 Let's do this next structure, sulfur hexafluoride. So hopefully you're like, whoa, that's weird, okay? Because sulfur and fluorine, you would expect them to make just SF2, okay, from what we've learned previous. But remember we said that if you get down to the third period, those central atoms can actually expand their valence. So we're going to show the expansion of valence here. So hopefully you see that sulfur is the central atom, okay? And the thing that we're going to do is just draw its normal valence electron. So one, two, three, four, five, six. Notice I drew them a little further apart than what I normally do. So when something expands its valence, when an atom expands its valence, or a central atom expands its valence, what it actually does is it'll split up those two electrons and actually allow them to bond separately, okay? The reason being is because it's got these D orbitals that it can push these electrons up to and actually allow the D orbitals to participate in bonding. And we'll talk more when we talk about molecular orbital theory. We'll talk more about promoting these to the D orbitals and actually showing the molecular orbitals. But anyways, draw our fluorines. So again, I don't know if I actually need to do this for you guys, but five, six, right? So, like I said, one of the electrons in the pair will make a bond, okay? So we'll have something like that. There's two of the substituents in there, what we call axial positions. And then four of them in the equatorial. So equatorial, like, on the equate. Well, what would be the bond angle between here and here for dated bonding? What would you expect it to be? So this is called, so I guess the structure, I guess I should say, both the electronic and the molecular is called octahedral. So we've got four around that equatorial axis. So what is the furthest four things can be on a straight line around a circle? What is that? 90, right? 360 divided by 4 would be 90, right? Because they're all on the same plane, right? Can you see that? They're all on the same plane, so it has to be 90. Only those four, so if you can't see it. Oh, I understand. Equator, right? You know, the equator, it's like, look at the Earth, right? There's this line around the Earth that we call the equator. So these guys, for those of you who are listening, right, and don't know me, you know, like I know my students well enough to be able to say that. But anyways, so look at these. You see the equatorial, in this case, flooring, right? So if you look, right, 90 degrees apart from each other, okay? So these guys are on the axis, right? You see that? So we call them axial, okay? So, what is the bond angle here? Here, sit here. What is that? 90 as well? Okay. Why? Because there's four on that side too. Was that just a good guess, or? Okay, so is everybody okay with the octahedral geometry? Okay. So again, remember, this is octahedral both electronically and we'll say electronically. That's the best we're going. Are there any questions on this one? Again, these period three and below's can expand their bay. So that's why it's doing it. So whenever you see something that looks a little weird, it probably doesn't expand in its bay.