- Define oxidation and reduction in terms of transfer of electrons and oxygen.
- Define oxidation states of atoms using oxidation numbers.
- Define oxidation and reduction in terms of change in oxidation state and use this to identify elements oxidised or reduced in chemical reactions.
- Write balanced ion-electron half equations and balance net ionic equations for simple oxidation / reduction reactions.
- Be familiar with reactions of common oxidants and reductants in terms of changes in state and colour.
- Explain that a cell is two half reactions and when a conducting pathway is provided the electrons will do useful work.
- Understand the need for a standard cell.
- Use standard reduction potentials to predict thermodynamic spontaneity reduction-oxidation reaction
- Predict the electrical potential of a voltaic cell.
- Sketch a voltaic (electrochemical) cell and label components
- Use standard cell notation to draw a cell diagram.
- Identify the positive electrode, the negative electrode and the substance being oxidised and reduced in an electrochemical cell.
- Describe how a dry cell and a lead/acid battery produce electrical energy.
Electrochemistry - Electrolysis
- Draw a labelled diagram of an electrochemical cell and write half equations for oxidation at the anode and reduction at the cathode for each molten salt and aqueous salt.
- Use activity series of metals to determine the products of electrolysis.
- Describe an example of industrial electrolysis using equations and descriptions of electrodes and electrolytes.