2. Electrolytic cell: Converts electrical energy to chemical energy. Electrolysis – Electrolytic Cell Copper chloride CuCl 2 + - Cu 2+ Cl - Cu 2+ (aq) + 2e -  Cu (s) REDUCTION CATHODE 2Cl - (aq)  Cl 2(g) + 2e - OXIDATION Anode

3. Purifying Copper Identify the anode cathode etc - + Cu 2+ + 2e -  Cu Cu 2+ Cu  Cu 2+ + 2e - Cu 2+ Impure copper (metals) dissolving Anode (oxidation) Pure copper forming Cathode (Reduction) sludge -+ electrons

4. Extraction of Aluminium Al 2 O 3 Al 3+ O 2- Al 3+ + 3e -  Al (l) 2O 2-  O 2 (g) +2e - + + + - - +

5. Cathode ( ) Voltaic (Galvanic) vs Electrolytic Copper chloride CuCl 2 + - Cu 2+ Cl - Cu 2+ (aq) + 2e -  Cu (s) REDUCTION CATHODE (-) 2Cl - (aq)  Cl 2(g) + 2e - OXIDATION Anode (+) __________ Zn ____ Cu V KNO 3(aq) + > Zn  Zn 2+ + 2e - CuSO 4 ZnSO 4 Salt bridge Anode (-) Zn + Cu 2+  Zn 2+ + Cu oxidation reduction REDUCING AGENT OXIDISING AGENT e- _ Cu 2+ + 2e -  Cu Chemical Energy  Electrical EnergyElectrical Energy  Chemical Energy + e-