Fund. K - Redox reactions

Fund. K - Redox reactions - Fundamentals: K Redox reactions...

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Fundamentals: K Redox reactions LEO GER Oxidation – loss of electrons Recognized by increased charge on the species Increase in oxidation number Reduction – gain of electrons Recognized by the decreased charge on the species Decrease in oxidation number Matched set: You don't have an oxidation reaction w/o a reduction reaction happening at the same time Oxidation numbers 1) Oxidation number of monatomic ions is the charge on the ion Ca 2+ = +2 I - = -1 2) Oxidation number of an element in elemental form* is 0 (*not combine with another element) Cl 2 (g) = 0 Ag (s) = 0 3) Oxidation number of atoms in a compound Like it is an ionic compound! The periodic table tells you! Group 1 = +1 Group 2 = +2 Group 7 = -1 (unless it is with oxygen or another halide, F = -1!) 4) Hydrogen with metal = -1 Hydrogen with non-metals = +1 HBr – hydrogen = +1 5) Oxygen = -2 except with F (Oxygen = -1) Perozides (O 2 2- ) O = -1 Superoxides (O 2 - ) O = -1/2? Oxidizing and reducing agents Oxidizing agents Reducing agents Decrease in ON Increase in ON Are being reduced Are being oxidized
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Al (s) + O 2 (g) → Al 2 O 3 0 0 +3 -2 Al – lost 3 e - (went from 0 to +3) It is oxidized It is the reducing agent O – gained 2 e - (went from 0 to -2) It is reduced It is the oxidizing agent Balancing! Not only do the atoms need to be balanced, but the charges too! Can’t gain or loose e - in a reaction 4 Al (s) + 3 O 2 (g) → 2 Al 2 O 3 total of 12 e - lost 0 0 +3 -2 total of 12 e - gained = balanced!!! This equation looks blananced, but we need to check to see if the number of e
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This note was uploaded on 04/24/2008 for the course CHEM 6A taught by Professor Pomeroy during the Winter '08 term at UCSD.

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Fund. K - Redox reactions - Fundamentals: K Redox reactions...

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