The first ionization potentials in electron v | vedclass

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(A) The electronic configuration of Nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which has a stable half-filled $p$-orbital.The electronic configuration of Oxyg

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$14.6, 13.6$

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(A) The electronic configuration of Nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which has a stable half-filled $p$-orbital.The electronic configuration of Oxygen $(O)$ is $1s^2 2s^2 2p^4$.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 potentials in electron volts $(eV)$ of nitrogen and oxygen atoms are respectively given by:

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