Increasing order of electron affinity is :-

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(C) The electron affinity $(EA)$ generally increases across a period from left to right and decreases down a group.Comparing the given elements: $N$ (

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$N < Al < O < Cl$

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(C) The electron affinity $(EA)$ generally increases across a period from left to right and decreases down a group.Comparing the given elements: $N$ (Group $15$,Period $2$),$O$ (Group $16$,Period $2$),$Cl$ (Group $17$,Period $3$),and $Al$ (Group $13$,Period $3$).$1$. $Al$ is a metal and has the lowest tendency to gain electrons,so it has the lowest electron affinity.$2$. Among $N$,$O$,and $Cl$: $N$ has a stable half-filled $p$-orbital $(2p^3)$,making its electron affinity very low (even lower than $O$).$3$. $Cl$ has the highest electron affinity among these due to its smaller size and effective nuclear charge compared to $Al$,and it is higher than $O$ because $O$ has high inter-electronic repulsion in its small $2p$ orbital.The correct order is $N < Al < O < Cl$.

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