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(B) $1$. The first ionization potential $(IE_1)$ of $Mg$ $(3s^2)$ is higher than $Al$ $(3s^2 3p^1)$ due to the stable fully-filled $s$-orbital. Statem

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The second ionization potential of $Mg$ is greater than the second ionization potential of $Na$.

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(B) $1$. The first ionization potential $(IE_1)$ of $Mg$ $(3s^2)$ is higher than $Al$ $(3s^2 3p^1)$ due to the stable fully-filled $s$-orbital. Statement $A$ is correct.$2$. $Na^+$ has a stable noble gas configuration $(1s^2 2s^2 2p^6)$. Removing a second electron from $Na^+$ requires significantly more energy than removing a second electron from $Mg^+$ $(3s^1)$. Thus,the second ionization potential $(IE_2)$ of $Na$ is much greater than that of $Mg$. Statement $B$ is incorrect.$3$. $IE_1$ of $Na$ $([Ne] 3s^1)$ is less than $Mg$ $([Ne] 3s^2)$. Statement $C$ is correct.$4$. $Mg^{2+}$ has a stable noble gas configuration $(1s^2 2s^2 2p^6)$. Removing a third electron from $Mg^{2+}$ requires much higher energy than removing a third electron from $Al^{2+}$ $(3s^1)$. Statement $D$ is correct.

Element	Ionization energy $1^{st}$ $(kJ/mol)$	Ionization energy $2^{nd}$ $(kJ/mol)$
$X$	$495$	$4563$
$Y$	$731$	$1450$

The incorrect statement among the following is:

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