why Transition elements show highest oxidation state in their oxides thanfluorides?

The highest oxidation states of transition metals are exhibited in their oxides as well as fluorides due to small size and high electronegativity of oxygen and fluorine. But in some cases, higher oxidation states are observed for oxides than fluorides.Example: Mn2O7 exists but MnF7 is unknown.This is due steric hindrance which is due to the difficulty in fitting of seven fluoride ions around a single manganese centre.

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This happens because oxygen has the property of creating a ppi ppi double bond which doesn't happen in Fluorine because it just wants only one electron to complete its valence orbital and can only form sigma bonds with less covalent character

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