 Okay, so let's start today with this mechanism of the chlorination of methane. So you can see here, we've got this thing, this molecule here, methane, everybody knows. We're going to react it with chlorine, and the chlorine's going to react with white first. And then you're going to make methyl chloride and HCI. So let's go over this mechanism. So the first step, remember, in all, this is a radical reaction. Of course, hopefully you guys can see that and tell it's a radical reaction. All radical reactions start with an initiation step. So, we've got the initiation. Pins is, like we said before, light shines down, hits this bond, and this bond homilizes, right, at your initiation. You have the two fluorine radicals, or fluorine atoms, whichever way you want to think about them, atoms are radicals. Okay, so now that we've got these radicals, then we're going to have the propagation step. We're going to take a radical and make a radical. So, how do we do that with this C-A form? Remember, this is the reactive species. So, this is going to do the reactivity. It sees one of these C-A bonds where your fish of arrow is showing the ocean of one electron. So, when we do that, that's where we make our HCl. Okay, you guys see that? We're also making the methyl radicals and have another propagation step. And in fact, it's just going to keep propagating. This is like one of those reactions that we talked about the other day where a lot of organic reactions are this way, where you can use the same thing over and over and over because it's being produced in the reaction previous and it's going to be reacting in the next reaction, right? So, you don't just have, in other words, you don't just have one of these and one of these. You have billions of them, you know? So, anyways, you've got this guy. And remember this initiation step, when we put light, this only breaks up a tiny, tiny portion of the chlorine molecules that are in there, okay? It doesn't break up very many, but you only need the one radical to start the reaction. Remember, all radical reactions are these chain reactions. So, we're going to propagate again. So, what did we make? We made the methyl radical. And we've got another Cl2 molecule. It's a very lay-bottle bond, right? So, you can tell that by light hitting it, it'll break it. So, we're going to break that bond again here, propagating the radical. So, you propagate this radical here and that goes on and does this reaction to another one, okay? So, you don't need, well, you don't want to think about these reactions as I have to do, I have to use everything in the one reaction, okay? So, it doesn't always balance out. In fact, you can see here how you balance the net reaction, right? So, we've got, what does it say? CH4 plus the chlorine radical opposed to the methyl radical plus HCl. The hydrogen abstraction occurs in CH3, the methyl radical, plus Cl2, right? So, this is going to react. Yeah, this is the same thing we're doing over here. When we do that, we make methyl chloride plus the chlorine radical again. So, remember, a reaction equation is just like an algebraic equation, right? So, and if something is on one side and on the other, so we're going to combine these two reactions into the formal overall reaction, right? So, in other words, let's just combine them all, okay, first. So, CH4 plus Cl dot CH3 dot plus Cl2 goes to CH3 dot plus HCl plus CH3 Cl plus Cl dot, like that, okay? And then we just see what's on this side, what's on this side, and cancel that, okay? So, they're the same. So, Cl dot is the same, right? We've got the methyl radical like that. And is there anything else? That's all I see. Sometimes you've got to take a step back. I think that's all I see. So, CH4 plus Cl2. And then here we're just going to put HB because, you know, makes HCl plus CH3, okay? So, that's how you balance reactions. You know that from general chemistry, though, right? So, this is what we would call the net reaction. Propagation stuff? Why did you break a second Cl2 instead of just using the... Well, like I said, there's very little of this. This one's probably already reacted with something else. These things are super reactive, you know? It's like, if you've got, you know, two guys that are ready to fight, you know, while one of them is fighting somebody, the other guy is not going to just sit there. He's going to go fight somebody else, you know what I'm saying? So, that's what you've got to think of. So, these guys, there's a bunch of them in there, and they're not, you know, reactive yet. So, once this happens, this bond is easy to break. Once you make this methyl radical, it's like, man, I really don't like it. The chlorine doesn't mind it as much, but this really doesn't like it, so it goes and reacts with the methyl. So, that is called the beatermination step. Well, okay, so, this is propagating, propagating, propagating, and eventually there will be a termination step, but it'll only happen once. At the very, very end, okay? So, yeah, and what would happen is, like, you'd have maybe two methyl radicals come together, that'll stop the reaction. All termination steps stop the chain reaction, right? So, you can have, if this guy finds another methyl radical, you can come together and make, you know, that thing, like that, right? So, you'd have, in other words, termination steps. What kind of termination steps do we have? We could have this reacting with another one. You could have, like, Dave was saying, you know, this methyl radical with the chlorine radical, like that. So, those are termination steps there, right? Or you could have the two chlorines, yeah. And so, those are all termination steps. Once that happens, it stops the chain reaction. But, of course, you're shining light on the thing. So, you know, it's gonna keep going until all your chlorine is, or all your stuff is chlorine. Okay? There any more questions on this?