The first electron affinity of C, N and O wil | vedclass

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(B) Key Point:$(i)$ Half-filled or fully-filled configurations have low electron affinity (i.e.,positive or less negative electron gain enthalpy).$(ii

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$N < C < O$

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(B) Key Point:$(i)$ Half-filled or fully-filled configurations have low electron affinity (i.e.,positive or less negative electron gain enthalpy).$(ii)$ Smaller the size, generally the more negative the electron gain enthalpy.On moving across a period, the size of atoms decreases due to an increase in nuclear charge.$(i)$ Electronic configurations of the elements are:$C (Z=6) = 1s^{2} 2s^{2} 2p^{2}$$N (Z=7) = 1s^{2} 2s^{2} 2p^{3}$$O (Z=8) = 1s^{2} 2s^{2} 2p^{4}$$(ii)$ Due to the stable half-filled electronic configuration of nitrogen $(2p^{3})$, it has a very low electron affinity (positive electron gain enthalpy value of $30.9 \ kJ/mol$).$(iii)$ As the size of $O$ is smaller than that of $C$, $O$ has a more negative electron gain enthalpy $(-141.1 \ kJ/mol)$ compared to $C$ $(-122.3 \ kJ/mol)$.Thus, the correct order of electron affinity is $N < C < O$.

The first electron affinity of $C, N$ and $O$ will be of the order

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