The electron affinity values of elements $A, B, C$ and $D$ are respectively $-135,-60,-200$ and $-348…
The electron affinity values of elements $A, B, C$ and $D$ are respectively $-135,-60,-200$ and $-348 \mathrm{~kJ} \mathrm{~mol} \mathrm{~m}^{-1}$. The outer electronic configuration of element $B$ is
$3 s^2 3 p^5$
$3 s^2 3 p^4$
$3 s^2 3 p^3$
$3 s^2 3 p^2$
Solution
Elements having half or completely-filled orbitals, ie, having stable electronic configuration have very low negative value of electron affinity.
Since, the electron affinity of $B$ is lowest among the given, it has stable electronic configuration, $i e, 3 s^2, 3 p^3$.