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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 $(C)$.

List-$I$ (Electronic configuration of neutral atom where $n=2$)	List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$	$I. 2080$
$B. ns^2np^1$	$II. 899$
$C. ns^2np^3$	$III. 800$
$D. ns^2np^6$	$IV. 1402$

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

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Match List-$I$ with List-$II$:
List-$I$ (Electronic configuration of neutral atom where $n=2$) List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$ $I. 2080$
$B. ns^2np^1$ $II. 899$
$C. ns^2np^3$ $III. 800$
$D. ns^2np^6$ $IV. 1402$

Which of the following elements are at the peaks of the ionization energy trend?

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