Answer:
The negative electron gain enthalpy
of chlorine \[({{\Delta }_{eg}}H=-349\,kJ\,\text{mo}{{\text{l}}^{-1}})\] is
more than that of fluorine \[({{\Delta }_{eg}}H=-328\,kJ\,\text{mo}{{\text{l}}^{-1}})\].
This means that an atom of chlorine has a greater attraction for the outside
electron than in case of fluorine. Therefore, chlorine can be converted to
chloride ion more readily as compared to fluorine forming fluoride ion.
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