Which of the following statements is correct | vedclass

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(D) The electronic configuration of $Na$ is $[Ne] 3s^1$ and $Mg$ is $[Ne] 3s^2$. For the first ionization enthalpy $(I)$,$Mg$ has a stable fully-fille

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$II(Na) > II(Mg)$

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(D) The electronic configuration of $Na$ is $[Ne] 3s^1$ and $Mg$ is $[Ne] 3s^2$. For the first ionization enthalpy $(I)$,$Mg$ has a stable fully-filled $s$-orbital,so $I(Mg) > I(Na)$. For the second ionization enthalpy $(II)$,$Na^+$ has the stable noble gas configuration $[Ne]$,making it very difficult to remove the second electron. Conversely,$Mg^+$ has the configuration $[Ne] 3s^1$,from which the second electron is relatively easier to remove. Therefore,$II(Na) > II(Mg)$.

Which of the following statements is correct regarding the first $(I)$ and second $(II)$ ionization enthalpies of sodium $(Na)$ and magnesium $(Mg)$?

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The second ionization enthalpy of an element is always higher than its first ionization enthalpy because

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