What is the correct order of electron affinity for the given groups?

In which of the following processes is the least energy required?

The electron affinities of halogens are $F = 322, Cl = 349, Br = 324, I = 295 \ kJ \ mol^{-1}$. The higher value for $Cl$ as compared to that of $F$ is due to :-

The formation of the oxide ion $O^{2-}_{(g)}$ requires first an exothermic and then an endothermic step as shown below:
$O_{(g)} + e^{-} \to O^{-}_{(g)}; \Delta H = -142 \, kJ \, mol^{-1}$
$O^{-}_{(g)} + e^{-} \to O^{2-}_{(g)}; \Delta H = 844 \, kJ \, mol^{-1}$
This is because:

The correct order of electron gain enthalpies of $Cl$,$F$,$Te$,and $Po$ is .....

The electron affinity values (in $kJ \ mol^{-1}$) for halogens $X, Y,$ and $Z$ are $-349, -333,$ and $-325$ respectively. Therefore,$X, Y,$ and $Z$ are respectively which of the following?