 So when we're building like a molecule like this So I guess this is just what I found like Evan was building over there So it's just not any any sort of molecule that we came up with on the piece of paper He was just building stuff. But anyways, this molecule is called a diamol Let's let's so let's look at the ball and stick Version of it and let's try to draw its Lewis structure We should all be able to. Okay, so when we're drawing Lewis structures or when we're looking at ball and stick models Usually what you'll see is that carbon atoms are black. Okay, and the red atoms are oxygen. Okay In this case, the yellow atoms are hydrogen. Usually they're white. Okay, but what? Usually yellow is solar, but you can tell it's hydrogen because it only makes the one right but anyway, so if we look at it, we should be able to draw this molecule so John see see like that and we've got So we're looking at it and this sort of configuration there as if it's standing like that We've got this atom this hydrogen atom this oxygen atom this carbon atom This carbon atom this oxygen atom and this hydrogen atom all in the same plane Does everybody see that so we should if we're going to draw it. We're going to draw it like that. Okay, so the two carbon atoms It's the oxygen atom there Over here is the other oxygen atom right there. Does everybody see how we're doing that here? hydrogen atom here hydrogen This hydrogen atom is coming towards us right here. Does everybody see that so it's this one So let's draw those two hydrogen Remember the wedge is how we show something coming towards us, right? The way is how we show something coming towards us right back What about these two hybrogens here that are kind of harder for you to see right but because they're going back And how do we do those? So that's the molecule that heaven just built right, but we're missing the lone pairs on the oxygen remember You've got to remember your lone pairs if you can't remember your lone pairs You could always do that fish hook thing that you Build the molecule one atom by one atom, but it takes a long time the way I would like you to think about it is to think that piece looks a lot like water, right And what's happened is we've replaced that hydrogen with all of this stuff over here So since that looks a lot like water, you should expect that that oxygen's got those two lone pairs Okay, so think about it that way another way you can think of it is if oxygen is Uncharged, then it's got two bonds and two lone pairs. Okay Another thing we could talk about is the molecular geometry around these atoms, okay So ladies and gentlemen, if we're talking about molecular geometry, okay We're talking about what is the geometry around the I've been saying this the central half Okay, well in this case, what is the central atom? There's actually a bunch of them. In fact, there's four central atoms, okay So what you can do is say, what's the geometry around this atom? What's the geometry around this atom, this atom, and this atom? Okay By geometry I'm talking about we could talk about the bond angle, okay So hopefully you guys could figure out If I asked you, what is the bond angle there? What would it be? 104 and a half, yeah, 104.5 and how'd you figure that out? It's greater than 90 Well, definitely that but it looks like water, right? That's the bond angle of water is 104.5 The other thing you want to think of is if you got something that's got two lone pairs Or two bonds and two lone pairs, it's going to be about one of 4.5. Okay What about here? What's the bond angle here? What is it? One on nine and a half, yeah And how'd you do that one? Because it looks a lot like methane, right? It looks like methane Is that we've taken those two hydrogens and put an OH group there instead and this whole thing Instead, okay, what about the bond angle here 104.5? So you see how you're getting this, right? So it's all these patterns that you're looking for so 104.5 Okay, what are some of the other things that ask it? It says molecular geometry It also says electron parachute. Okay, that means what is the geometry of the electrons? Okay, so Just like around the carbon, right? There's four pairs of electrons around this carbon. Do you guys see that? Four pairs of electrons Just like there's four pairs of electrons around this oxygen, right? Does everybody see that? So if you've got four pairs Your electron geometry is always tetrahedral because they still want to be as far apart from each other as possible Okay, so the electrons are tetrahedral So if we wanted to draw water just to emphasize this, right? So water looks like Let's draw the hydrogens Like it as if I think I have water built So Let's pretend we're looking at water like this, right? So that's how we've drawn it right there But remember electrons when they're paired up they hate other electron pairs So they want to be as far away from each other as possible So we could think of the electron pairs As being in the plane there if you will that this is out of the plane. Okay, so just like this Is front and back, right? It looks similar To water except it doesn't have those two months, right? Okay, so water has lone pairs Is the same and both Is everybody okay with that the electron geometry is the same and we asked what's the electronic geometry? Well, this one's clearly tetrahedral. So since this one's very similar to that. It's tetrahedral as well. Okay, so They're both tetrahedral Molecular geometry is what you already know, right? Molecular geometry is just showing the geometry of the molecule itself, right? So if you imagine yourself as being a little person and not being able to see those electrons, right? You can only see those three atoms, right? So the molecular geometry Is going to be what for this one big, right? Very good. And then this one is going to be tetrahedral