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(D) Ionisation energy generally increases across a period due to a decrease in atomic size and effective nuclear charge.Comparing the configurations:$

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$Ne [3s^2 3p^3]$

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(D) Ionisation energy generally increases across a period due to a decrease in atomic size and effective nuclear charge.Comparing the configurations:$A: [Ne] 3s^2 3p^2$ (Period $3$,Group $14$)$B: [Ar] 3d^{10} 4s^2 4p^3$ (Period $4$,Group $15$)$C: [Ne] 3s^2 3p^1$ (Period $3$,Group $13$)$D: [Ne] 3s^2 3p^3$ (Period $3$,Group $15$)Elements in Period $3$ have smaller atomic radii than those in Period $4$,so elements in Period $3$ generally have higher ionisation energies than those in Period $4$.Among the Period $3$ elements $(A, C, D)$,the configuration $[Ne] 3s^2 3p^3$ corresponds to a half-filled $p$-orbital,which is exceptionally stable.Therefore,$[Ne] 3s^2 3p^3$ has the highest ionisation energy.

Amongst the elements with the following electronic configurations,which one of them may have the highest ionisation energy?

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