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Oxidation-Reduction Reactions

Oxidation-Reduction Reactions. Oxidation-reduction (redox) reactions are those in which one or more electrons are transferred. Remember that the sum of the oxidation states in a neutral compound must equal zero and must be equal to the overall charge in an ionic compound .

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Oxidation-Reduction Reactions

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  1. Oxidation-Reduction Reactions Oxidation-reduction (redox) reactions are those in which one or more electrons are transferred. Remember that the sum of the oxidation states in a neutral compound mustequal zero and must be equal to the overall charge in an ionic compound. Assign oxidation states to each of the atoms in the following compounds: a. FeF2 b. H2O c. KMnO4 d. C2H6 e. ICl5 f. SO42- K = +1, Mn = +7, O = -2 Fe = +2, F = -1 H = +1, O = -2 1(+2) 2(-1) 2(+1) 1(-2) 1(+1) +7 4(-2) I = +5, Cl = -1 C = -3, H = +1 S = +6, O = -2 2(-3) 6(+1) +5 5(-1) +6 4(-2) +2 Assign oxidation states to each atom in the equation. Fe2O3 + 2 Al  Al2O3 + 2 Fe Fe gains electrons. It has been REDUCED +3 -2 0 +3 -2 0 Al lost electrons. It has been OXIDIZED

  2. Remember LEO GER: LOSE ELECTRONS OXIDATION GAIN ELECTRONS REDUCTION Something that is reduced is called an oxidizing agent. Something that is oxidized is called a reducing agent. For each reaction, identify that atoms that undergo reduction, or oxidation. • 2 H2(g) + O2(g) 2 H2O (g) • Zn (s) + Cu2+(aq) Zn2+(aq) + Cu (s) • 2 AgCl(s) + H2(g) 2 H+(aq) + 2 Ag (s) + 2 Cl-(aq) d. 2 MnO4-(aq) + 16 H+(aq) + 5 C2O42-(aq) 2 Mn2+(aq) + 10 CO2(g) + 8 H2O(l) oxidized: hydrogen (0 to +1) reduced: oxygen (0 to -2) 0 0 +1 -2 oxidized: zinc (0 to +2) reduced: copper (+2 to 0) 0 +2 +2 0 +1 -1 0 +1 0 -1 oxidized: hydrogen (0 to +1) reduced: silver (+1 to 0) +7 -2 +1 +3 -2 +2 +4 -2 +1 -2 oxidized: carbon (+3 to +4) reduced: manganese (+7 to +2)

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