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(D) The electronic configuration of $Na$ $(Z=11)$ is $[Ne] 3s^1$. After losing one electron,it achieves the stable noble gas configuration of $Ne$ $(1

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$II_{Na} > II_{Mg}$

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(D) The electronic configuration of $Na$ $(Z=11)$ is $[Ne] 3s^1$. After losing one electron,it achieves the stable noble gas configuration of $Ne$ $(1s^2 2s^2 2p^6)$.Removing the second electron from this stable configuration requires a very high amount of energy.The electronic configuration of $Mg$ $(Z=12)$ is $[Ne] 3s^2$. After losing one electron,it becomes $[Ne] 3s^1$,which is relatively easier to ionize further compared to the stable $Ne$ core of $Na^+$.Therefore,the second ionization potential of sodium is significantly higher than that of magnesium,i.e.,$II_{Na} > II_{Mg}$.

Which of the following relations is correct with respect to the first $(I)$ and second $(II)$ ionization potentials of sodium $(Na)$ and magnesium $(Mg)$?

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