why pbcl4 act as strong oxidizing agent
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As we go down in a group 14 elements of periodic table , we observe that +4 oxidation state decreases while that of +2 oxidation state increases due to inert pair effect. so, the outermost s-orbital electrons shows reluctance to take part in reaction. This leads to greater stability of +2 oxidation state in group 14 elements.
Instead of losing 4 electrons [ 2 electrons from S and 2 from P orbitals ], they tend to loose the p orbitals electrons . hence Pb+4 can easily gain 2 electrons to form more stable Pb+2 ions.
Pb (lead) show +2 oxidation state and easily gets reduced and therefore oxides others.
Hence PbCl4 is stronger oxidizing agent.
Instead of losing 4 electrons [ 2 electrons from S and 2 from P orbitals ], they tend to loose the p orbitals electrons . hence Pb+4 can easily gain 2 electrons to form more stable Pb+2 ions.
Pb (lead) show +2 oxidation state and easily gets reduced and therefore oxides others.
Hence PbCl4 is stronger oxidizing agent.
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