 So I guess the question was, let's show or demonstrate how to go from the isolated beryllium atom to the hybridized beryllium atom in this beryllium dichloride compound. Just want to think about it that way. So beryllium would first got to think about what its atomic orbitals look like. So and when we're talking about atomic orbitals, we're talking about the valence shell. So what we want to do is think about drawing a condensed molecular orbital diagram. Is that OK? Or atomic orbital? So in this case, you can help me out if you want. But beryllium, if we look at a periodic table, it's going to have in its valence shell just the two electrons in the 2x. So it's got the 2s orbital. But it's also got the 3 2p orbitals very close in energy to that 2s. Does everybody remember that when we were talking about this? OK, so let's fill its orbital diagram. So when we do that, it's only got the two electrons and it's valence shell, so we fill it like that. If we look at this, beryllium should not be able to make any bonds, because it doesn't have any half-filled orbitals. And remember, we need half-filled orbitals to make bonds. Because when we're thinking about the chlorine atom, when we're looking at its 3p, so its valence shell, it's got that half-filled orbital that it can make its bond up. In fact, chlorine in this structure doesn't need to rehybridize. Recall that? Beryllium, in order to make two bonds, needs to have two half-filled orbitals. Is everybody OK with what I'm saying? So what it does is it hybridizes those orbitals. How many orbitals will it hybridize? How about that? Two, because it needs to make two bonds. So it's going to hybridize with one. It's one 2s and one of its two p's. So in other words, it's going to make two sp orbitals, right? Because as many as you hybridize is as many as you get out. As many as you stick in the blender is as many you get out of. So those are your sp orbitals. And they're called spy, because we use one s and one p orbital to make them. It's also still got its two p orbitals that we didn't use, that are still higher in energy. So when we fill this using all the various rules of filling electron orbital diagrams that you know, we should get those two electrons now being split up into each one of those sp orbitals. Is that OK with everybody? And then, of course, what will happen? So now we've got, well, let's drop it. We've got those electrons split up like that. And chlorine, if you want to think about the best for theory, the chlorines are still using their three p orbitals to do this. So if you want to think about it in these kind of hybridized orbital fashion, you've kind of got this sp orbital. And I'm just going to show one side of this, OK? But it's one electron like that. And then you've got the chlorine closer, so we don't get any perspective questions. So chlorine's got its p orbital that I can combine with there. And then the other side does the same thing that we talked about with this one. So what's the bond angle? So what's the bond angle? 1-8. You didn't even have to really figure that out that way. You know that once you are sp-hybridized, you've got a 1-8 bond angle. Remember we talked about that? So sp-3 is about what? 109 and 1 half, right? sp-2 is what? You guys remember? 120. And sp is 1-8, right? Yeah, do you have a question on that? I'm just going to ask it before we can do a chart where we get in class. Yeah, well I'm going to try to record all of them, everyone that we did in class, OK? Yeah, so hopefully we'll get them all in. Any other questions on this?