 Not anymore. So let's do this one, PCL5. So we're trying to do this hybridization thing here. So how do we justify? Because we would expect, of course, hopefully everybody thinks phosphorus is in the middle of this molecule. All the chlorines are on the periphery. And phosphorus is rehybridizing, becoming hypervalent. Is everybody OK with that thought process? So how does that happen? So well, we got to think of the valence electrons and phosphorus and where they're located. So let's go ahead and write those valence electrons. So 3s. And remember, we skip that 4s. I can go to the 3d's. We're filling. Boss, is everybody OK with what we've done so far? Why is that 3d there? Like what we said, right? We're skipping the 4s. Why? Because 3d is actually lower in energy when we think about it. Remember, we were talking about that. Those d orbitals, when they get filled, they can come condensed and things like that. So go back and watch those lecture videos if you have any trouble. OK, so how do we fill this up with the electrons or when we hybridize? We're hybridizing with those d orbitals. So of course, if we looked here, right, phosphorus should only be able to make three bonds. We know it makes five. We look here also. We know that those bonds, if we saw them, should be 90 degrees apart, right? Because the d orbitals, I guess this is something we didn't talk about in the last one, are on these three axes, x, y, and z axes. So those axes are 90 degrees apart from each other. And if you look, it's not the case with all of those bonds. In fact, PCL 5, we should be able to predict that it would be trigonal by a parameter of five bonds. So it should look like this. I guess you've got a 90 degree angle between those. But here, you've got a 120 degree angle. And here, you've got a 180 degree angle. Is everybody OK with that? So if you want to, you can pass this thing. Here, we can do this for you guys. So of course, those bond angles are not 90 degrees, or at least not all of them. So we need to be able to make five bonds. OK? How do we do that? Well, we need five orbitals to do that, and five electrons, which we've got five electrons. And we've got more than five orbitals. So the ones that we're going to use are the ones that are lowest in energy first, of course. So all of the s's, all one of the s's, all three of the p's. And that would give us four orbitals. So we need still one more. So we've got to go snag one of those d's. So if we're using one s, three p's, and one d, what is the hybridized orbital stuff? s, p, three d. And we put how many into the blender? Five. So let's write a hybridized theorem. So we're going to get how many out? Five, four, five. And they're all going to be equivalent in energy. And we're still going to have our four 3-d orbitals up there, OK? Now we're going to hybridized orbitals, our s, p, 3-d orbitals. And hopefully, now we realize that we can make five bonds. And again, I guess we use chlorine again. So remember, chlorine, it's got its half-filled orbital. So it's just going to use that d to stick on, OK? So we can, we'll just look at one of these bonds. So when we do that, we're going to have that s, p, 3-d bond, our orbital. And it's going to interact with the 3-p orbital of the orbital of the bond. Is everybody OK with that? Does that answer most of your questions then? OK, so when we see this, how many bonds are we expecting to have? Five, right? So phosphorus can make five bonds. So I'm going to erase this part, and we're going to kind of do Vesper theory on it, too. Is that OK? We've got it up here, like building the thing. We can justify that structure that I showed you. So in fact, the electronic structure is the same as I3 minus, if you recall. That was like an example we did, I think, two examples of them. So phosphorus, that's going to give us the Lewis structure. Phosphorus can do this, because it's period 3 or below. If we want to draw this in, you know, I'll get out of the way. If we want to draw this in, can I erase this, OK? I guess I expect you to be a speedrider, so. OK, so when we're going to draw something like this, in perspective, right? Equatorial coreings and axial coreings, remember we talked about this. What's the electronic structure? The cellular. Whatever the cellular structure is. Trigonal bioparamable, right? And I know I already said this a million times. But what's the molecular challenge? Trigonal bioparamable. How did you know it was trigonal bioparamable? The electronic geometry that is? There's no lone hair. I have electronic. Because there's five electron groups. Five electron groups. Everybody OK with that? If there's six, that's when it's octahedral. Then it's octahedral, yeah. We can do an octahedral one eventually. I'd like to get back and do a smaller one. Any other questions on this one?