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(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which has a half-filled $p$-orbital. This configuration provides extra stabilit

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The half-filled $p$-orbitals possess extra stability

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(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which has a half-filled $p$-orbital. This configuration provides extra stability to the nitrogen atom. In contrast,oxygen $(O)$ has the configuration $1s^2 2s^2 2p^4$. Removing an electron from the stable half-filled $p$-orbital of nitrogen requires more energy than removing an electron from the $p$-orbital of oxygen. Therefore,the correct option is $(C)$.

The ionization energy of nitrogen is larger than that of oxygen because of

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