Which of the following statements is incorrec | vedclass

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(B) The electronic configurations are: $Mg: [Ne] 3s^2$ $Na: [Ne] 3s^1$ Since $Mg$ has a fully filled $3s$ orbital,its first ionization energy $(IE_1)$

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

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(B) The electronic configurations are: $Mg: [Ne] 3s^2$ $Na: [Ne] 3s^1$ Since $Mg$ has a fully filled $3s$ orbital,its first ionization energy $(IE_1)$ is higher than that of $Na$. Thus,$IE_1(Na) For second ionization energy $(IE_2)$: $Mg^+: [Ne] 3s^1 \rightarrow Mg^{2+} + e^-$ $Na^+: [Ne] 2s^2 2p^6 \rightarrow Na^{2+} + e^-$ Removing an electron from the stable noble gas configuration of $Na^+$ requires much higher energy than from $Mg^+$. Thus,$IE_2(Na) > IE_2(Mg)$. For third ionization energy $(IE_3)$: $Mg^{2+}: [Ne] \rightarrow Mg^{3+} + e^-$ $Al^{2+}: [Ne] 3s^1 \rightarrow Al^{3+} + e^-$ Removing an electron from the stable noble gas configuration of $Mg^{2+}$ requires much higher energy than from $Al^{2+}$. Thus,$IE_3(Mg) > IE_3(Al)$. Statement $B$ is incorrect because $IE_2(Na) > IE_2(Mg)$.

Which of the following statements is incorrect?

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