Grade levels: Senior High (10-12)

Shows how the Brønsted-Lowry Theory explains the limitations of Arrhenius’ Theory. Demonstrates the five-step method for writing Brønsted-Lowry equations using the acid-base table from the data booklet.

Reactions involving polyprotic and anions of polyprotic acids can be predicated by adding the proton transfer equations together. Students test and evaluate these predictions through laboratory activities.

Various types of pH curves are generated using a pH probe and a computer interface, comparisons of the different curves are made, and information obtained from the curves discussed.

Demonstrates universal indicators and universal indicator strips. Students are challenged to design an experiment that determines the relative pH of several solutions using only indicators.

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.