Let's do this one now, okay? PCL 5? Yeah, I'm all right. Let's do this just as you'd be in my camera. PCL 5, okay? So how will we normally do this? Okay, so hopefully you guys can already see something weird about this, right? As you would expect, phosphorus and chlorine to make blood content. PCL 3. PCL 3, okay? But it's not that. It's expanded. So phosphorus must be expanding its veins, okay? So let's draw phosphorus as the central atom. Like that. Okay, and we'll put our advertised around it. So does everybody okay with what I've done so far? That makes sense. What happens is these three would expect to be bonding. What will happen is one of these will be promoted into another orbital, so it's by itself so they can bond. We'll talk more about this in a second. We do molecular orbital. So like that. So this is going to give us something that's more, got more things bonded to the central atom than the tetrahedral electronic structure. So everybody okay with that? So in this case it's going to be five things. I erase this so I can show the perspective. It's everybody got this. So when we draw it in, we're going to have four atoms in the plane, like that, and then two atoms, not at all. And remember this is through Vesper theory, as far as they can get away from each other. So you see one, two, three, four atoms in the plane, this one's coming towards us, that one's going away. So we call the ones around the center of equatorial, like an equator. Equatorial, like an equator. So if you want to look, those three are the equatorial. These two are the axial. So everybody okay with that? Equatorial and axial. So what was your question? How do you know when they're going to be on a different plane? You just got to know the central atom and how many things are bonded to it. So how many electron groups? So just like what we're doing to treat, this is the next one up, okay? And then are those two C L's on the same plane? These two as each other, yes. They're all on the same plane, right? So all four of those atoms are also on the same plane too, right? But there's one, this one's not on the same plane as these things, right? This one's in front, that one's in front. But this one, this one, this one, and that one are all on the same plane if you turn it over like that. Check this out. Here, catch this for her. I think catch things. Yeah, but you can't see, right? Yeah, that's true. You couldn't even see the clock two seconds ago. Okay, so anyways, this thing, hopefully you can see kind of the pyramid, right? You see the pyramid there and kind of an upside down pyramid there. This thing is called... ...by pyramidal, okay? So, and if we look, this bond angle here is 90 degrees, and this bond angle here is 120 degrees. Okay? As you would expect. So, trigonal bipyramidal, right? So, there's two triangles on top of each other. So, are there any questions about this one? So, are the three C-Ls in the plane with the P? Is that because P should have three, should have three C-Ls? How did it supposed to be if it has fun? It has nothing to do that. It's just about how far away these electron groups want to push each other. Okay? It has nothing to do with what it's supposed to do, previous. Okay? So, it's just that these ones want to be as far apart from each other as possible. These ones want to be as far apart from each other as possible, and these ones want to be as far apart from each other as possible. So, you also have another bond angle here, right? That one, which is 180 degrees. So, if I ask you electron structure, is this trigonal bipyramidal? Okay? And the molecular structure, is also trigonal bipyramidal. Okay? Are there any questions about this one? Okay, cool. So, I'd also say go watch the other video. I made one of an octahedral complex, which is that one that we talked about earlier, SF6. Okay? So, I recorded that video earlier. It's fairly similar to this one. Okay?