The first ionization enthalpies of Nitrogen () and Oxygen () are and respectively. Which of the foll — Periodic Table and Periodicity Chemistry Question
Question
The first ionization enthalpies of Nitrogen ($N$) and Oxygen ($O$) are $14.0 \text{ eV}$ and $13.6 \text{ eV}$ respectively. Which of the following correctly describes their second ionization enthalpies ($IE_2$)?
Answer: B
💡 Solution & Explanation
$IE_1(N) > IE_1(O)$ because N has a stable $2p^3$ half-filled configuration. However, after losing one electron, $O^+$ becomes $2p^3$ (highly stable), while $N^+$ becomes $2p^2$. Thus, $IE_2(O)$ is strictly greater than $IE_2(N)$.
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