The enthalpy changes for the addition of an electron to gaseous fluorine and chlorine atoms are shown in the table below.

Element	Process	\(\Delta H^\circ\text{ (kJ/mol)}\)
\(\text{F}\)	\(\text{F}(g) + e^- \rightarrow \text{F}^-(g)\)	\(-328\)
\(\text{Cl}\)	\(\text{Cl}(g) + e^- \rightarrow \text{Cl}^-(g)\)	\(-349\)

Which of the following statements best explains why the addition of an electron to \(\text{F}(g)\) releases less energy than the addition of an electron to \(\text{Cl}(g)\)?