Which of the following has the highest first | vedclass

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(C) The first ionization energy increases across a period and decreases down a group.Comparing the elements $N$,$O$,$P$,and $S$:$N$ $(2s^2 2p^3)$ has

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Nitrogen

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(C) The first ionization energy increases across a period and decreases down a group.Comparing the elements $N$,$O$,$P$,and $S$:$N$ $(2s^2 2p^3)$ has a stable half-filled $p$-orbital configuration,which makes it harder to remove an electron compared to $O$ $(2s^2 2p^4)$.$P$ $(3s^2 3p^3)$ also has a stable half-filled configuration but is in a higher period than $N$,so its ionization energy is lower than that of $N$.Therefore,$N$ has the highest first ionization energy among the given options.

Which of the following has the highest first ionization energy?

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Assertion $(A)$: First ionisation enthalpy of oxygen is less than that of nitrogen.
Reason $(R)$: Atoms with half-filled or completely filled orbitals are less stable.
The correct option among the following is:

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