Which of the following statements is not correct ?

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The tendency to exhibit + 2 oxidation state for Ge, Sn and Pb is in the order Ge < Sn < Pb

Carbon and silicon mostly exhibit + 4 oxidation state in their compounds

Lead in + 4 oxidation state acts as an oxidising agent

Tin in + 4 oxidation state acts as a good reducing agent.

answer is D.

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Detailed Solution

IV A group elementsCommon oxidation state is : "+4"C shows :- +4 -4Si:- +4 [Stable]→ For Ge,Sn +4 is stable oxidation state hence in +2 oxidation state they acts as reducing agents→ Where as for Pb +2 oxidation state is state [due to inert pair effect] hence in +4 oxidation state Pb acts as oxidising agent→ Higher oxidation state is due to involvement of ns and np electroni.e., Lower oxidation state is due to involvent of only np electroni.e., ns2 np(2) ⇒ +2Higher oxidation stable stability dcecreases from top to bottomLower oxidation state stability increases from top to bottomGe+2 < Sn+2 < Pb+2 Stability order

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