The correct values of ionization enthalpies ( | vedclass

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(D) The first ionization enthalpy values for the given elements are: $Si = 786 \ kJ \ mol^{-1}$,$P = 1012 \ kJ \ mol^{-1}$,$S = 999 \ kJ \ mol^{-1}$,a

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$786, 999, 1012, 1256$

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(D) The first ionization enthalpy values for the given elements are: $Si = 786 \ kJ \ mol^{-1}$,$P = 1012 \ kJ \ mol^{-1}$,$S = 999 \ kJ \ mol^{-1}$,and $Cl = 1256 \ kJ \ mol^{-1}$.Across a period,ionization enthalpy generally increases due to increasing effective nuclear charge and decreasing atomic size.However,$P$ $(3s^2 3p^3)$ has a stable half-filled $p$-orbital configuration,which makes its ionization enthalpy higher than that of $S$ $(3s^2 3p^4)$.Therefore,the correct order is $Si < S < P < Cl$,and the corresponding values are $786, 999, 1012, 1256$.

The correct values of ionization enthalpies (in $kJ \ mol^{-1}$) of $Si, P, Cl$ and $S$ respectively are

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