Considering the parameters such as bond dissociation enthalpy, electron gain enthalpy and hydration enthalpy, compare the oxidising power of `F_(2)` and `Cl_(2)`.

Explanation

The electrode potential of `F_(2)( + 2.87V)` is much higher than that of `Cl_(2) (+1.36V)`. Hence, `F_(2)` is a much stronger oxidising agent than `Cl_(2)` . Electrode potential depends on three factors namely, (i) bond dissociation energy (ii) electron gain enthalpy (iii) hydration energy. Electron gain enthalpy of `F_(2)(-333 kJcdotmol^(-1))` is less negative than that of `Cl_(2) (-349kJcdotmol^(-1))` . However, the bond dissociation energy of F -F bond `(158.8kJcdotmol^(-1))` is much lower than that of Cl-Cl bond `(242.6kJcdotmol^(-1))`. Similarly the hydration energy of `F^(-)` ion `(515kJcdotmol^(-1))` is much higher than that of `Cl^(-)` ion `(381kJcdotmo1^(-1))` . The last two factors more than compensate the less negative electron gain enthalpy of `F_(2)` . As a result, electrode potential of `F_(2)` is higher than that of `Cl_(2)` . Hence, `F_(2)` is a much stronger oxidising agent than `Cl_(2)`.