The first ionisation potential of Na,Mg,Al an | vedclass

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Question

(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionization enthalpy generally increases.For $Al$ $(3s^{2} 3p

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$Na  Al < Si$

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(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionization enthalpy generally increases.For $Al$ $(3s^{2} 3p^{1})$,the electron is removed from a partially filled $3p$ orbital.For $Mg$ $(3s^{2})$,the electron is removed from a stable,fully filled $3s$ orbital.Removal of an electron from a stable,fully filled orbital requires more energy than removal from a partially filled orbital.Thus,the ionization enthalpy of $Mg$ is greater than that of $Al$.The correct order of first ionization enthalpies is: $Na  Al < Si$.

The first ionisation potential of $Na$,$Mg$,$Al$ and $Si$ are in the order :-

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