Give examples and suggest reasons for the following features of the transition metal chemistry :
(i) The lowest oxide of transition metal is basic, the highest is amphoteric acidic.
(ii) A transition metal exhibits highest oxidation state in oxides and fluorides.
(iii) The highest oxidation state is exhibited in oxoanions of a metal.

Explanation

(i) The lower oxide of transition metal is basic because the metal atom has low oxidation state and still has electrons to donate whereas highest is acidic due to highest oxidation state and not left with free electrons. For example. `overset(II)(MnO)` is basic whereas `overset(VII)(Mn_(2)O_(7))` is acidic.
(ii) A transition metal exhibits higher oxidation states in oxides and fluorides. This is because oxygen and fluorine are highly electronegative elements, small in size (and strongest oxidising agents). For example, osmium shows an oxidation states of +6 in `OsF_(6)` and vanadium shows an oxidation state of +5 in `V_(2)O_(5)`.
(iii) Oxometal anions have highest oxidation state, e.g., Cr in `Cr_(2)O_(7)^(2-)` and `CrO_(4)^(2-)` have an oxidation state of +6 whereas Mn in `MnO_(4)^(-)` has an oxidation state of +7. This is again due to the combination of the metal with oxygen, which is highly electronegative and oxidising element.