 So let's let's try this one guys together. So we just get a beryllium hydride, right? Let's do a different molecule. Let's do carbon dioxide. Okay, so some of you have already done carbon dioxide. What do we know about carbon and oxygen? So what do we know about carbon specifically? How many bonds does it like? Four. And how many bonds does oxygen like that have? Bonds. Good. Two, right? Two. Okay, so how do you think this molecule is arranged? There's two double bonds. So the carbon's in the middle, right? Double bond to an oxygen, double bond to an oxygen. And there's two wrong pairs on each of those oxygens. So remember, they won't shell electron pair repulsion theory, right? So if we've got these electron pairs or these bonds, right? They want to be as far apart from each other as possible. Remember here, we've got the same thing happening. Here, what did we say the bond angle was? Eight, right? Why? Because we've got two bonds and they want to be as far away from each other as possible. What about here? What do you think the bond angle is here? 180. 180 as well, right? Why? Because these double bonds act as one whole bond, okay? So what is the molecular geometry around that carbon at? Linear. Is the molecular geometry. What about the electron pair geometry? Electrons arranged around that effect. Linear. Linearly, right? They're the same. Right? Aren't they the same? That's the bonds. What about here? Are the electrons arranged linearly? What are the, what's the electron arrangement around the oxygens? Trigonal planar. Trigonal planar around the oxygen. So that's the electron geometry. Right? What about the, could you do the molecular geometry around the oxygen? You can't do it. You've got to do a bond to a bond, okay? There's no second bond. But you can do the electronic. See the electronic around the oxygen is trigonal planar. You can do both the electronic and the molecular around the carbon, right? Why? Because you can do an angle from electron to electron if you want to call that an angle and bonds to bonds or whatever. Is that okay? Notice the difference between this and this. So if we wanted to say, okay, let's write this one out. Number of electron pairs for beryllium hydride. Let's write these two out. We'll compare them. So what's the number of electron pairs for beryllium hydride? You can look over that. Two. Two, right? And the electron pairs for carbon dioxide? Four. Four, right? Even though there's two double bonds and each bond double bond consists of four electrons each, right? So you can already see there's a difference, right? So what about the bonding pairs? How many are here? Bonding pairs. Two. Two, right? And of course, we're talking about around the carbon in carbon dioxide. What about bonding pairs around the carbon in carbon dioxide? All four of them, right? How'd you figure that out? You could look at the number of bonds or you could see that there's zero lone pairs, right? How many lone pairs are here in beryllium hydride? Zero. What about in carbon dioxide? We're looking around the carbon, remember? We could do this for the oxygen if you want to. Let's do the oxygen in a second, okay? So this will be the carbon dioxide carbon. How many, oh, what was this? The electron structure, right? What's the electron structure for beryllium hydride? Linear. Linear. And around the carbon, what is it? What about the molecular? Linear. Linear for beryllium hydride. And what about for the linear? Since you guys wanted to do it for the oxygen, let's do it for the oxygen, too. So how many electron pairs do we have around that? Two. How many? Right? What's the electronic geometry around that? Oxygen. Trigonal planar. Trigonal planar? You can't do it because you've got to do it with angle. Does that make sense to everybody? Okay. So you should be able to do these things. If you see, you should be able to see patterns, right? Four or zero, that's almost definitely hard. Four, two, two, five, four, three, one, that's nitrogen. You can see the pattern on the periodic table, hopefully.