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(A) The first ionisation potential generally increases across a period from left to right due to an increase in effective nuclear charge. All these el

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$B$

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(A) The first ionisation potential generally increases across a period from left to right due to an increase in effective nuclear charge. All these elements belong to the $2^{nd}$ period. The order of first ionisation potential is $B $N$ has a higher value than $O$ due to its stable half-filled $2p^3$ electronic configuration. Therefore,$B$ (Boron) has the lowest first ionisation potential among the given elements.

Which of the following has the lowest first ionisation potential?

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