04_Oxidation Numbers_Worksheet1 - Name:_ Page | 1...

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Name:__________________________________Lab:_______________________AM/PMPage | 1REDOX REACTIONS & OXIDATION NUMBERSINTRODUCTIONOxidation-Reduction (redox) reactions take place in the world at every moment.Theway batteries produce electricity, the process by which iron rusts, photosynthesis,bleaching your hair—all of these are examples of redox reactions.Redox reactionsrefer to the pair of reactions:Reduction (the gain of electrons by one reactant) andOxidation (the loss of electrons by the other reactant.)These processes always occurtogether—if one substance is being reduced, that means the other species is beingoxidized.And since the electrons lost by one species are being gained by the otherspecies, there is no net gain/loss of electrons overall.As the term “oxidation” might suggest, many redox reactions involve the reaction of asubstance with oxygen, for example, the rusting of iron:4 Fe (s) + 3 O2(g)  2 Fe2O3(s)In this reaction, iron is being oxidized, while oxygen is being reduced.However, IT ISIMPORTANT TO REMEMBER that many redox reactions do not involve oxygen at all,for example, the formation of sodium chloride:2 Na (s) + Cl2(g)  2 NaCl(s)This gives rise to the fundamental definition ofOxidation:Loss of Electrons, andconversely fundamental definition ofReduction:Gain of Electrons.

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