The first I.E. of Na, Mg, Al and Si are in th | vedclass

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(B) The first ionization energy $(I.E.)$ of $Na, Mg, Al,$ and $Si$ follows the order: $Na < Al < Mg < Si$.Generally,on moving from left to right in a

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$Na < Al < Mg < Si$

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(B) The first ionization energy $(I.E.)$ of $Na, Mg, Al,$ and $Si$ follows the order: $Na Generally,on moving from left to right in a period,the ionization energy increases due to an increase in effective nuclear charge.However,$Mg$ has a higher $I.E.$ than $Al$ because $Mg$ has a stable,fully-filled $3s^{2}$ valence shell configuration.$Al$ has a valence shell configuration of $3s^{2} 3p^{1}$.It requires less energy to remove a $p$ electron from $Al$ than to remove an $s$ electron from the stable,fully-filled $3s^{2}$ subshell of $Mg$.

The first $I.E.$ of $Na, Mg, Al$ and $Si$ are in the order:

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