1. Chemical Kinetics
Reaction rate - the change in concentration of reactant or product per unit time.

2. Factors Affecting Rates
Temperature
Concentration of reactants
Particle size
Presence of a catalyst

3. Rates
Average rates - the difference in concentration over a set amount of time. Table 12.2
Instantaneous rates - calculated from the slope of the line tangent to the curve at a certain point.

4. Reaction rates
Rates are not constant.
Rates vary with time because concentrations vary with time.

5. Rate Laws
Rate = k[A]n[B]m[C]p
k = rate constant
n,m,p = order ; must be determined by experiment.

6. Differential rate law
Expresses how a rate depends on concentration.
Often this is just called the rate law.

7. Integrated rate law
Expresses how the concentration depends on time.

8. Reaction Mechanism
The series of elementary steps by which a reaction occurs.
An elementary step is a step whose rate law can be determined from its molecularity.

9. Molecularity
The number of species that must collide to produce the reaction in that step.
Unimolecular involves one molecule.
Bimolecular and termolecular involve 2 and 3 species respectively

10. Intermediate
A species that is neither a reactant or a product. This species is produced and consumed in the reaction.

11. Rate Determining Step
This is the slowest step of the mechanism. The reaction can only proceed as fast as this rate determining step will allow.

12. Requirements of Mechanisms
The sum of the elementary steps must give the overall balanced equation.
The mechanism must agree with the experimentally determined rate law. The rate determining step.

13. Collision model for kinetics
Reactant molecules must collide in order to react.
Concentration
Particle size
Temperature
Molecular orientation

14. Requirements for reaction
The collision energy must equal or exceed the activation energy.
The orientation of the reactants must allow the formation of new bonds.