1. Unit 8 Kinetics and Rates of Reactions

2. What can we do to increase or decrease the rate of a reaction?

3. Collision Theory

4. What is Collision Theory?
Major idea of kinetic theory
Reacting particles will hit each other and the walls of the container they are in millions and millions of times
When they have enough energy, they stick to each other and will form a bond (products)
If not enough energy they will bounce off and try again

5. Continue Particles will do this until they form a bond
In addition to the energy level being correct, the particles also must be in the proper alignment to exchange/share electrons

6. What is a rate?

7. Rate Definition and notes
Rate is the speed or pace of a reaction
Measured in concentration and time
We expect reactions to have a rate that produces products in an efficient way
Faster is better for us

9. Activation Energy

10. Definition and Notes
Minimum amount of energy that is required to start a reaction
Think of it as a barrier to producing products
If you cannot pass this point, you cannot produce products
We search for ways to lower activation energy but NEVER TO INCREASE IT!!!!!!!!!!!!!!!!

12. Factors that effect the rate of a Reaction
1. Nature of Reactants
2. Concentration
Covalent slow
Ionic fast
Increase concentration increase collisions and increase rate
Decrease concentration decrease collisions and decrease rate

13. Factors 3. Surface Area 4. Pressure (Gases Only)
Increase SA Increase Rate
Increase Pressure Increase Collisions Increase Rate
Decrease Pressure Decrease Collisions and Decrease Rate

14. Factors 5. Catalysts 6., Temperature
Speed up reaction by lowering activation energy
Provide an alternate pathway for the reaction to take place
High temps increase rate
Low temps decrease rate
All about collisions