MnO4 2- undergoes disproportionation reaction but MnO4 - does not. Explain.
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Disproportionation is a type of redox reaction in which a species is simultaneously reduced and oxidised forming two different products.
In MnO42-, the oxidation state of manganese is +6. It can disproportionate to form MnO2 and MnO4-.
3MnO42- + 4H+ → MnO2 + 2MnO4- + 2H2O
However, the oxidation state of Mn in MnO4- is +7 which is the maximum possible oxidation state of Mn (atomic number 25, 1s2 2s2 2p6 3s2 3p6 3d54s2) and hence it cannot undergo disproportionation reaction.
In MnO42-, the oxidation state of manganese is +6. It can disproportionate to form MnO2 and MnO4-.
3MnO42- + 4H+ → MnO2 + 2MnO4- + 2H2O
However, the oxidation state of Mn in MnO4- is +7 which is the maximum possible oxidation state of Mn (atomic number 25, 1s2 2s2 2p6 3s2 3p6 3d54s2) and hence it cannot undergo disproportionation reaction.
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Answer:
Since, +2 oxidation state is more stable as compared to +3 oxidation state due to stable half filled electronic configuration, therefore Mn(III) disproportionates to Mn(II).
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