DO NOW

1. DO NOW • Get out Reaction Mechanism Practice. • Pick up review. • Kinetics Test Monday. • Concentration and Reaction Rate lab due Tuesday.

2. REACTION MECHANISM PRACTICE

3. REACTION MECHANISM PRACTICE

4. PRACTICE

5. KINETICS Review

6. REVIEW • Define Kinetics. • Kinetics: The area of chemistry concerned with the speed at which reactions occur. • Some reactions are fast and some are slow. • Make sure you can make a distinction between rate and time. • If the rate of a reaction is high, the time of the reaction is low.

7. REVIEW 2. Discuss the collision theory. • The particles must collide. • The particles must collide with the correctorientation. • The particles must collide with sufficient energy to form an activated complex.

8. REVIEW 3. List the factors (nature of reactants, concentration, temperature, surface area, and catalysis) that effect reaction rates and be able to explain them according to collision theory. Nature of the Reactants The rate of a reaction depends on the particular reactants and the complexity of the bonds that have to be broken and formed in order for the reaction to proceed. • Ionic reactions occur very fast. • Reactions involving covalent bonds take place more slowly. • The phase of the reactants can have an effect on reaction rate.

9. REVIEW 3. List the factors (nature of reactants, concentration, temperature, surface area, and catalysis) that effect reaction rates and be able to explain them according to collision theory. Concentration • The rate of reaction is defined as a change in the concentration over time. • WHY: Increase concentration and there are more particles in a given volume. So, the chances of the particles colliding increase.

10. REVIEW 3. List the factors (nature of reactants, concentration, temperature, surface area, and catalysis) that effect reaction rates and be able to explain them according to collision theory. Surface Area • The larger the surface area of the reactant, the greater the number of particles that are exposed for the reaction. • WHY: Increasing the surface area increases the frequency of collisions.

11. REVIEW 3. List the factors (nature of reactants, concentration, temperature, surface area, and catalysis) that effect reaction rates and be able to explain them according to collision theory. Temperature • Increased temperature usually increases the reaction rate. The temperature rises and the average kinetic energy increases. The faster the molecules move, the more frequently they will collide. • WHY? Increasing the temperature gives more particles the required activation energy and also increases the effectiveness of the collision.

12. REVIEW 3. List the factors (nature of reactants, concentration, temperature, surface area, and catalysis) that effect reaction rates and be able to explain them according to collision theory. Catalysts • A catalyst is a substance that increases the rate of a reaction without itself being used up in the reaction. • A catalyst does not appear in the overall chemical equation. • Catalysts work by lowering the amount of energy required to get the reactants to react. • Opposite from catalysts are inhibitors. • Inhibitors slow down the rate of a reaction by binding to the reactants to keep them from reacting.

13. REVIEW 4. Identify the parts of a potential energy diagram including activation energy, Ea, transition state, energy of reactants, energy of the activated complex, energy of products, and heat of reaction.

14. REVIEW

15. REVIEW 5. Identify a potential energy diagram for an exothermic reaction and an endothermic reaction.

16. REVIEW 6. Know what a catalyst is and how it affects a potential energy diagram.

17. REVIEW 7. Describe reaction mechanisms for simple reactions and identify the parts of the multiple steps as well as determine the final balanced equation. Most chemical reactions consist of a series of steps. A series of reactions that lead the reactants to become products is called a REACTION MECHANISM. A detailed reaction mechanism describes the order in which bonds breakand atoms rearrangethroughout the course of the chemical reactions.

18. REVIEW 7. Describe reaction mechanisms for simple reactions and identify the parts of the multiple steps as well as determine the final balanced equation. How to Solve These:  FIRST: Write the balancedequation. SECOND: Check off those substances that have been used. THIRD: Fill in the missingreactants and/or products. • REMEMBER: EACHline is a balanced equation.

19. REVIEW 7. Describe reaction mechanisms for simple reactions and identify the parts of the multiple steps as well as determine the final balanced equation. • INTERMEDIATE PRODUCT: A substance that is produced in one step of a reaction and then is consumed in a later step of that reaction. • It appears first as a product and later as a reactant disappears. • The rate of the overall reaction is limited to the rate of the sloweststep and is called therate determining step. CATALYST: A substance that disappears in one step of a reaction and then appears in a later step of that reaction. It appears first as a reactant and later as a product.

20. THE TEST 11 multiple choice 4-5 questions concerning a reaction mechanism 3 short answer 2 potential energy diagrams with 13-15 questions

21. TO DO • Work on lab and review sheet. • Test Monday. • Review due Monday for test redo points. • Lab due Tuesday.

22. DO NOW • Turn in Review sheet. • Get ready for test. You might want a calculator but it is not necessary. • Lab due tomorrow. • NO ELECTRONIC DEVICES AT ALL (even music) during the testing time. I will take that device and give it back Friday afternoon or to your parent, whichever comes first.