Which of the following statements is wrong?

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(B) The electronic configuration of $Mg$ is $[Ne] 3s^2$ and $Na$ is $[Ne] 3s^1$. After the removal of one electron,$Mg^+$ becomes $[Ne] 3s^1$ and $Na^

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

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(B) The electronic configuration of $Mg$ is $[Ne] 3s^2$ and $Na$ is $[Ne] 3s^1$. After the removal of one electron,$Mg^+$ becomes $[Ne] 3s^1$ and $Na^+$ becomes $[Ne] 2s^2 2p^6$ (stable noble gas configuration). Since $Na^+$ has a stable noble gas configuration,it is extremely difficult to remove a second electron from it. Therefore,the second ionization potential of $Na$ is significantly higher than that of $Mg$. Thus,the statement that the second ionization potential of $Mg$ is greater than that of $Na$ is incorrect.

Element	$A, B, C$
$IE_1$	$400, 550, 1150$
$IE_2$	$2650, 1070, 2090$

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