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(A) The electron affinity of an element is the energy released when an electron is added to a neutral gaseous atom. Nitrogen $(N)$ has a stable half-f

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Nitrogen

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(A) The electron affinity of an element is the energy released when an electron is added to a neutral gaseous atom. Nitrogen $(N)$ has a stable half-filled $2p^3$ configuration,making it very difficult to add an electron,resulting in a very low (often negative) electron affinity. Phosphorus $(P)$ also has a half-filled $3p^3$ configuration,but because the $3p$ orbital is larger and further from the nucleus than the $2p$ orbital,the electron-electron repulsion is less significant than in nitrogen. However,comparing the options provided,Nitrogen has the lowest electron affinity due to its small size and high inter-electronic repulsion when adding an electron to the $2p$ subshell. Therefore,the correct answer is Nitrogen.

Which of the following elements will have the lowest electron affinity?

Similar Questions

The amount of energy released for the process $X_{(g)} + e^- \to X^-_{(g)}$ is minimum and maximum respectively for :-
$(a) \ F$
$(b) \ Cl$
$(c) \ N$
$(d) \ B$
Correct answer is :-

Which of the given atoms has the greatest electron affinity?

Which of the following elements have the highest and lowest electron gain enthalpy,respectively?

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