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I get that group 14 elements show +4 and +2 oxidation states so they can form both ionic and covalent compounds and so they are amphoteric but monoxide means that these elements have to show +2 oxidation state in these oxides and dioxide means that the oxidation state of these elements will be +4.

Monoxides of ge,sn and pb should be ionic because of fajan's rule and dioxides should be covalent then why are they amphoteric? I know that it is because they react with both alkali and acids but what is the reason for such behaviour?

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Consider that elements in Group 1 are far less electronegative than than those amphoteric elements, and in Group 17, they're far more electronegative.

In solution , $\ce{Na+}$ readily donates an electron to tin, for example, form sodium stannate, $\ce{Na2(Sn(OH)6)}$.

On the other side, $\ce{Cl-}$ readily attracts an electron to form tin(II) chloride.

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