Question

Statement I $P{b}^{4+}$ compounds are stronger oxidising agents than $S{n}^{2+}$ compounds.
Statement II The higher oxidation states for the group $14$ elements are more stable for the heavier members of the group due to ‘inert pair effect’
(a) Statement I is correct Statement II is correct Statement II is the correct explanation of Statement I
(b) Statement I is correct; Statement II is correct Statement II is not the correct explanation of Statement I
(c) Statement I is correct: Statement II is incorrect
(d) Statement I is incorrect; Statement II is correct

Answer 1

In group $13,14,15$ as we descend down in group, the higher oxidation state becomes less tenable due to inert pair effect. Therefore, lead show $+2$ as stable oxidation state. Hence, $P{b}^{4+}$ act as a strong oxidising agent, itself reduced to $P{b}^{2+}$ very easily. Both statement I and statement II are correct and statement II is a correct explanation of statement I.