The incorrect statement among the following i | vedclass

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(C) Electronic configurations: $Mg (Z=12): [Ne] 3s^2$,$Al (Z=13): [Ne] 3s^2 3p^1$. $1$. First ionization potential $(IE_1)$: $Mg$ has a stable fully-f

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The first ionization potential of $Mg$ is greater than the third ionization potential of $Al$.

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(C) Electronic configurations: $Mg (Z=12): [Ne] 3s^2$,$Al (Z=13): [Ne] 3s^2 3p^1$. $1$. First ionization potential $(IE_1)$: $Mg$ has a stable fully-filled $3s$ orbital,so $IE_1(Mg) > IE_1(Al)$. Thus,statement $A$ is correct. $2$. Second ionization potential $(IE_2)$: $Mg^+$ is $[Ne] 3s^1$,$Al^+$ is $[Ne] 3s^2$. Removing an electron from $Al^+$ is harder due to the stable $3s^2$ configuration,so $IE_2(Al) > IE_2(Mg)$. Thus,statement $B$ is correct. $3$. Third ionization potential $(IE_3)$: $Mg^{2+}$ is $[Ne]$,$Al^{2+}$ is $[Ne] 3s^1$. $Mg^{2+}$ has a noble gas configuration,making it extremely difficult to remove the third electron. Thus,$IE_3(Mg) > IE_3(Al)$. Thus,statement $D$ is correct. $4$. Comparing $IE_1(Mg)$ and $IE_3(Al)$: $IE_1(Mg)$ is relatively low (removing from $3s^2$),while $IE_3(Al)$ is very high (removing from $3s^2$ after $3p^1$ and $3s^1$ are gone). Therefore,$IE_3(Al) > IE_1(Mg)$. Statement $C$ is incorrect.

The incorrect statement among the following is:

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