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  1. Define oxidation and reduction in terms of transfer of electrons and oxygen.
  2. Define oxidation states of atoms using oxidation numbers.
  3. Define oxidation and reduction in terms of change in oxidation state and use this to identify elements oxidised or reduced in chemical reactions.
  4. Write balanced ion-electron half equations and balance net ionic equations for simple oxidation / reduction reactions.
  5. Be familiar with reactions of common oxidants and reductants in terms of changes in state and colour.

Electrochemistry -

  1. Explain that a cell is two half reactions and when a conducting pathway is provided the electrons will do useful work.
  2. Understand the need for a standard cell.
  3. Use standard reduction potentials to predict thermodynamic spontaneity reduction-oxidation reaction
  4. Predict the electrical potential of a voltaic cell.
  5. Sketch a voltaic (electrochemical) cell and label components
  6. Use standard cell notation to draw a cell diagram.
  7. Identify the positive electrode, the negative electrode and the substance being oxidised and reduced in an electrochemical cell.
  8. Describe how a dry cell and a lead/acid battery produce electrical energy.

Electrochemistry - Electrolysis

  1. 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.
  2. Use activity series of metals to determine the products of electrolysis.
  3. Describe an example of industrial electrolysis using equations and descriptions of electrodes and electrolytes.