Pb^4+ acts as an oxidising agent but Sn^2+ acts as a reducing agent.
Explain the following :
Pb4+ acts as an oxidising agent but Sn2+ acts as a reducing agent.
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Inert pair effect is less prominent in Sn than in Pb. Therefore, +2 oxidation of Sn is less stable than its +4 oxidation state. In other words, Sn2+ can easily lose two electrons to form Sn4+ and hence Sn2+ acts as a reducing agent.
Sn2+ →Sn4+ + 2e
In contrast, the inert pair effect is’ more prominent in Pb than in Sn. Therefore, +2 oxidation state of Pb is more stable than its +4 oxidation state. In other words, Pb4+ can easily lose two electrons to form Pb2+ and hence Pb4+ acts as an oxidising agent.
Pb4+ + 2e- → -Pb2+
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