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Galvanic and Electrolytic Cells

Galvanic and Electrolytic Cells. SCH 4C1. Review. Zn (s) + Cu 2+ ( aq )  Cu (s) + Zn 2+ ( aq ) Zinc is oxidized, Copper is reduced The Cu 2 + removes two electrons from the Zn atoms Zn (s)  Zn 2+ ( aq ) + 2e - Cu 2+ ( aq ) + 2e -  Cu (s). Galvanic Cell (copy).

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Galvanic and Electrolytic Cells

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  1. Galvanic and Electrolytic Cells SCH 4C1

  2. Review • Zn (s) + Cu2+ (aq)  Cu (s) + Zn2+(aq) • Zinc is oxidized, Copper is reduced • The Cu2+ removes two electrons from the Zn atoms • Zn (s)  Zn2+ (aq) + 2e- • Cu2+ (aq) + 2e-  Cu (s)

  3. Galvanic Cell (copy) • Converts chemical energy to electrical energy from a REDOX reaction • A.K.A. a battery!

  4. Cu2+(aq) + 2e- Cu(s) Zn (s) Zn2+(aq) + 2e-

  5. How does it work? (copy) • Electrons lost by Zn (s) travel through the wire to reach the Cu2+ ions, to turn them into Cu (s) • The redox reactions occur in separate half-cells and are spontaneous

  6. REMINDER • Electricity is the flow of electrons • Conductors allow the flow of electrons to occur • Insulators do not!

  7. Parts (copy) • Electrodes – solid conductors in each ½ cell • 1. Anode – oxidation occurs • 2. Cathode – reduction occurs • Electrolyte Solution – contains ions of each metal electrode • Salt Bridge – contains conc. salt solution; prevents charge build-up in ½ cells

  8. Think RedCat

  9. Let’s Put it Together!

  10. Electrolytic Cells (copy) • Converts electrical energy to chemical energy from a REDOX rxn • Non-spontaneous (energy is needed) • E.g. Electrolysis of NaCl(s) to get Na(s) and Cl2 (g)

  11. Molten NaCl

  12. HW • Read pg. 398 (about salt bridges) • pg. 397 # a – hand in • pg. 400 # 7 – hand in • Review/Copy Table 1 from pg. 431

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