Question

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

Answer 1

here we use the concept of that the transition metals have vacant d orbital thus they can exchange the electrons i.e. they can expand their oxidation states variaibly thus they show the variable oxidation state.
however in non transition metals they cannot expand their octet by transferring electrons to d orbital.
Eg. is the oxidation state of mn2+,mn5+ etc

Answer 2

Answer:

The transition metals show a number of variable oxidation states due to the participation of (n – 1) d electrons in addition to ns electrons in the bond formation. They therefore, exhibit a large number of variable oxidation states. On the other hand, the non-transition metals generally belonging to s-block do not show variable oxidation states because by the loss of valence s-electrons, they acquire the configuration of the nearest noble gas elements.

In the p-block the lower oxidation states are favoured by the heavier members (due to inert pair effect), the opposite is true in the groups of d-block. For example, in group 6, Mo(VI) and W(VI) are found to be more stable than Cr(VI). Thus Cr(VI) in the form of dichromate in acidic medium is a strong oxidising agent, whereas MoO3 and WO3 are not.

Explanation: