Assertion : Pb⁴⁺ compounds are stronger oxidising agents than Sn²⁺ compounds. Reason : The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to ‘inert pair effect’.

4 Pb + compounds are stronger oxidizing agents than 2 Sn + compounds, this is because the bottom elements of group 14 show the inert pair effect, as a result, the oxidation state of the bottom elements reduces by 2. Therefore, the bottom elements show a stable +2 oxidation state. That is why 4 Pb + accepts electron and get reduced to form 2 Pb + ion, and acts as an oxidizing agent. But in case of 2 Sn + the inert pair effect is less applicable, that is why it can donate electrons to form 2 Sn + to get oxidized and acts as a reducing agent. The lower oxidation states (+2) for the group 14