 OK, let's briefly discuss these radical initiators. So you've already learned of one radical initiator, and we talked about it before. It's this NBS. Do you guys remember that? And it had that nitrogen-broming bond. And remember, we talked about how it was a real weak bond due to the orbital overlap is bad between the nitrogen, which is very small, and a very, very big, right? So in this case, as you can see, we don't have that similar big, small orbital overlap. These two atoms and all of these examples are the same atom, right? Two C-levels, two oxygens, two oxygens. So they're all the same size. But what you want to know about all of these is that these, especially these halogens, right? They have a weak halogen bond, OK? And you know that we talked about that with Br2. We could shine light on it and break it apart too, OK? So it's very similar. Chlorine is more reactive, and we'll talk about the different halogens and their reactivity in a little bit. But chlorine is the one that you see used most often. And it's due to its very weak bond there. You can see it's 243 kilojoules per mole, right? These peroxides, if you guys have ever used, like, hydrogen peroxide or whatever, right? You know that it's a very reactive material, OK? The reason being is because of these oxygen-oxygen bonds. So this could be like, you think of this as like hydrogen peroxide or something like that. Sometimes you'll have these organic peroxides, so you can dissolve them into organic solvents, you know, and use them that way. But anyway, as you can see, when we have that oxygen-oxygen bond, what's going to happen? So in both of these, right, let's draw the mechanism. The mechanism of that one is there, right? Of course, the mechanism of that one is just like that. This oxygen-oxygen bond is very weak, too. They would not prefer to be bonded to each other. And then, of course, once you make what's called a peroxy acid, these things here, these are even got even a more weak oxygen-oxygen bond due to the resonance that you can. So let's draw a couple of resonance structures of this thing, right? So we've got that one drawn there for us. So we should be able to draw another one. Hopefully, everybody can do it. Remember, whenever you can make resonance, that gives stability to the particular structure that you're looking. So this decrease in bond dissociation energy is due to the relative stability of the radical that's formed. So this is stable, especially relative to something like this that has no ability to resonate. So is everybody OK with that, if that makes sense? You can initiate these usually with either heat or light. It'll give them enough energy, not very good. Do you think that's still the same? It's two resonance structures, right? That radical, that electron, that electron on both of those things, OK? So it's got a partial character on both of them. They're resonance structures of each other. Why did it label this oxygen 1? That's still oxygen 1, right? Label that oxygen 2. That's still oxygen 2. Don't think too, thinking way too hard about it, OK? Any other questions?