Hg2Cl2 (s) + SnCl4 (aq) → 2HgCl2 (aq) +SnCl2(aq)
. Removal of
electropositive element

how is this a oxidation reaction ? And which element is oxidised ? Please explain this reaction step by step .

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Solution

Oxidation state of Cl is -1(always since it is a halogen unless and until it occurs in special forms)

On reactant side
Oxidation state of Hg is +1
Oxidation state of Sn is +4

On product side
Oxidation state of Hg is +2
Oxidation state of Sn is +2

Since oxidation number of Hg increased it is oxidised and since oxidation number of Sn is reduced it is reduced. This is a redox reaction since both oxidation and reduction occured.

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