Both `O_(2) and F_(2)` stabilize high oxidation states but the ability of oxygen to stabilize the higher oxidation state exceeds than that of flrorine. Account for this observation.

Explanation

Compounds in the higher oxidation states are more covalent than in lower oxidation states. Since `O^(2-)` ion has larger ionic size (140 pm) than `F^(-)` ion (136 pm), therefore, any element in a higher oxidation state can polarize `O^(2-)` ion more easily than `F^(-)` ion. As a result, oxides are more covalent than fluorides in the higher oxidation states and hence more stable than fluorides.