The correct electron affinity order is (EA = | vedclass

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(B) Electron affinity is the energy released when an electron is added to a gaseous species. It is directly related to the stability of the species fo

Vedclass · Accepted Answer

$O^{+} > N^{+} > NO^{+}$

Vedclass · Answer

(B) Electron affinity is the energy released when an electron is added to a gaseous species. It is directly related to the stability of the species formed after electron gain.$N^{+} (1s^{2} 2s^{2} 2p^{2})$: Adding an electron gives $N$ $(1s^{2} 2s^{2} 2p^{3})$,which has a stable half-filled $p$-orbital configuration.$O^{+} (1s^{2} 2s^{2} 2p^{3})$: Adding an electron gives $O$ $(1s^{2} 2s^{2} 2p^{4})$,which is less stable than the half-filled state.$NO^{+}$: This is an isoelectronic species with $N_{2}$ ($14$ electrons). Adding an electron to $NO^{+}$ leads to $NO$ ($15$ electrons),where the electron enters the antibonding $\pi^{*}$ orbital,which is less favorable.Comparing the effective nuclear charge $(Z_{eff})$,$O^{+}$ has a higher $Z_{eff}$ than $N^{+}$,but the stability of the resulting neutral atom is the dominant factor here. The correct order of electron affinity is $O^{+} > N^{+} > NO^{+}$.

The correct electron affinity order is $(EA = -\Delta H_{EG})$

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