 Okay, so it says the central atom in bromine pentafluoride has how many bonding pairs of electrons and how many non-bonding pairs of electrons? So let's just go ahead and build this structure. So bromine pentafluoride, so hopefully when you look at a structure or a molecular formula like this, you see that of course one of these atoms is going to be the central atom, right? Which one do you predict will be the central atom? Bromine. Bromine, why would you predict that? So does fluorine, right? It can expand its valence, right? So fluorine can't expand its valence, why is that? It's not big enough. Yeah, it's not big enough, right? So it can't have all those arms around. So let's put bromine in the middle there and let's draw its valence electrons. So remember it's expanding its valence. Draw them a little further away from each other. And how many fluorines do we have? Well, five. So five of those electrons are going to be making bonds. So let's draw the fluorine. And again, we're just starting constituent atoms so we can show everyone how we build these things. Fluid structure wise. And then we can go to talk about the electronic and the molecular structure. Okay, so there's five fluorines. So let's show the bonds being made. Okay, so hopefully you guys can see, right? We're going to have five bonds and one lone pair, right? Because we've got those two electrons left over. So how many electron groups is that five bonds and two, and a lone pair? Six. Six, right? So what's the electronic structure of this thing going to be? Optical. Optical. Okay, so let's just keep that in mind while we're building. Well, let's just go ahead and skip the Lewis structure part and just build or show the three-dimensional structure of this molecule. So bromine. And so we're going to have the one fluorine straight down. And since this is octahedral, right, we're going to have four groups in the plane here. Remember how to draw those? I guess we've already answered the question in advance on this. But let's just keep going with some. So is everybody cool with drawing something like that? So what did we say the electronic structure was octahedral? What would the molecular structure be? Yeah? Square gram. So why is that? Because remember, if you're like a little guy looking at that thing, you can't see these lone pairs up there. You can only see the atoms. This is an upside-down square parameter. Normally we draw it the other way. But it's fine to draw it this way. It's just like standing on its head or something. And I guess what was the question? It said how many bonds and how many lone pairs? So how many bonds, how many lone pairs? So bonds, I guess you guys can count those. Somebody tell me just for fun. Five. Five bonds and lone pair electrons? One lone pair. Anything else you guys want to know about this? What's the bond angle here? Somebody tell me that. 90, right? Why would it be 90? Because there's four on a plane, right? So four on a plane, the furthest they can get apart is 90 degrees. What about this bond angle here? What would you expect it to be? It's probably a little different than that. But yeah, you might expect it to be 90. It might be a little bit less than 90, because the lone pair kind of pushes these all down. But nice. Today, going to work.