1. Reaction mechanism
Most reactions occur in a series of steps. Most you don’t see.
The reaction mechanism is these series of steps.

2. Reaction Mechanism Elementary Steps
a reaction where the rate law can be written from its molecularity = total # of atoms, ions, or molecules that must collide to produce a reaction

3. Elementary Steps Look at steps to determine overall reaction.
Look at overall order of reaction.
Unimolecular-one species: A --> Products
Overall first order rate = k[A]

4. Elementary Steps Look at steps to determine overall reaction.
Look at overall order of reaction.
Bimolecular-two different species or two of same species could be
A + B  Products or
2A  products or
2B  products
Overall second order
rate = k[A][B] or rate =k[A]2 or rate = k[B]2

5. Elementary Steps Look at steps to determine overall reaction.
Look at overall order of reaction.
Termolecular-
three different species (A + B + C  products) or
2A + one species (2A + B  products) or
3A (3A  products) or ……
Overall third order
rate = k[A][B][C] or rate =k[A]2[B] or rate=k[A]3

6. Reaction mechanism It was found to be rate = k[NO2]2
EX:
NO2 + NO2 --k1--> NO3 + NO slow
NO3 + CO --k2--> NO2 + CO2 fast
NO2 + CO > NO + CO2
As usual, the rate law was determined experimentally
It was found to be rate = k[NO2]2
What do you notice?

7. Reaction mechanism EX: NO2 + NO2 --k1--> NO3 + NO slow
NO3 + CO --k2--> NO2 + CO2 fast
NO2 + CO ---> NO + CO2
No CO?
Must be zero order. Don’t include it in rate law.

8. Reaction mechanism
EX:
NO2 + NO2 --k1--> NO3 + NO slow
NO3 + CO --k2--> NO2 + CO2 fast
NO2 + CO ---> NO + CO2
The rate law is based on the slowest step in the reaction! This is called the rate determining step. Always the case.

9. Reaction mechanism
EX:
NO2 + NO2 --k1--> NO3 + NO slow
NO3 + CO --k2--> NO2 + CO2 fast
NO2 + CO ---> NO + CO2
The sum of the steps must equal the overall balanced equation.
(Need to justify your answer – Part ONE of TWO)

10. Reaction mechanism
EX:
NO2 + NO2 --k1--> NO3 + NO slow
NO3 + CO --k2--> NO2 + CO2 fast
NO2 + CO ---> NO + CO2
The slowest step (rate determining step) must agree with the experimentally proven rate law
(Need to justify your answer – Part TWO of TWO)

11. Reaction mechanism 5) Vocabulary:
EX:
NO2 + NO2 --k1--> NO3 + NO slow
NO3 + CO --k2--> NO2 + CO2 fast
NO2 + CO ---> NO + CO2
5) Vocabulary:
a) NO3? It was produced in reaction 1 and then consumed in reaction This is called an intermediate.

12. Reaction mechanism 5) Vocabulary:
EX:
NO2 + NO2 --k1--> NO3 + NO slow
NO3 + CO --k2--> NO2 + CO2 fast
NO2 + CO ---> NO + CO2
5) Vocabulary:
b) NO2? Need it for the reaction in exp 1 but then is not consumed in exp 2. By definition this is a catalyst.

14. Drawing an energy diagram for a mechanism

15. AP Problems 1999 #3 2 NO + Br2 ---> 2NOBr was found experimentally.
Rate = k[NO]2[Br2]
The following mechanism was proposed for the reaction
Br NO ---> NOBr2 (slow)
NOBr2 + NO ---> 2 NOBr (fast)
Is this mechanism consistent with the given experimental observations? Justify your answer. Does it fulfill all the requirements?

16. Other AP problems
2000 # 6e
Consider the reaction O NO --> O NO2
Rate = k [O3][NO]
The following three step mechanism is proposed for the reaction. Identify the step that must be the slowest. Explain
Step 1: O3 + NO ---> O + NO3
Step 2: O + O > 2 O2
Step 3: NO3 + NO ---> 2 NO2

17. 2002 #7
The proposed mechanism for the depletion of O3 in the upper atmosphere is shown below:
Step 1 O3 + Cl > O2 + ClO
Step 2 ClO + O ---> Cl + O2
a) write a balanced equation for the overall reaction represented by Step 1 and 2
b) Identify the catalyst in the mechanism above. Justify your answer
c) Clearly identify the intermediate in the mechanism above. Justify your answer.
d) If the rate law for the overall reaction is found to be rate = k[O3][Cl]
  d1. Find the overall order of the reaction
d2. Designate appropriate units for the rate constant, k
d3. Determine the rate determining step of the reaction and justify your answer.