REVISION ELECTROCHEMISTRY OXIDATION Oxidation is a loss of electrons The oxidation number increases E.g. Electrodes where oxidation take place will reduce in mass We write the oxidation reaction upside-down from the table Reducing agent ANODE The electrode where oxidation takes place REDUCTION Reduction is a gain of electrons The oxidation number decreases E.g. Electrodes where reduction take place will increase in mass We write the reduction reaction right-way-round from the table Oxidising agent CATHODE The electrode where reduction takes place ELECTROLYTE solution/liquid/dissolved substance that conducts electricity through the movement of ions. TABLE OF STANDARD REDUCTION POTENTIALS STANDARD CONDITIONS CELL POTENTIALS GALVANIC CELL a cell in which chemical energy is converted into electrical energy. A galvanic (voltaic) cell has self-sustaining electrode reactions SPONTATEOUS REACTIONS SALT BRIDGE Its function is to maintain ELECTRICAL neutrality 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 | C - (aq) |C 2 (g) || F 2 (g) | F - (aq) | Pt 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. ELECTROLYTIC CELL ELECTROPLATING REFINING OF COPPER CHLOOR-ALKALI INDUSTRY RECOVERY OF ALUMINIUM