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Explain why the highest oxidation state for group 14 (IVA), +4, is exclusively observed for carbon...

Explain why the highest oxidation state for group 14 (IVA), +4, is exclusively observed for carbon but hard to stabilize for lead, which has +2 as its most stable oxidation state. When formulating your answer, also consider what oxidation states are typically exhibited by silicon, germanium and tin.

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Lead which is 6th period element with outer shell configuration of 6s2 6p2. Here removing two electrons from p shell results in Pb2+ and its more stable than Pb4+ (which we get by removing 4 valence electrons). This is because of inert pair effect. The d shells in Lead are weak in shielding the nuclear charge and thus nucleus has hold the 6s electrons tighter and thus removing s electron requires more energy. Hence lead exist mostly as Pb2+ which is more stable than Pb4+. For lower period elements like Carbon there are no "d" shell electrons which have weak shielding affect. Hence +4 is easily observed in carbon.

Then tendancy for +2 state increases as atom size increases i.e its order of C2+ < Si2+ < Ge2+ < Pb2+

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