 Okay, so let's attempt to do this problem. It says, pyridoxal phosphate, a close relative of vitamin B6, is involved in a large number of metabolic reactions. Tell the hybridization and predict the bond angles for each non-terminal atom. In order to figure out what the hybridization is, you're going to have to figure out how many electron groups does each one of these atoms have a right fit, okay? So if you are good at that, then the hybridization and the bond angle come directly from that information, okay? So non-terminal, why don't we go ahead and expand like this portion, this portion of the structure, put our long pairs on there as well, because that really helps, okay? So I'm going to expand this and say this is a methyl group, so we can really see our terminal relative to our non-terminal atom. And then remember here, this is a CH2, a methylene CH2 with two hydrogens on it, okay? Do we need to expand that part portion of the structure too? Should we do it? Okay, we can do that. And then recall, each of these is a carbon 2 here in this ring, okay, the aromatic ring. And each one of those carbons has one substituent off on it, okay? So here, that substituent is what we call a methyl group, a hydroxyl group, right, aldehyde, okay, this big R group. And then this one you see it doesn't have anything there, but it's got one, two, three bonds to it, so it must have a hydrogen there, okay? So let's just identify that just to make sure, because this is what chapter one still, right? So we're kind of learning how to do this stuff, okay? So is it okay that I don't put the C's within there, is that fine? Okay, wonderful. So the next thing we'll do is go ahead and put our lone pairs on everything, okay? Do you already have it written on there? Okay, so let's do and do it together, okay? So remember, if your carbons are fully saturated with bonds, you know? So like if we look at this carbon, it's got four bonds on it. This carbon has got one, two, three, four bonds, okay? So that's not going to have any lone pairs, okay? So if I look at all of my carbons there, they all have four bonds on them, okay? So really what we're looking at now is the hetero atoms to see do they have lone pairs or not, okay? So can you help me out? Should nitrogen here have a lone pair? Yeah, how many? Two. Well, one pair of electrons, right? Yeah, so two electrons. Okay, so we call that one lone pair, okay? So what about this oxygen here? Two lone pairs. Very good, yeah? Okay, and I know it said all the non-terminals, but let's go ahead and look at, this would be kind of a terminal oxygen, you know? But let's look how many, so two lone pairs again. And again, I'm trying to draw them in such a way as to show the directionality of these lone pairs. So really kind of, hopefully we'll help you out at least down the road when you really start to understand this stuff. Okay, so I don't see any more hetero atoms until I get to here, right? Is that how many lone pairs are there? Two as well. This one up here? It's two. Two, very good. What about this oxygen here? It gives you a clue with that negative charge. It's given one away, so it should only have, it should have five electrons. Well, it's gaining one if it's- I'm sorry, so it's such a three lone pairs. Three lone pairs, yeah, very good. So are you doing the formal charge equation backwards in your head? Yes. Okay, wonderful. Yeah, that's good. Okay? And then this one? And then this one? And then this one? It's two lone pairs. Two as well. This one up here? It's two. Two, very good. What about this oxygen here? Okay, wonderful. Yeah, that's good. Okay? And then this one? Also three lone pairs. And what about the phosphorus? Can you do that one? It's kind of one of those, remember, the weird atoms that expand their valence? Should I- should I give you a clue? Okay, this, if you look, phosphorus has five valence electrons. You can see they're all being used to bond there, so it's not going to have a charge. So remember, five minus zero minus one half of ten is going to be five minus five, so that's going to be zero. Okay? If you want to go through that slower, just watch the video again, okay? So is- are you- we cool with the electron? Yes. Okay, wonderful. So now what we want to do is look for the electronic structure around each of these atoms, okay? So what you'll find is the amount of electron groups kind of tells you what the bond angle is, and from that bond angle you can get the hybridization, okay? So let's just start here, because it wants us to do all non-terminals, okay? So we'll start here. How many electron groups does that carbon have around it? Do you remember what we considered electron groups? Yeah. So one bond was one, double bonds was just one electron group, triple bonds was just one electron group, and lone pairs, one electron group, okay? So this has four single bonds around it, so how many electron groups? Four. Four, right? So with things with four electron groups, what shape do they become? Tetrahedral, okay? 109.5. Yeah, 109.5, so we've really skipped over the hybridization part, so once we say tetrahedral, once we say that electron groups, there's four of them, that's sp3 already, okay? Three, and what was the other thing I wanted, the bond angle, right? Yeah. Okay, so something with four sigma bonds is going to be what? 109.5. 109.5, yeah. So let's go to this carbon here, okay? So how many electron groups does it have around it? Four as well. So what did we say? Single bonds? Double bonds count as one, triple bonds count as one, and lone pairs count as one, okay? So it's got? Three. Three, okay? So if it's got three that approximates what bond angle? Just the angle number. Oh, angle is 120. 120, right? So that's going to be trigonal planar. Trigonal planar. Trigonal, right? Trigonal. Okay? So it's nothing crazy. You want to remember three trigonal, okay, that really goes together very nicely, okay? So if we've got three groups, right, so this one had four, right? The bond angle here was 120, what did we say that hybridization is, sp2 always, okay? So let's look at this one here. Is there anything similar between that one and that one? That's the exact same. So do we need to go through the analysis of that one? Yeah, that one. Okay, I'm just going to write the same thing down, okay? So in fact, I'm just going to write a little arrow there, okay? Because that one's also sp2 and 120 degree bond angle, okay? What about this one here? It's the same thing, right? Same thing. So let's put another arrow there. What about this one there? Up at the top. Sp2. Sp2, right? So same thing. And what about this one over here on the edge? The same. Same, okay. So now let's look at that nitrogen that's on that ring. How many electron groups does the nitrogen have around it? It's three as well. Three as well. So what do you think the hybridization is going to be? So that's a sp2. Sp2 as well. Here, when we're talking about bond angle, right, we're going to talk about the angle between here and here because this is not a bond, okay? Because it's got a lone pair, oftentimes we'll think, well, it's going to crowd those two bonds in a little bit. But when you're in one of these aromatic rings, it really doesn't deform the shape as much, you know? So we're going to say this is 120 as well, okay? If this were an atom in a non-cyclic structure, an acyclic structure, or I guess more so, if that structure weren't aromatic where they had alternating double and single bonds, then it would deform the bond angle and it would kind of collapse it a little bit, okay, like we've talked about before in class, okay? So we're going to put, is that all right, just a little arrow there? Okay, so let's look at this one here. So how many? It's also got three. Three. So what is it going to be? That car is the sp2. The sp2. And what's the bond angle? 120. I know it said only the non-terminal ones. Let's look at this one though. What do you think? How many bond, or how many electrons? So it's got three as well. Three as well. Three as well. So what's the hybridization? That hybridization is sp2. Sp2. We can't name a bond angle though because there's no bond to bond, right? When we started a bond and go to the next bond, it's the same bond, so we can't do a bond angle. But yes, it is sp2, okay? So you can do, yeah, you don't have to worry, yeah, don't worry about that. As long as you're trying, that's all right. So, four. So that's going to be sp3. Sp3. With one of 9.5 angle. Let's look at this one over here, this oxygen over here. How many electron groups are there? It has four. Four. So what's the hybridization? Sp3. Sp3. What's the bond angle of this one then? Four. Four electron groups. So what should it look like? What should it approximately look like? Should be, but what do electron lone pairs do? They make that angle smaller, okay? Don't make up new rules. Do the rules that I taught you, okay? So, if this is smaller than 109, is it going to be 180? No. Okay, so let's try again. So what do you think it's going to be? Do you remember those other bond angles that I gave you to remember? 107. Okay. Okay, what was the other one? Well, so how many electron groups did you need for that? I don't know. Okay, then you got to remember, we'll just, I'll just give it to you. 104.5. 104.5, okay? Let's go to this one over here. Okay, so how many electron groups? Four electron groups. Okay, so what's the hybridization? Sp3. Sp3, what's the bond angle? That one also be 104.5. It is also 104.5, okay? Remember, I'm asking questions, you're giving me some sort of answer. So yes, you're supposed to say that is 104.5, right? Because we just went over one that was exactly like that. Recall. Okay. Again, we can say on this one, we can say it's sp2 hybridized, but we can't give a bond angle. That's why they're trying to tell you don't do the terminal one. So let's not worry about those oxygens there, because they do act a bit strange, okay? But this phosphorous there, right? What is the amount of electron groups around that phosphorous? Four. Four. So what's the hybridization? It's an sp3. Sp3. So what's the bond angle going to be? No, try it again. I'm sorry, sorry. 109.5. 109.5, okay? So are there any questions on that particular one? We could even go back through these and say, what is the molecular structure, you know? We could say, well, this one's tetrahedral. This one's bent, you know? This one's trigonal planar. Trigonal planar, trigonal planar, trigonal planar, trigonal planar, trigonal planar, bent, okay? Tetrahedral, bent, tetrahedral, okay? Are there any questions left on that one? Okay, wonderful. We're going to kill it.