Compare the oxidizing powers of `F_(2) and Cl_(2)` on the basis of bond dissociation enthalpy, electron gain enthalpy of halogens and hydration enthalpy of halide ions.

Explanation

To compare the oxidizing powers of \( F_2 \) (fluorine) and \( Cl_2 \) (chlorine), we will analyze three key factors: bond dissociation enthalpy, electron gain enthalpy, and hydration enthalpy of halide ions.

### Step 1: Bond Dissociation Enthalpy
- **Definition**: Bond dissociation enthalpy is the energy required to break a bond in a molecule.
- **Comparison**: The bond dissociation enthalpy of \( F_2 \) is lower than that of \( Cl_2 \). This is because the \( F_2 \) molecule experiences greater inter-electronic repulsion due to the smaller size of fluorine atoms, which leads to weaker \( F-F \) bonds compared to \( Cl-Cl \) bonds.
- **Conclusion**: A lower bond dissociation enthalpy in \( F_2 \) means that it can more readily break apart and participate in oxidation reactions compared to \( Cl_2 \).

### Step 2: Electron Gain Enthalpy
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