Arrange N,S,O and F in order of decreasing el | vedclass

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(A) Electron gain enthalpy generally becomes more negative (increases in magnitude) as we move from left to right across a period due to decreasing at

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$F > S > O > N$

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(A) Electron gain enthalpy generally becomes more negative (increases in magnitude) as we move from left to right across a period due to decreasing atomic size. However,there are exceptions due to electron-electron repulsions in smaller atoms. For $F$ (Fluorine),it has the highest electron gain enthalpy among these. For $O$ (Oxygen),the incoming electron experiences significant repulsion due to its small size,making its electron gain enthalpy less negative than that of $S$ (Sulphur). $N$ (Nitrogen) has a half-filled $2p$ subshell $(2p^3)$,making it very stable and resulting in a very low (near zero) electron gain enthalpy. Thus,the correct order of decreasing electron gain enthalpy is $F > S > O > N$.

Arrange $N$,$S$,$O$ and $F$ in order of decreasing electron gain enthalpy.

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