JEE Advance - Chemistry (2008 - Paper 1 Offline - No. 13)
Statement 1 : Pb$$^{4+}$$ compounds are stronger oxidising agents than Sn$$^{4+}$$ compounds.
and
Statement 2 : The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to 'inert pair effect'.
Statement 1 is True, Statement 2 is True; Statement 2 is correct explanation for Statement 1.
Statement 1 is True, Statement 2 is True; Statement 2 is NOT correct explanation for Statement 1.
Statement 1 is True, Statement 2 is False.
Statement 1 is False, Statement 2 is True.
Explanation
In p-block elements, inert pair effect is observed, due to which lower oxidation state becomes more stable on going down the group. In 14th group (C, Si, Ge, Sn, Pb) Pb is placed at lower position than Sn, that's why lower oxidation state is more stable for lead (Pb$$^{2+}$$) and Sn$$^{+4}$$ is more stable than Pb$$^{+4}$$. So, Pb$$^{+4}$$ compounds are stronger oxidising agents than Sn$$^{+4}$$ compounds. Lower oxidation for the group 14th elements are more stable for the heavier members.
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