 Okay, so let's show how boron goes from its atomic orbitals to its molecular orbitals in the molecule, or in a molecule such as boron trifluoron, okay, in other words. So if we look at boron, right, we know how to draw its molecular orbital diagram, or its atomic orbital diagram, its orbital diagram. So let's go ahead and do, well, let's just do it for the Baylons electrons though, okay. So in this case it's going to be, you guys can help me out, because it's 2s and it's 2p. And if we look at where it is, 1, 2, well, 1, 2, 3, alright, so 1, 2, 3. So if we're thinking about it like this, and its atomic orbitals, we might think that this boron should only be able to make one bond, is everybody okay with that? It's got only one half-billed orbital, but we know from the structure that it's making three bonds. And we know that it does make three bonds from our experience in chemistry so far. So we know that something must be happening with these atomic orbitals in order for it to be able to bond, is everybody okay with that? So that's something that we all know happens is rehypertization, right? So we're going to rehyper, so we're rehypertizing our boron, so this is the boron. Well, so we want to make three bonds, and we've got three electrons. So how many orbitals do we need to do that? Three. Three, okay. So what three are we going to take? This one. Yeah, two p's and one s, something like that, and we're going to have the one two p left. So let's go ahead and do that. So since we took one s and two p's, we're going to make sp2 orbitals. So that gives us a clue as to what the bond angle should be for these bonds. So we put in three, so we get out three, right? Whatever other thing you get out. And if you want to, you can put your two p orbital up there. And then you're just going to follow your filling rules, you get those three electrons there. And now, of course, the fluorines can come and make bonds with their two p orbitals, their unfilled two p orbitals. Is that all right with everybody? So if we wanted to draw, you know, one of the actual, well, let's draw it before on what it looks like with its orbitals. So we've got one, so this is an sp2 orbital. And then we've got one sp2, if you can imagine, coming out like that. And then the other one, can you guys tell? Like that. OK, so sp2, right? sp2, sp2. So those are the orbitals. It's molecular orbitals, that's what it's made. But it's also got still that two p orbital. And when you guys learn about organic chemistry, you know, this is where electrons will come. So this is called the Lewis acid, and we'll talk more about that, I guess next semester. But, you know, things with a lot of electron density will come in and attack that, because this doesn't have any electron density. It wouldn't mind having a full octet if you want to think about that. But anyways, the last thing we want to talk about is how the fluorine bonds to it, right? So we'll show it on this. We'll just do one of them, because it'll get way too messy here. But anyways, the fluorine, it didn't need to rehybridize, so sorry, we're going off the board. But that's a big load, and that's a big load. So naturally those two will be the same size. And this being the 2p orbital. And that overlap right there, that's your covalent bond. OK, so we've got the one there. Any questions, I guess? I'm going to kill it.