How is the variability in oxidation states of transition metals different from that of non-transition metals? Illustrate with examples.

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Solution

In transition elements the oxidation states vary by unity (clue to incomplete filling of d-orbitals) e.g., Mn exhibits +2, +3, +4, +5, +6 and +7 all differing by 1.

In non-transition element, this variation is selective, always differing by 2. e.g., S exhibits 2, 4, 6 oxidation states. N exhibits 3, 5 etc.

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Give examples and suggest reasons for the following features of the transition metal chemistry:

(i)The lowest oxide of transition metal is basic, and the highest is amphoteric/acidic.

(ii) A transition metal exhibits the highest oxidation state in oxides and fluorides.

(iii) The highest oxidation state is exhibited in the oxoanions of a metal.

The electron which take part in order to exhibit variable Oxidation states by Transition metals are

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