1. REVISION ELECTROCHEMISTRY

2. OXIDATION is a loss of electrons An increase in oxidation number REDUCTION is a gain of electrons A decrease in oxidation number CATHODE The electrode where reduction takes place ANODE The electrode where oxidation takes place

3. ELECTROLYTE solution/liquid/dissolved substance that conducts electricity through the movement of ions.

4. TABLE OF STANDARD REDUCTION POTENTIALS

5. STANDARD CONDITIONS

7. GALVANIC CELL a cell in which chemical energy is converted into electrical energy. A galvanic (voltaic) cell has self-sustaining electrode reactions

8. SPONTATEOUS REACTIONS

9. CELL POTENTIALS

10. CELL NOTATION The H 2 |H + half-cell is treated just like any other half-cell.. Cell terminals (electrodes) are written on the outside of the cell notation. Active electrodes reducing agent | oxidised species || oxidising agent | reduced species Inert electrodes (usually Pt or C): Pt | reducing agent | oxidised species || oxidising agent | reduced species | Pt Example: Pt | Cℓ - (aq) |Cℓ 2 (g) || F 2 (g) | F - (aq) | Pt

11. SALT BRIDGE Its function is to maintain ELECTRICAL neutrality

16. ELECTROLYTIC CELL a cell in which electrical energy is converted into chemical energy. ELECTROLYSIS The chemical process in which electrical energy is converted to chemical energy OR the use of electrical energy to produce a chemical change.

17. ELECTROLYTIC CELL

18. ELECTROPLATING

20. REFINING OF COPPER

22. CHLOOR-ALKALI INDUSTRIE

23. RECOVERY OF ALUMINIUM