Which of the following is most stable ?

IV A group elementsCommon oxidation state is : "+4"C shows :- +4 -4Si:- +4 [Stable] Ge,Sn:+2,+4Stable Pb: +2Stable,+4→ 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 involvement of only np electroni.e., ns2 np(2) ⇒ +2Higher oxidation state stability decreases from top to bottom  Lower oxidation state stability increases from top to bottomGe+2 < Sn+2 < Pb+2 Stability order