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(A) The electronic configurations correspond to the following elements:$I$: $1s^2 2s^2 2p^6 3s^2 3p^5$ is Chlorine $(Cl)$.$II$: $1s^2 2s^2 2p^3$ is Ni

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$II < IV < III < I$

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(A) The electronic configurations correspond to the following elements:$I$: $1s^2 2s^2 2p^6 3s^2 3p^5$ is Chlorine $(Cl)$.$II$: $1s^2 2s^2 2p^3$ is Nitrogen $(N)$.$III$: $1s^2 2s^2 2p^5$ is Fluorine $(F)$.$IV$: $1s^2 2s^2 2p^6 3s^2 3p^1$ is Aluminium $(Al)$.Electron affinity generally increases across a period and decreases down a group.However,Nitrogen $(N)$ has a half-filled $p$-orbital $(2p^3)$,making it very stable,resulting in a very low (near zero or negative) electron affinity.Fluorine $(F)$ has a smaller size than Chlorine $(Cl)$,leading to inter-electronic repulsions,which makes the electron affinity of $Cl$ higher than $F$.Aluminium $(Al)$ is a metal with a low electron affinity.Thus,the order is $N < Al < F < Cl$,which corresponds to $II < IV < III < I$.

The increasing order of electron affinity for the given electronic configurations of elements is:
$I$. $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^5$ $(Cl)$
$II$. $1s^2 \ 2s^2 \ 2p^3$ $(N)$
$III$. $1s^2 \ 2s^2 \ 2p^5$ $(F)$
$IV$. $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1$ $(Al)$

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The increasing order of electron affinity for the given electronic configurations of elements is:$I$. $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^5$ $(Cl)$$II$. $1s^2 \ 2s^2 \ 2p^3$ $(N)$$III$. $1s^2 \ 2s^2 \ 2p^5$ $(F)$$IV$. $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1$ $(Al)$