Which element in each of the following pairs has a more negative electron gain enthalpy?
$(i)$ $O$ or $F$ $(ii)$ $F$ or $Cl$

In which of the following processes is the highest energy absorbed?

Fluorine has lower electron affinity than chlorine because of

Among the following configurations,the element which has the highest electron affinity is

The value of $2^{nd}$ electron gain enthalpy for $O$ and $S$ will be (in $kJ/mol$)

Knowing the electron gain enthalpy values for $O \rightarrow O^{-}$ and $O \rightarrow O^{2-}$ as $-141 \ kJ \ mol^{-1}$ and $702 \ kJ \ mol^{-1}$ respectively,how can you account for the formation of a large number of oxides having $O^{2-}$ species and not $O^{-}$?
(Hint: Consider lattice energy factor in the formation of compounds).