $(IE)$ generally increases across a period due to an increase in effective nuclear charge.Elements with half-filled or fully

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$[Ne] \, 3s^{2} \, 3p^{3}$

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(B) The ionization energy $(IE)$ generally increases across a period due to an increase in effective nuclear charge.Elements with half-filled or fully-filled subshells possess extra stability,resulting in higher $IE$ values.Comparing the given configurations:Option $A$ $([Ne] \, 3s^{2} \, 3p^{1})$ is $Al$ (Group $13$).Option $B$ $([Ne] \, 3s^{2} \, 3p^{3})$ is $P$ (Group $15$,half-filled $p$-subshell).Option $C$ $([Ne] \, 3s^{2} \, 3p^{2})$ is $Si$ (Group $14$).Option $D$ $([Ar] \, 3d^{10} \, 4s^{2} \, 4p^{3})$ is $As$ (Group $15$,but in the $4^{th}$ period).Since $IE$ decreases down a group,$P$ ($3^{rd}$ period) has a higher $IE$ than $As$ ($4^{th}$ period).Therefore,the element with the highest $IE$ is $[Ne] \, 3s^{2} \, 3p^{3}$.

Amongst the following elements,the highest ionization energy is

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