 OK, so like I was saying, we did the super oxide earlier this morning, molecular orbital theory. So we're going to take the atomic orbitals and make the polyatomic ion that is peroxide, OK? So if you guys recall how we do that, so I'm just going to assume you do recall this and I'm just going to talk, OK? So if you recall, we used the valence electrons of the two atoms that we're using, or in this case, the two ions that we're using to combine to form the polyatomic ion, OK? So if we think about the valence, or let's just start with what two ions are we using, right? So this is O2 2 minus, right? So what can we use? O minus, right? And what would be the other one? O minus, right? Or we could use O and O2 minus, something like that, if you want to think about it. I'm just going to use O minus and O minus. Is that OK with everybody? So we'll do O minus here. And if you remember, the valence shell, right, has the three P's and the one X, right? So what is this? This is the two S, and these are the three two P's, right? OK, so let's go over here, and hopefully I'm riding it far enough away, right the other O minus. And it's going to have those same four bones, OK? Is everybody OK with what I've done so far? OK, so now what do I need to do? I need to put electrons in my orbitals. Is that correct? OK, so how many electrons would O minus have to put in those orbitals? And how would I figure that out? Periodic table, and what would I do? Count up. It'd be 6 plus 1. So 7. Where do I get that 1 from? Because it's O minus, right? So there's going to be 7 on this one and 7 on that one. So they're going to have the same atomic orbital construction, right? So remember all your orbital-filling rules, right? So 1, 2, 3, 4, 5, 6, 7, like that. You OK with that? OK, and then we're going to have the exact same thing over here, right? So 1, 2, 3, 4, 5, 6, 7. And if you remember, some of the two P's feel, not feel, like touch, but feel weird, right? Oxygen is not one of those, OK? So you don't have to worry about remembering the switch. We'll switch it. OK, so let's build our molecular orbitals now. What is this one down here called? Do you guys remember? Sigma 2x. Good job. What's this one up here? Sigma star 2x, right? Is that right? And then so what's going to be next? What's down here? No, sigma. Because this one isn't a weird one, right? So sigma, you would expect the sigma is to form first. Yeah, it's going to be the sigma 2. And we'll write these ones are the what? And these ones, what is this one? Very good. And then, OK, so let's write those in. So what did you say this one down here was? 2D, this one, this one? You can help me out. This one? What is this? 5 stars. Very good, yeah, 5 star 2p, this one? 5 star 2p. What's this one? Sigma 2p. Sigma star 2p, OK? So I'll let you guys write that down. Now what do we do? We just fill up like normal, right? OK, so how many electrons do we have here in the bottom part? 4, right? 2 from here and 2 from there. So that's going to fill up both of these orbitals, right? So 1, 2, 3, 4. How many do we have here? 1, 2, 3, 4, 5. Plus 5 is 10, right? So 2, 1, 2, 3, 4, 5, 6, 7, 8. 9, 10, like that. Is everybody OK with that? So would you expect this polyatomic ion to be stable enough to be formed? Why would you expect that? Well, that's the best way. That's the statement you want to make. But we do. Yeah, you got to figure out what the bond order is, right? So that was what was said in the back. But we know that peroxides exist, right? That's something that we just studied. So we should hope that we get a bond order that's greater than 0, right? If we don't, then we messed up somewhere, if that makes sense. So you would expect both the superoxide and the peroxide to be a bond order greater than 0. Does that make sense? OK. And the superoxide we figured out was, in fact, I believe it was 1.5, which I remember correctly, OK? So let's figure out what this one is. And how do we do the bond order? Well, do you guys remember what the bond order equation was? 1.5. Yeah, very good. So how many bonding electrons? 1 and 2, is that correct? And anti-bonding, how many? 6. 1, 2, 1.5 of 2, 9, 8 minus 6 is 2, it's going to equal what? 1. So bond order is 1. Does this thing exist? So is it stable? Yeah, it exists. Would this be attracted to a magnet, the peroxide? No, very good. No, why not? I don't see any of our molecular orbitals that are half-filled. So just like Reggie says, since there's no half-filled shells or no half-filled orbitals, it's not going to be attracted to any magnets, OK? So the last thing I want to do, then, is to figure out, well, what is the molecular electron configuration, or the electron configuration of this polyatomic ion? Can you guys help me out in drawing it out? So if you remember with these ones, we put parentheses around, so what would we start with? So again, this is just for the valence, OK? So you could put the sigma 1s star first, but we'll just do the valence electron configuration, OK? So sigma 2s 2, right? What would be next? Sigma star 2s. Help me out, guys. 2. Next? Yeah. Sigma 2p 2 pi 2p what? 4. If you guys aren't knowing this, then you're going to have to know this, remember, OK? So this one is going to be what? Pi star 2p 4 and is that it? Yes, that's it. So that would be the valence electron configuration. If we wanted the full, we would just put, that would be the full electron, so the valence. So the valence is all the valence. Does that make sense? Any questions? Any more questions that you would like answered about something like this? So remember, you want to be able to do this with both peroxide and the superoxide just to confirm that these kinds of ions can exist. Does everybody understand what I'm trying to say? OK, one. So I'm going to kill this unless anybody's got a final word. OK?