 So let's do this boron trichloride, and you guys can help me out as much as you want. So boron, how many valence electrons? Three. Three. So everybody's okay with that, right? Would boron or fluorine be the central lab in this one? Boron. Boron, right? Why? And that's a good point, but fluorine only makes how many bonds? Three. One bond. Right? That's all right. Boron's going to make the three. That's the first thing you guys are doing, unless you guys are doing awesome. Okay? So are we cool with that? Everybody would have gotten that, right? And now we're going to do what? Fishers. Fishers, yeah. Like that. So what particle does this look like that we built before? Yeah, that's CO32 minus. Right? Okay. So what was the molecular structure of CO32 minus? Do you guys remember? Trigonal. No, pyramidal. Planar, right? Why would this be planar and not pyramidal? Because they're all on the same plane, but why would it not be pyramidal? Why is ammonia pyramidal, and this isn't? Doesn't have the valence electron to push the other bonds away. Okay? These are not as far apart as they could be, right? So let's draw Vesper theory. Using Vesper theory, I guess I should say. So what's the bond angle? Remember, bond angle is bond to bond. What's the bond angle? Predictive bond angle, 120 degrees. Very good. No, that's good. Okay. What's the electronic structure of this? Same as the molecular structure, trigonal perplanar, okay? So how about this? What's the electronic structure around the fluorine? Tetrahedral. Yeah, so the electronic structure around the fluorine is tetrahedral. You guys go with that? Why? Because there's the four areas of electron density. Any questions on this one?