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(C) The electronic configurations of $Na^+$,$Ne^+$,$Mg^+$,and $Al^+$ (after the removal of the first electron) are as follows:$Na^+: 1s^2, 2s^2, 2p^6$

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$Mg < Al < Ne < Na$

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(C) The electronic configurations of $Na^+$,$Ne^+$,$Mg^+$,and $Al^+$ (after the removal of the first electron) are as follows:$Na^+: 1s^2, 2s^2, 2p^6$ (Stable noble gas configuration)$Ne^+: 1s^2, 2s^2, 2p^5$$Mg^+: 1s^2, 2s^2, 2p^6, 3s^1$$Al^+: 1s^2, 2s^2, 2p^6, 3s^2$Ionisation energy depends on the stability of the electronic configuration,effective nuclear charge,and atomic size.$Na^+$ has a stable noble gas configuration $(2p^6)$,making the removal of a second electron extremely difficult,resulting in the highest $IE_2$.$Mg^+$ has a $3s^1$ configuration,which is relatively easy to remove compared to the others.$Al^+$ has a $3s^2$ configuration,which is more stable than $Mg^+$.$Ne^+$ has a $2p^5$ configuration,which is more stable than $Al^+$.Thus,the correct order of $IE_2$ is $Mg < Al < Ne < Na$.

Which one of the following is the correct order of the second ionisation potential of $Na$,$Ne$,$Mg$,and $Al$?

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