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Question

$$PbCl_{4}$$ is less stable then $$SnCl_{4}$$, $$PbCl_{2}$$ is more stable then $$SnCl_{2}$$. Give reasons.


Solution

The stability of higher oxidation state decreases down the group whereas the stability of lower oxidation state increases down the group.This trend is the consequence of inert pair effect due to which two electron of lead in s-orbital do not participate in chemical bonding.Hence Pb shows +2 oxidation state predominantly.
Whereas no such effect occurs in Sn and hence it prefer to form $$SnCl_4$$  in comparison of $$SnCl_2$$

Chemistry

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