 So let's try to build superoxide using molecular orbital theory, okay? So remember, when we were doing molecular orbital theory, this was a couple chapters ago, but now we've just introduced superoxide, so we're going to build that. We're only going to be talking about the Bay-Wence electrons, okay? So remember what does O2 minus look like, or what is it composed of? It's going to be composed of O, O minus, right? So we add those two things together, O and O minus, we'll get O2 minus. Is everybody okay with that? Okay, wonderful. So when we look at the atom oxygen in its Bay-Wence shell, its Bay-Wence shell is in period two, or energy level two, right? So it's going to have the 2s and 2p orbitals to fill, okay? So let's write those down. So just the atomic, some more room. Down here, that's going to be the 2s, and these should be at the same level. We're trying to make more energetic than the other one. So 2s and 2s, and 2p, 2p. So all three of those are the 2p. So when we build the atomic orbital, we've got to see how many Bay-Wence electrons each of these atoms, or ions in this case, would have, right? So if we look, one, two, three, four, five, six, right? That's what we would expect oxygen to have. So if we remember our filling rules, one, two, three, four, five, and six, like that. Okay? O minus, of course, has six plus one electron. So it's going to be one, two, three, four, five, six, seven, like that. So are you okay with what we've done so far? Okay, good. So now we're going to build our molecular orbitals. One down here, sigma 2s, sigma star 2s. Now remember oxygen, oxygen, fluorine, and neon, these are the normal filling. They're sigma first. It's not super even, but sigma 2p, pi, 2p, pi, pi star 2p, pi star 2p, sigma star 2p. You guys remember how to build those things? Okay, wonderful. Now what do we do? We just put them in, right? As they would fill, normal. So one, two, so one, two, three, four, one, two, three, four, one, two, three, four, five, six, seven, eight, nine. Okay? One, two, three, four, five, six, seven, eight. Is everybody okay with that filling? Okay, so now let's think of, well, what's the bond order? Okay, so if the bond order, for this to exist, the bond order has to be what? Greater than zero. Greater than zero. So do you guys remember the bond order equation? One half the bonding electrons minus the anti-bonding electrons, right? So we've got one half, how many bonding electrons? Anti-bonding, molecular orbital theory, we can have, okay, which is over. We're going to have here, so it would be one half, three, right? Which would be one point. So that's the bond order. So would you expect this thing to exist or not? Yeah, definitely. Would this be attracted to a magnet? Would you expect superoxide? Why? Because it's got an unfair electron, right? And I guess the other thing we can do is write its molecular orbital electron configuration. Do you want to do that? So let's do that. So for it to not exist, it's the bond order that means zero. Okay? It can only be zero or positive numbers. Can't be negative, okay? So the reason being is because you've got to fill the bonding orbitals before the anti-bonding orbitals. So the least amount of electrons you could have is one, right? So that would be a half bond order, if that makes sense. But you could have a bond order of zero if you had two and two or something. Which would be a non-existent molecule. Yeah, go back, I've recorded a few more of these. Go back and check those out too, okay? This is a more detailed one. But let's write the orbital configuration or the electron configuration. So how do we do that? Well, we just look at what we've got here. So remember in this case we put them in parentheses. So sigma 2S2. Like that, right? Because we've got two electrons in the sigma 2S. Okay? Then what would be next? Good job, sigma star 2S2. Right? And how many do we have in there? Two. Two. Very good. Then next, sigma 2P. How many? Two. And then next, pi, 2P. How many? And you add them all together, so just like you said, four. And do we have more? Pi star 2P. And how many? So that would be the electron configuration. Question? I can talk to sigma star 2P and it has nothing, you don't. You're not going to include it. No. You're not going to include it. It's just like if you were talking about, I don't know, oxygen itself, atom, and you say, well, what about the 3X? Right? You don't say anything about it because there's no electron. It's just represented in the atom. Yeah. Well, it's got that orbital there, but it's just no electron there. Okay? So that orbital does exist. There's just, it's like a house that's not on, it's there, but nobody listens. Any questions about this? This is a good question, okay? Okay, good. Okay. Do you want it on this one? No, okay. So good job, guys. That's all I have for you today. Okay, bye-bye.