Which of the following orders regarding ioniz | vedclass

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(C) The first ionization energy $(IE_1)$ generally increases across a period due to increasing effective nuclear charge. However, nitrogen $(N)$ has a

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$N > O < F$

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(C) The first ionization energy $(IE_1)$ generally increases across a period due to increasing effective nuclear charge. However, nitrogen $(N)$ has a stable half-filled $2p^3$ electronic configuration, which makes it harder to remove an electron compared to oxygen $(O)$.Thus, $IE_1$ of $N > O$.Since fluorine $(F)$ has a smaller atomic size and higher effective nuclear charge than oxygen, $IE_1$ of $F > O$.Combining these, the correct order is $N > O < F$.

Which of the following orders regarding ionization energy is correct?

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