The first ionization energy (in kJ / mol) of | vedclass

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(A) The electronic configurations are:$Na = [Ne] 3s^{1}$$Mg = [Ne] 3s^{2}$$Al = [Ne] 3s^{2} 3p^{1}$$Si = [Ne] 3s^{2} 3p^{2}$Ionization energy generall

Vedclass · Accepted Answer

$496, 737, 577, 786$

Vedclass · Answer

(A) The electronic configurations are:$Na = [Ne] 3s^{1}$$Mg = [Ne] 3s^{2}$$Al = [Ne] 3s^{2} 3p^{1}$$Si = [Ne] 3s^{2} 3p^{2}$Ionization energy generally increases across a period,but $Mg$ has a higher ionization energy than $Al$ due to the stable,fully-filled $3s$ orbital in $Mg$ compared to the $3p$ electron in $Al$.The values are:$Na = 496 \ kJ/mol$$Mg = 737 \ kJ/mol$$Al = 577 \ kJ/mol$$Si = 786 \ kJ/mol$Thus,the correct order is $496, 737, 577, 786$.

The first ionization energy (in $kJ / mol$) of $Na, Mg, Al$ and $Si$ respectively,are

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