Oxididizing agent -vs- Reducing agent?

Question

MnO2+ 4H3O+ -----> Mn2+ + Cl2 + 6H2O

In the reaction of Manganese (IV) oxide with chloride ion, determine which species is the oxidizing agent and which is the reducing agent.

Please give a short explanation as though you were talking to a 5 year old.

Thanks

Answer 1

Oxidation is a loss of electrons.
Reduction is a gain of electrons.
The oxidizing AGENT will cause something to be oxidized (losing electrons) so the oxidizing AGENT must be reduced (gaining electrons).

MnO2 :the Mn has a valence of plus 4.
Mn+2: the product Mn+2 has gained 2 electrons.
The MnO2 is the oxidizing agent (it has been reduced)

The Cl- ion goes from a valence of -1 to a valence of 0 a loss of an electron. The Cl- ion was oxidized.

Remember: Oxidation is a LOSS of electron and the oxidizing agent will be reduced (a gain of electrons). The oxidizing agent must gain the electrons lost by the substance that has been oxidized .

Answer 2

2Cl- (oxidation number = -1) is oxidized to Cl2 (oxidation number = 0). It's getting less minus, therefore more plus. When oxidation numbers increase, that's oxidation. So MnO2 must be the oxidizing agent.

MnO2 (oxidation number = +4) is getting reduced to Mn2+ (oxidation number = +2). It's getting less plus. When oxidation numbers decrease, that's reduction. So Cl- must be the reducing agent.

Answer 3

Mn goes from +4 to +2 so it is the oxidizing agent
Cl- goes from -1 to 0 si it is the reducing agent

Answer 4

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Answer 5

LEO - loss of electrons is oxidation
GER - Gain of electrons is reduction.
REDCAT - reduction at the cathode.

Answer 6

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