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Highest oxidation states of transition metals are typically observed only in their:
AHydrides
BCarbides
COxides and fluorides
DSulphides
Answer & Solution
Correct answer: C. Oxides and fluorides
Oxygen and fluorine are both small, very electronegative and strong oxidising agents. They can stabilise high formal positive charges on the metal by drawing electron density away. Consequently the highest oxidation states (e.g. $\mathrm{Mn^{+7}}$ in $\mathrm{KMnO_4}$, $\mathrm{Os^{+8}}$ in $\mathrm{OsO_4}$) are observed in oxides and fluorides, not in compounds with less electronegative elements.
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