Languages: English

Explains how metals are obtained from molten ores and presents a historical perspective of Sir Humphrey Davy’s work. Explores similar technology used today in the Hall process, the Downs cell and the formation of magnesium metal.

Our reliance on fossil fuels is the basis for a risk/benefit analysis of energy sources. The advantages and disadvantages of fossil fuels are discussed and several alternate energy sources reviewed.

Discusses Michael Faraday’s contributions to science. Explains electrical units and the Faraday, and the relationship between current, time and mol of electrons. Sample problems demonstrate the stoichiometric connection to electrolysis.

Provides a historical perspective of oxidation and reduction using examples of reactions. Introduces the terms oxidation and reduction, and oxidizing agent and reducing agent. Examples of half-reactions and real-life applications reinforce the terms.

Compares the costs of recycling to that of producing aluminum and iron from their ores. Students look at the economic and environmental advantages and disadvantages associated with each process.

Explains the terms spontaneous and non-spontaneous, shows the strength of oxidizing and reducing agents, and develops a reduction half-reaction table. Explains the spontaneity rule, performs experiments to test it and records the results on a data table.

Explains several reversible reactions and a juggler demonstrates the differences between steady state, open and closed systems. Experiments using evaporation show the difference between an open and closed system. Defines equilibrium.

Performs experiments to: identify the chemical responsible; compare relative strengths on non-metallic oxidizing agents; develop a reduction half-reaction table; and combine this table with the one developed in the previous program.

Demonstrates how change in temperature can favour either a forward or reverse rate of a reaction. On a molecular level, the hydrogen iodine, hydrogen iodide equilibrium shows what happens from the start of a reaction until the system reaches equilibrium.