 Okay, so what we're going to do is we know molybdenum is one of these anomalous electron configuration atoms, right? So what we're going to do is predict what molybdenum should be and then figure out what it is, okay? So help me write the electron configuration for molybdenum if you don't mind. So 1s2, 2s2, 2p6, 3s2, it's next, 3p6, what's next? 4s2, 3d, very good, 10, 4p6, 5, s2, 4d, 4 is what you would expect it to be, okay? That's what you would expect it to be, right? The thing is, is when you have these half-filled B orbitals, molybdenum and chromium will act weird, okay? So what they'll do is they'll take one of their S electrons in the previous S orbital and add it to the D electron subset, okay? So instead of being the 5s2, 4d4, what is it going to be? 5s1, 4d5, okay? So let's go ahead, so all of this is going to be the same. So if we wanted to, we could write, what, Argo, sorry, chromium, I have these anomalous atoms in my head. So let's go ahead and, well, I don't know if we have enough room, but we'll try to build the electron configuration on, or the electron diagram on this board, okay? So where do we start? The 1s way down here, and the 2s, and the 2p, how many orbitals come out? Three. And then what's next? The 3s1, 3d, 3 of them, 4s, how many? 5d, what's next? 4p, 4p, and then 5s, and it looks like I'm going to have two of these here, too, and then 4d, and is that it? So let's build it like it should have been if it added, if it added in correctly, okay, through off valve, harness, and collie inclusion, okay? So it should go 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 13, 14, 15, 16, 17, 18, 19, 20, 21, 22, 23, 24, 25, 26, 27, 28, 29, 30, 31, 32, 33, 34, 35, 36, 37, 38, 39, 40, 41, 42, right? So that's the way it should build. Is everybody okay with me doing all of that? So remember, this is increasing energy here. But remember, these anomalous ones are more stable when they have an either half-filled D subset or a full D subset, okay? This one's one away from having a half-filled, so what it does is it actually will take that second 5s electron and move it up to that D orbital there, okay? So let's draw the new configuration or the new diagram, I mean? So that's what it looks like. Everybody okay with that? So you've got to remember these 5 atoms that do that. That's the function of the 5s chain. I mean, so the thing is, is the reason it does, we'll talk about that in a second, but once you fill up your D orbital, the S orbital actually is higher in energy, okay? But let's, since we have molybdenum up here, let's just do silver, because it's really close to molybdenum and we can kill them both with one stone, okay? So what should silver's condensed orbital diagram look like? I mean, condensed electron configuration, so this is molybdenum, right? What should silver's look like? They are 5s, well, that's, well, okay, so what does it look like? Okay, let's say that, 5s1 or D10, right? But if we did what it should, like you were thinking I was saying, it would have been 5s2, 4d0, right, okay? But, so it does the same thing as molybdenum, right? But what do we do? We just put those electrons in that higher orbital, so 1, 2, 3, 4, 5, like that, okay? So to answer the duke's question now, what happens once we fill that up, these s electrons become more energetic than the 4d's, okay? And in fact, it happened down here, too, we just didn't indicate, okay, so that's what happens every time, okay? So when you have a half-filled d subset or a full-filled d subset, they become very stable, okay? So it induces these ones that are very close to it, to make a half or full-filled one, is everybody okay with this? Okay, good.