Question

PbCl4 is stronger oxidizing agent than SnCl4.Why?

Answer 1

The electronic configuration of group 14 elements is ns2 np2 .So the most common oxidation state exhibited by them should be +4 .+2 oxidation state is more and more common. On  moving down the group the higher oxidation state becomes less stable .This is because of the inert pair effect .Thus Ge ,Sn,and Pb show both the +2 and +4 oxidation states ,the stability of the lower oxidation state decreases on moving down the group .
 
                         C   Si   Ge   Sn  Pb >
(stability of +2 state  increases and +4 state decreases)     
Thus PbCl4 is less stable than SnCl4 .