 OK, it's true. You think it's funny, but it's totally true. Anyways, I think it's funny, too, honestly. So let's try this reaction here. Hopefully you guys can see already that this is different than the last reaction that we did. This is, first of all, a single replacement reaction at four. The last one, do you guys remember? This is a double replacement reaction. So is this a redox reaction or a non-redox reaction? Redox. Redox, right? It's a redox, OK? So hopefully you guys can see that, and I know that you guys can. So since it's a redox reaction, that means something has to be reduced and something has to be oxidized, right? OK, so let's go about figuring out what that is. And in fact, this is touching on what we're going to get to at the end of this lecture, but it's still OK to start it there. So the first thing we want to look at is what the two ions or the two metals have done, right? So what we're seeing here is magnesium is starting at a zero oxidation state, like that. And it's going to a two plus oxidation state like that. The other thing that we see, hopefully, is that Cu starts as a two plus oxidation state. It goes to. So do you guys remember what we say Leo of the lion says, Gerr and all of that stuff? The easy thing to remember, I always think, is when I look at these numbers. The one that gets smaller is the one that's reduced. So which one of these is reduced? Copper gets reduced. Copper gets reduced. So copper gets reduced, so magnesium must get what? Oxidized. Oxidized, OK? So they're opposite of each other. So one second. So just like when bleach does the bleaching, right? So something that gets reduced, right, has gotten reduced by something else, OK? Does that make sense? So the thing that gets oxidized is the reducing agent, right? And the thing that gets reduced is the oxidizing agent. Why? Because this thing is oxidizing this thing, like that. So just like bleach doesn't get bleached when you bleach things. It's the thing that the bleach encounters that gets bleached, if you want to think about it that way. For me, it's easiest to look at it through these half reactions, say which one gets reduced, which one gets oxidized, and then go backwards from that, OK? So since this one got reduced, it must be the oxidizer. Does that make sense? Or the other one gets oxidized, right? So the thing that's oxidizing it must be the oxidizer. What if it went to like a 0 to a negative 2? That still would be reduced, right? 0 to a negative 2, yeah. That's still being reduced, yeah. So if the number gets lower, that's reducing the number, right? Is everybody OK with that? Any questions on reducing and oxidizing agents? OK, good question.