Which of the following statements is incorrec | vedclass

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(B) The electronic configuration of $Mg$ is $[Ne] 3s^2$ and $Al$ is $[Ne] 3s^2 3p^1$. Due to the stable fully-filled $s$-orbital,$Mg$ has a higher fir

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The second ionization enthalpy of $Mg$ is higher than the second ionization enthalpy of $Na$.

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(B) The electronic configuration of $Mg$ is $[Ne] 3s^2$ and $Al$ is $[Ne] 3s^2 3p^1$. Due to the stable fully-filled $s$-orbital,$Mg$ has a higher first ionization enthalpy than $Al$. Thus,statement $A$ is correct.$Na$ has configuration $[Ne] 3s^1$. After removing one electron,$Na^+$ attains a stable noble gas configuration $([Ne])$. Therefore,removing the second electron from $Na^+$ requires a very high amount of energy. Thus,the second ionization enthalpy of $Na$ is much higher than that of $Mg$. Statement $B$ is incorrect.$Na$ $([Ne] 3s^1)$ has a lower first ionization enthalpy than $Mg$ $([Ne] 3s^2)$ due to lower effective nuclear charge and less stable configuration. Statement $C$ is correct.$Mg^{2+}$ has a stable noble gas configuration $([Ne])$,so removing the third electron requires significantly more energy than removing the third electron from $Al^{2+}$ $([Ne] 3s^1)$. Statement $D$ is correct.

Which of the following statements is incorrect?

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