 OK, let's start that again. So this time, we're going to talk about one of these odd-filling diatomic, polyatomic ions. So here, we're going to use molecular orbital theory to figure out, well, what's the bond order of this N2 plus? Does it exist? All of that stuff. So the one thing, again, you want to remember about the atoms boron, carbon, and nitrogen is that in their two P's, they make their pi bonds first, OK? So N2 plus, you're going to have N combining with what? N plus, right? Is everybody OK with that? So down here, and you'll see why I don't like to do these, because I'm too tall, I think. So 2S down there. 2S down there. Remember, we're only using the valence electrons. So this is the sigma 2S orbital. This is the sigma star 2S orbital. So just like how we did lithium and beryllium and all of those things. Up here is where we have the weird stuff, OK? So now we're doing the two P's. One, two, three, like that. One, two, three, two P's. OK, so what did we say? It makes the pi bonds first, these weird ones. So one, two, and the sigma bond next, like that, OK? This should actually work. These aren't the easiest thing to draw on the board. OK, but now, up here, it does pi and then sigma, like you would expect, OK? So we call these ones pi 2P, pi 2P, sigma 2P, like that. This one's called, what do you think? Very good, pi star 2P, pi star 2P, and this one? Sigma star 2P. 2P, OK? Very good. Is everybody OK with that? OK, so now let's fill in what we got here. So how many valence electrons does nitrogen have? Just n. 5. 5, right? So one, two, so again, off-boub, Hund's rule, polyexclusion, right? So one, two, three, four. What about n plus? How many electrons does it have? Four. Four, right? So one, two, five. So one, what did we say we expected the bond order to be? Well, 1 half less than 3, right? Which would be 2 and 1 half, right? If you look at this, already you should be able to tell that it's going to be 3. And how do we know 3 to start off with 3? Because from Vesper theory, right? We said when we build nitrogen and Vesper. So anyways, let's draw the, well, let's do the bond order first, OK? So what's the bond order? electrons minus the anti-bonding electrons. So 1 half. How many bonding electrons do we have? One, two, three, four, five, six, seven, OK? And you could have just done these ones, but make sure you just do all of them in the valence, OK? So seven minus anti-bonding. Well, how many do we have? Seven minus two. And that would give you the same as five. Bond order of 2.5, like we were expecting, OK? Would you expect this molecule to exist? Yeah, definitely. Would this be a relatively strong bond or a weak bond, do you think? Pretty strong, right? Pretty strong, 2.5. Is it attracted or not attracted? It is attracted, so it's diamagnetic, right? So it's got the one unpaired electron there, OK? A lot. Yeah, I mean, that's all it needs, though, is the one unpaired electron. And what you'll find again is that this is one of those reasons that you need to kind of compare molecular orbital theory with Vesper theory, because Vesper theory doesn't tell you anything about that, OK? It just tells you structural information. Last thing I'd like to do is do the entire electron configuration, OK? Or, yeah, let's do the entire electron configuration. So, OK, so remember stars on the bottom, sigma 1s2, sigma star 1s2, sigma 2s2, sigma star 2, 2e1. Is that all the questions that we had asked before, I think? OK, so any questions on this one?