The first ionization potential values (in eV) | vedclass

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Question

(A) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which is a stable half-filled $p$-orbital configuration.Oxygen $(O)$ has the co

Vedclass · Accepted Answer

$14.6, 13.6$

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(A) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which is a stable half-filled $p$-orbital configuration.Oxygen $(O)$ has the configuration $1s^2 2s^2 2p^4$.Due to the extra stability of the half-filled $2p$ subshell in nitrogen,it requires more energy to remove an electron compared to oxygen.Therefore,the first ionization potential of nitrogen $(14.6 \ eV)$ is higher than that of oxygen $(13.6 \ eV)$.

The first ionization potential values (in $eV$) for nitrogen and oxygen atoms are respectively:

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