This is one of the best depictions of a free radical reaction I have seen. It shows what can go on in this reactions and how we get from starting material to desired final product.
Initiation = 1 neutral provides two radicals. This is what starts the entire reaction. This is also the only initiation step that can occur as CH4 is not going to participate in that type of reaction.
Propagation = 1 neutral + 1 radical provides a different neutral and a different radical. In this reaction, the most likely propagation is chlorine abstracting a proton from methane to give HCl and the methyl radical. The next step is where the methyl radical breaks up two Cl atoms. What I really like about this depiction is that it shows that the Cl* from reaction 3 can be recycled back into step 2. This means that the reaction is self-propagating. This also means that IN THEORY you could have one initiation reaction, followed by a bunch of propagation, ending with one termination reaction. Of course, in real life, for many reasons, this does not happen as there are lots of initiation reactions.
Termination = 2 radicals providing one neutral. The part to remember here is that any two radicals can get together to terminate the reaction and form a neutral species. Since we have 2 types of radicals in the reaction (Cl* and CH3*) , there are three combinations of potential termination steps. Reaction 4 gives us back starting material, so it is fine. Reaction 6 gives us product, so it is also fine. Reaction 5 give us a byproduct, which strangely enough can replace methane in the propagation step and give us another by-product.
Think about this picture and figure out all of the side reactions that might occur to fowl up the reaction. Then, (for you advanced students) think about what ways exist that you can minimize those side reactions.
Hope this was helpful to you all, and as always, happy reacting.