Define and discuss the function of a catalyst in a chemical reaction. Show an example of the conversion of cis-2-butene into trans-2-butene using a halogen atom. Show step by step how the catalyst is involved in speeding up the chemical reaction. Use print outs to aid the demonstration. Also discuss the effect of ozone on the environment. Determine how oxygen is converted to ozone by halogen carbonates. Discuss the harmful effects of UV radiation on skin and eyes caused by decreases in the ozone layer concentration due to chemicals like freon. Show how the freon decreases the ozone layer by catalyzing the decomposition reaction.

Define and discuss activation energy. Relate it to the minimum energy needed to react. Discuss the effects on the rate of reaction when activation energy is low and when it is high. Use example of Nitrogen dioxide combing with carbon monoxide to form nitrogen monoxide and carbon dioxide. View and analyze the reaction rate graph. Define on the graph the transition states, the activation energy and the heat of reaction. Show the difference between an endothemic and exothermic reaction graph.

Discuss the effect on the rate of reaction due to concentration increases of reactants. From graphs show how the rate is directly proportional to the concentration of reactant increases. Use the example of highly concentrated hydrogen peroxide which becomes violently explosive and decomposes at a rate which is too rapid to measure. Discuss why this is due to collision theory. Determine that the rate of decomposition can be shown by the formula rate=k(concentration). Show a graph plot. Analyze a second concentration v rate reaction

Demonstrate and discuss factors which influence the rate of a chemical reaction. Demonstrate effect of a catalyst, the effect of temperature and surface area. use lab demonstrations for each one. Discuss and analyze yesterday's lab of the iodine clock reaction. Present the two formulas used for each reaction and discuss.

Rate of reaction lab. Iodine clock reaction. Lab will demonstrate how the chemical reaction will occur based on the time for a specific iodine-starch reaction to occur and show a positive reaction for iodine.

Define rate in terms of concentration and time. Determine that both are measurable. Use an example of the decomposition of a specific compound to outline how to determine the rate of the reaction. Show that the rate is a negative number due to decomposition. Note that the rate is always expressed as positive, even when decomposition. Discuss that the rate of reaction decreases during the course of a reaction.
Review and analyze homework questions and answers.

Prepare a free entry problem to be solved in class. From the formula to determine free energy, and some given numbers, have Joshua derive the entropy an enthalpy needed to solve th fee energy equation. Once each unknown is solved, substitute into the equation and solve for the free energy.Analyze the results and determine if the reaction will proceed spontaneously. View and discuss a AP video which involves Gibbs free enenergy.

Derive a single thermodynamic function which would allow the determination of a spontaneous reaction. Discuss why and how every substance possess free energy, but it is the changes in free energy, delta G, that are measured in chemical and physical reactions. The Gibbs fee energy formula is presented, viewed on a graph, and determined how each result on the graph determines whether the reaction will occur spontaneously or not. Spontaneous reactions are determined by whether G is less than zero, equal to zero, or greater than zero

Describe how buffers will adjust pH of a solution very slightly. Discuss why a buffered solution is resistant to change in the pH when an acid or base is added. Define a buffer in terms of added acid and conjugate base formation. Introduce a buffer problem: What is the pH of a solution that contains a given molarity of acetic acid and a given molarity of sodium acetate. Work through the problem completely, include the formation of an ICE table and derivation of the pH based on the new pH of the solution

Compare changes in blood pH and water pH when a small amount of acid is added to both. Define why a buffer solution works. List the requirements for a buffer solution. Discuss the acid and conjugate base of the acid. Use acetic acid as an example. Discuss the adjustment of the pH of acetic acid when acetate ion is added to the solution. Explain using common ion effect and LeChatekiers principle