The first ionization enthalpy of Al is lower | vedclass

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(D) The electronic configuration of $Mg$ $(Z=12)$ is $[Ne] 3s^2$,which is a stable,completely filled orbital configuration. The electronic configurati

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$Mg$ has a completely filled $3s$ orbital.

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(D) The electronic configuration of $Mg$ $(Z=12)$ is $[Ne] 3s^2$,which is a stable,completely filled orbital configuration. The electronic configuration of $Al$ $(Z=13)$ is $[Ne] 3s^2 3p^1$. Removing an electron from $Mg$ requires breaking the stable,fully filled $3s$ subshell,which requires more energy. In $Al$,the electron is removed from the $3p$ orbital,which is easier as it is shielded by the $3s$ electrons and is less stable than the fully filled $3s$ subshell. Therefore,the first ionization enthalpy of $Al$ is lower than that of $Mg$ due to the stable electronic configuration of $Mg$.

Element	$IE_1$	$IE_2$	$IE_3$	Code	Element
$1$	$2080$	$3963$	$6130$	$(a)$	$H$
$2$	$520$	$7297$	$11810$	$(b)$	$Li$
$3$	$900$	$1758$	$14810$	$(c)$	$Be$
$4$	$800$	$2428$	$3660$	$(d)$	$B$
-	-	-	-	$(e)$	$Ne$

The first ionization enthalpy of $Al$ is lower than that of $Mg$ because .......................

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