[bobert16]

Hi, I have the following net reaction:
CCl2F2 + O3 + O -> CClF2 + Cl + 2O2

This is the given mechanism:

1. Rapid Equilibrium: CCl2F2 <-> CClF2 + Cl
2. Slowest Step: Cl + O3 -> ClO + O2
3. Fast Step: ClO + O -> Cl + O2

I had to find the reaction intermediates. I identified Cl and ClO, as they are produced and consumed without affecting the overall reaction. However, there is at least one more I am missing. I would really appreciate the help in finding the other intermediate... my mind is drawing a blank.

[enahs]

Chlorine is one of the 7 atoms you are supposed to remember is diatomic. That is, it does not just sit around as Cl, it forms Cl₂ gas when given a chance.

[bobert16]

I know Chlorine is diatomic, but Cl₂ gas is not formed in this reaction.

I simply wrote the mechanism provided by my teacher for the overall reaction (the mechanism is the elementary steps that occur to create the overall reaction).  In these elementary processes, a Cl radical is formed (Elementary Step 1) and then immediately used up (Elementary Step 2).  This indicates that the Cl radical is a reaction intermediate.  The ClO radical is also a reaction intermediate - it is produced and used up in the elementary processes without affecting the overal reaction.

My question is what is the other intermediate present?  There are supposed to be three of them, but I can't think of the third and final one.

[Sam (NG)]

Is the oxygen radical a reactive intermediate? If i was doing steady state analysis i would be considering it i think. Oh no, wait, you've put an oxygen radical in the reactants.  But surely that is formed from the photolysis of Ozone (or some equivalent reaction).  Is this an atmospheric reaction?