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Electrochemistry (Oxidation/Reduction)

Electrochemistry (Oxidation/Reduction). CHEM 2124 – General Chemistry II Alfred State College Professor Bensley. Learning Objectives. Define oxidation-reduction reaction. Learn the oxidation number rules and assign oxidation numbers.

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Electrochemistry (Oxidation/Reduction)

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  1. Electrochemistry (Oxidation/Reduction) CHEM 2124 – General Chemistry II Alfred State College Professor Bensley

  2. Learning Objectives • Define oxidation-reduction reaction. • Learn the oxidation number rules and assign oxidation numbers. • Write the half-reactions of an oxidation-reduction reaction. • Determine the species undergoing oxidation and reduction. • Describe and construct basic galvanic cells • Calculate cell potential for basic galvanic cells

  3. Oxidation and Reduction • General Features • Oxidation Numbers Assign oxidation numbers to Carbon in each of the following compounds: 1. Carbon Monoxide 2. Carbon Dioxide 3. C6H12O6 (Glucose)4. Sodium Bicarbonate For each of the following chemical reactions, determine whether or not the reaction is an example of an oxidation-reduction reaction. LiOH + HCN  H2O + LiCN LiCl + AgNO3 AgCl + LiNO3 P4 (s) + 5O2 (g)  P4O10 (s) CuCl2 (aq) + Al (s)  AlCl3 (aq) + Cu (s)

  4. Oxidation and Reduction • Half Reactions What happens when copper wire is placed in a silver nitrate solution?

  5. For each of the following Redox reactions, write the individual half-reactions. • Fe (s) + CuSO4 (aq)  Cu (s) + FeSO4 (aq) • Co (s) + Cl2 (g)  CoCl2 (g) In each of the following reactions, identify the oxidizing agent and the reducing agent. • Co (s) + Cl2 (g)  CoCl2 (g) • 2Al (s) + 3F2 (g)  2AlF3 (s) • PbS (s) + 4H2O2 (aq)  PbSO4 (aq) + 4H2O (l)

  6. Oxidation and Reduction IV. Examples of Oxidation–Reduction Reactions • Combination Reactions • Decomposition Reactions • Displacement Reactions • Combustion Reactions

  7. Oxidation and Reduction V. Galvanic or voltaic cells

  8. Anode Zn (s)  Zn 2+ (aq) + 2e- Cathode Cu 2+ (aq) + 2e- Cu (s)

  9. Oxidation and Reduction • Galvanic Cell Terminology • Half cells • Anode • Cathode • Salt Bridge • Cell Notation • Cell Potential E0 (cell)= E0 (red) – E0 (ox)

  10. Order the following oxidizing agents from weakest to strongest. Cu2+ (aq), Fe2+ (aq), Fe3+ (aq) Order the following reducing agents from weakest to strongest. H2 (g), Al (s), Cu (s)

  11. Example • Sketch the cell formed by Cd in Cd(NO3)2 and Ag in AgNO3. • Write the half-reactions, label the anode, cathode, salt bridge, and direction of electron flow. • Write the cell notation. • Calculate the overall cell potential for this cell.

  12. VII. Biological Applications Oxidation and Reduction • Respiration • Oxidation of glucose to CO2 • Reduction of O2 to H2O C6H12O6 (s) + 6O2 (g)  6CO2 (g) + 6H2O (g) • Photosynthesis • Oxidation of H2O to O2 • Reduction of CO2 to glucose • 6CO2 (g) + 6H2O (g) + light  C6H12O6 + 6O2 (g)

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