 Okay, so let's start doing the nitrogen in this hydrogen cyanide molecule. So we just did carbon, so you can watch that last video. Now we're going to do nitrogen, the same thing, okay? So what do we have to do first when we're doing this hybridization, showing the hybridization? First we have to show the what? The valence. Atomic orbitals, so the valence electrons in the atomic orbital, right? And what do we say we want to do nitrogen, right? So what are the valence orbitals? We have five. Five electrons, but what are the orbitals themselves? Two s. How many? One. One. Two p. How many? Three. Three. And then you said valence electrons? Five. Five. They're going to fill together. They're very good. One. Two. Three. Very good. Okay? One, two, three. That's five. Everybody cool with that? No. Okay, so we can do this in a number of ways, but we've drawn out the structure here. What is the hybridization for that nitrogen? SP. It's going to be SP, right? So we know it from the electronic geometry. We know it that it's a triple bonded nitrogen. We can think of it a number of different ways, okay? We know that it's making two sigma bonds. That's probably the best way to think about it going forward from here, okay? But if you need to go backwards, you can do it the other way, kind of the check off ways. Okay? So what are we going to do? We're going to mix them up or hybridize. What did we say we're going to make over here? SP. SP. So how many SP orbitals are we making? Two. Two. How do we know there's two of them? One S and one P. Yeah, because it's SP means that the one S and one P got mixed up, right? So how do we depict that over here? Remember, we like to draw the box around them, like that. So we're having the one S and the one P. So let's go ahead, put those there, and what happened to our other two P's over here? Nothing happened to them, right? Did they get stuck in the blender? Uh-huh. Okay, so we're just going to put the P up here, and if you want to write two P, that's fine too. So now what are we going to do? Let's draw our electrons in. Okay? So, one, two, three, four, five, okay? These are relatively close in energy. I know we're drawing them far apart, so that's how they're going to feel in this thing, okay? So if you look at this, how many SP bonds should nitrogen be able to make? One. One. Does it make one SP bond? With what? Carbon. The carbon, right? What orbital and carbon is it making it with? The SP orbital and carbon, right? Do we have an overlap there? It's an SP. We're going to show that, and if I have enough room on camera, we'll show it. Maybe I'll erase this side, if I don't. So this is the SP carbon orbital overlap, right? What is this here? It's the lone pair, okay? And what would these two do, that we're going to make the pi bonds, okay? So now I want to show that orbital system, kind of like what we did in class earlier today. Is everybody okay with us doing that? Okay, so it doesn't look like I'm going to have enough room to put it over there. So would anybody be too displeased if I erase this side? Okay. You would be displeased? What's up? If you don't know there are triple bonds, you know there's triple bonds, so you put the SP. If you don't know that, how can you know it's SP? How many sigma bonds is the carbon making? The carbon itself, how many sigma bonds? Two. Two. So you know you're going to make two sigma bonded bonds. And everything else is a pi bond. Okay, that's how to do it. Okay, so think about that, try some, and then come back and see if you're having trouble with it. Okay? Okay, so now let's draw the entire orbital system. Okay, or at least around the... Well, we could draw the entire one because this is small. Hydrogen? Hydrogen? So we're still... Should we say hydrogen has what orbital is it making the bond with? The SP of carbon. The SP of carbon, but what is the... The S orbital. The S orbital, right? So it looks like that, right? The SP orbital, remember, it kind of looks like a little bit S character, a little bit P character. So I'm going to kind of draw it. And you don't have to be super exact with these things. So this is what kind of a bond would you call this, say? Well, it's a sigma bond, right? That's a sigma bond. Okay? Then we're going to show the next one, right? So the next sigma bond is made up of a what? Two SPs. Two SPs. SP from a carbon and SP from a nitrogen. So remember, the little lobe is the anti-bonding orbital. That's another sigma bond. That's another sigma bond, yes. A little between the carbon and the nitrogen. So we made a sigma bond here. And a sigma bond here. And then, of course, we've got the other SP. What's it doing? Here. The lone pairs. Yeah, the lone pairs are over here. And then what else do we've got between these carbon and nitrogen? The two high bonds. Yeah, the two high bonds. And we get those from the what orbitals? The P orbitals. So... Oh, sweet. Yeah. And then there's the other P orbital. So it gets kind of cumbersome. So now we're going to say, OK, so remember, that's a half and a half pi bond. So half, half pi bond makes one full pi bond, right? Right. Yes? Are you going to ask us to draw this one? So a scan tron? Not on a scan tron, no. But if it were a multiple choice, you may see something that looks like this, OK? This is in a very easy multiple choice question to actually put a bunch of different structures on the piece of paper. Yeah. Are you going to have bonus questions? Potentially. Don't count on it, though. OK, Kim, should we show the other pi bond? Do you have any questions? Those are the two pi bonds? Those are the two pi bonds. Yeah. So it's not four bonds. It's two and two, but they're each half bonds. So two pi bonds are two sigma bonds. Yeah. And the whole of the structure, right? Of between the carbon and nitrogen, there's only one sigma and two pi bonds. So a question you're asking about atomic orbitals would be strictly just what we pulled from the periodic table. Yes. Like the orbital would be the hybridization. Uh-huh. Yes, you have to show the hybridization or the rehydration. Depending on if it went from, like, what we were talking about. Yeah. Something like that. Any other questions? OK. So that's a pretty detailed one. And we did really well. I like those questions. We cool? OK.