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.$1$. Comparing $N$ ($2p^3$,stable h

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$Al < N < O < Cl$

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(C) The electron affinity $(EA)$ generally increases across a period from left to right and decreases down a group.$1$. Comparing $N$ ($2p^3$,stable half-filled configuration) and $O$ $(2p^4)$: $N$ has a very low electron affinity due to its stable half-filled subshell,so $EA(N) $2$. Comparing $O$ and $Cl$: $Cl$ has the highest electron affinity in the periodic table due to its small size and effective nuclear charge,so $EA(O) $3$. Comparing $Al$ and $N$: $Al$ is a metal with a low tendency to gain electrons compared to non-metals,thus $EA(Al) Combining these,the increasing order is $Al < N < O < Cl$.

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The increasing order of electron affinity for the given electronic configurations of elements is:
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