Week of 2/29/16

1. Week of 2/29/16 When the products have more energy than the reactants, the reaction is EXOTHERMIC or ENDOTHERMIC? When the reactants have more energy than the products, the reaction is EXOTHERMIC or ENDOTHERMIC? When heat is given off in a reaction, it is EXOTHERMIC or ENDOTHERMIC? When heat is absorbed in a reaction, it is EXOTHERMIC or ENDOTHERMIC?

2. Answers When the products have more energy than the reactants, the reaction is EXOTHERMIC or ENDOTHERMIC? When the reactants have more energy than the products, the reaction is EXOTHERMIC or ENDOTHERMIC? When heat is given off in a reaction, it is EXOTHERMIC or ENDOTHERMIC? When heat is absorbed in a reaction, it is EXOTHERMIC or ENDOTHERMIC?

3. Answers When the products have more energy than the reactants, the reaction is EXOTHERMIC or ENDOTHERMIC? When the reactants have more energy than the products, the reaction is EXOTHERMIC or ENDOTHERMIC? When heat is given off in a reaction, it is EXOTHERMIC or ENDOTHERMIC? When heat is absorbed in a reaction, it is EXOTHERMIC or ENDOTHERMIC?

4. Answers When the products have more energy than the reactants, the reaction is EXOTHERMIC or ENDOTHERMIC? When the reactants have more energy than the products, the reaction is EXOTHERMIC or ENDOTHERMIC? When heat is given off in a reaction, it is EXOTHERMIC or ENDOTHERMIC? When heat is absorbed in a reaction, it is EXOTHERMIC or ENDOTHERMIC?

5. Answers When the products have more energy than the reactants, the reaction is EXOTHERMIC or ENDOTHERMIC? When the reactants have more energy than the products, the reaction is EXOTHERMIC or ENDOTHERMIC? When heat is given off in a reaction, it is EXOTHERMIC or ENDOTHERMIC? When heat is absorbed in a reaction, it is EXOTHERMIC or ENDOTHERMIC?

6. Chapter 17Reaction Kinetics

7. Ch 17.1 Reaction Kinetics

8. Chemical Reactions • Activation Energy: the minimum energy that colliding particles must have in order to react. • Activated Complex: an unstable arrangement of atoms that forms momentarily at the peak of the activation-energy barrier. • This is also called the Transition State.

9. Energy Diagrams • ∆Eforward = energy of products – energy of reactants • ∆Ereverse = energy of reactants – energy of products • Ea = energy of activated complex – energy of reactants • Ea’ = energy of activated complex – energy of products

10. ∆Eforward is positive for endothermic and negative for exothermic ∆Ereverse is negative for endothermic and positive for exothermic

11. Examples!!

12. Science Starter When the products are higher than the reactants on an energy diagram is the reaction ENDOTHERMIC or EXOTHERMIC? What is the highest point on the energy diagram called? The line drawn from the reactants that points to the products is labeled as ____.

13. Science Starter When the products are higher than the reactants on an energy diagram is the reaction ENDOTHERMIC or EXOTHERMIC? What is the highest point on the energy diagram called? The line drawn from the reactants that points to the products is labeled as ____.

14. Science Starter When the products are higher than the reactants on an energy diagram is the reaction ENDOTHERMIC or EXOTHERMIC? What is the highest point on the energy diagram called? Activated Complex The line drawn from the reactants that points to the products is labeled as ____.

15. Science Starter When the products are higher than the reactants on an energy diagram is the reaction ENDOTHERMIC or EXOTHERMIC? What is the highest point on the energy diagram called? Activated Complex The line drawn from the reactants that points to the products is labeled as E .

16. Ch 17.2

17. Rate Influencing Factors • The rate of a chemical reaction depends upon temperature, concentration, particle size, and the use of a catalyst. • The nature of the reactants and their bonds is also a factor, but not one that can be easily changed so we will not talk about it.

18. TEMPERATURE CONCENTRATION Raising the temperature speeds up the reaction and lowering the temperature slows down the reaction. The higher the concentration, the more likely collisions will take place, which increases the reaction rate.

19. PARTICLE SIZE • The smaller the particle size, the more surface area, which increases the reaction rate. • Adding a catalyst will increase the rate of reaction, in some cases, better than increasing the temperature. • Inhibitor: a substance that interferes with the action of a catalyst. • These will slow down or even stop a reaction. CATALYST

20. Science Starter How do the following affect reaction rate? Decreasing temperature Adding a catalyst Increasing Surface Area Increasing Particle Size Decreasing concentration

21. Science Starter How do the following affect reaction rate? Decreasing temperature Decrease Adding a catalyst Increasing Surface Area Increasing Particle Size Decreasing concentration

22. Science Starter How do the following affect reaction rate? Decreasing temperature Decrease Adding a catalyst Increase Increasing Surface Area Increasing Particle Size Decreasing concentration

23. Science Starter How do the following affect reaction rate? Decreasing temperature Decrease Adding a catalyst Increase Increasing Surface Area Increase Increasing Particle Size Decreasing concentration

24. Science Starter How do the following affect reaction rate? Decreasing temperature Decrease Adding a catalyst Increase Increasing Surface Area Increase Increasing Particle Size Decrease Decreasing concentration

25. Science Starter How do the following affect reaction rate? Decreasing temperature Decrease Adding a catalyst Increase Increasing Surface Area Increase Increasing Particle Size Decrease Decreasing concentration Decrease

26. Science Starter How do the following affect reaction rate? Decreasing temperature Decrease Adding a catalyst Increase Increasing Surface Area Increase Increasing Particle Size Decrease Decreasing concentration Decrease