`F_(2)` is a stronger oxidising agent than `Cl_(2)`

Explanation

The elcetrode potential of `F_(2) and Cl_(2)` are :
`F_(2) + 2e^(-) rarr 2 F^(-) , E^(@) = + 2.87 V and Cl_(2) + 2e^(-) rarr 2 Cl^(-) , E^(@) = 1.36 V`
Since `E^(@)` for `F_(2)//F^(-)` electrode is higher than that of `Cl_(2)//Cl^(-)` electrode, therefore, `F_(2)` is more easily reduced than `Cl_(2)`. In other words, `F_(2)` is a stronger oxidising agent than `Cl_(2)`. For example, `F_(2)` oxidises `CL^(-)` ions to `Cl_(2)` but `Cl_(2)` does not oxide `F^(-)` ions to `F_(2)`.