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| 1. |
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. |
| Answer» Solution :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. | |