Openchemistry/Redox

Electrochemistry -
 * 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.
 * 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.