Assertion : Pb^{4+} compounds are stronger ox | vedclass

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(C) The assertion is correct because,due to the 'inert pair effect',the stability of the $+4$ oxidation state decreases down the group $14$ $(C > Si >

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If the Assertion is correct but Reason is incorrect.

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(C) The assertion is correct because,due to the 'inert pair effect',the stability of the $+4$ oxidation state decreases down the group $14$ $(C > Si > Ge > Sn > Pb)$.Consequently,$Pb^{4+}$ is highly unstable and acts as a strong oxidizing agent to reduce itself to the more stable $+2$ state.The reason is incorrect because the higher oxidation states (like $+4$) become less stable,not more stable,for the heavier members of the group due to the 'inert pair effect'.

Assertion : $Pb^{4+}$ compounds are stronger oxidizing agents than $Sn^{4+}$ 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'.

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Assertion : $Pb^{4+}$ compounds are stronger oxidizing agents than $Sn^{4+}$ 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'.