`PbCl_4` is less stable than `SnCl_4` while `PbCl_2` is more stable than `SnCl_2`. Justify or contradict.

Explanation

In case of group-14 elements the number of d-or f-electrons increases down the group from Ge to Pb. Hence, the inert pair effect becomes gradually more prominent. As a result, stability of +4 oxidation state decreases and +2 oxidation state increases down the group. Consequently, Pb is more stable in +2 state whereas Sn is more stable in +4 state. Therefore, `PbCl_4` is less stable than `SnCl_4` while `PbCl_2` is more stable than `SnCl_2`.