2. Explain the collision theory including the two factors for an effective collision (i.e. correct orientation and energy (activation energy, Eac or greater).
3. Using the collision theory and the Kinetic Molecular Theory, explain reaction mechanism including determining rate limiting/determining steps, which species is a catalyst/intermediate, and the relationship between the number of reactant particles and the rate of the reaction. (i.e. making products).
4. Using the Kinetic Energy graph, explain the factors for increasing/decreasing the rate of reaction including temperature, amount of reactant particles near each other per volume (including surface area that is just changing concentration of solid), and addition of catalyst. Need to explain thru effective collisions.
5. Be able to give the five different ways to change the amount of reactant particles near each other per volume (see 4 above). They are a) reactant concentrations, b) surface area, c) stirring, d) increase/decrease pressure of a gas phase reactant, and e) decrease/increase volume of container (for gas phase reactant).
6. Draw a Potential Energy diagram for both an exothermic and endothermic reaction and identify the heat of reaction, potential energy of product/reactant/activated complex/activation energy. Student need to define the role of activation energy and activated complex in reacting reactants into products (e.g. ball rolling over hill). Also include knowing the "sign" of heat of reaction for exothermic/endothermic reaction.
7. Change the above Potential Energy diagram for the addition of the catalysts and how it affect the rate of reaction.