 Okay, so guys, let's draw now the electron configuration for this anomalous filling, um, Adam Cromie, okay? So, um, I'm going to, hopefully I have enough room on this small board to draw the entire electron configuration, or the entire electron diagram is what I really want to draw. Um, so we're going to start down here with the 1s, 2s, so I guess the first thing we should do is, what is Cromie and his electron configuration, let's draw that out, so, or what is what we predicted? 1s2, 2s2, you guys can help me if you want, 2d6, 3s2, right, 3d6, 4s2, 3d4, okay, that's a little bit predicted to be, right? Okay, but in actuality, it's not, and let's just show how, what it actually does, okay? So, 1s2s2d, that's 3 of them, 3s1, 3p, 4s, and then 3d, okay, is everybody okay with that orbital diagram? So now let's fill it up, okay, remember, off valve principle, start at the bottom, all a exclusion principle, the second one has to go upside down. Huns rule, if we have degenerate orbitals, we go on one at a time, okay, so we, the last four, one, two, three, four, okay, so remember, I told you chromium is one of these anomalous people. So, what it actually does, and the reason being, like I said, is because half field d orbitals subset is better than a non-half field, okay, or more energetically stable, okay, so what chromium will do is it will take one of its 4s electrons, so one of these two electrons and move it up into that 3d orbital, okay, to make it half filled, does everybody understand what I'm saying? So, again, it just is more stable to do this one, okay, and that's why, remember, that's why anything happens in chemistry, it's because of stability, okay, so what it'll do is it'll take this 2nd electron and move it to there, okay, so let's just show that, like that, and remove this from over here, so it looks like that now. So notice, it didn't, it kind of is anomalous, right, it doesn't fill using the off valve principle, okay, why, because the 4s isn't all filled up, so now let's draw the real electron configuration for chromium, okay, so most of it's the same, right, so you guys can help me if you want, 1s2, 2s2, 2p6, 3s2, 3p6, what is this going to be now, 4s1, and this one, 3d5, okay, copper does the same thing, okay, copper does the same thing, molybdenum does the same thing, silver does the same thing, and gold does the same thing, okay, so let's do copper's configuration now, okay, let's just, just to show, right, this is not the right configuration for chromium, this is the right configuration for chromium, okay, so instead of chromium now let's look at copper, okay, so can I erase these electron configurations up here, anybody have a problem with that, okay, so instead of chromium we're going to look at copper now, so let's just erase these, okay, so we're at 4, so let's draw the electron configuration that copper should be first, okay, so what is it, 1s2, 2s2, 2p6, 3s2, 3d9, 3d9, does everybody understand that, just by looking at the periodic table, right, okay, so we've got up to 4s1, so we've got to put our 4s2 in there now, right, and then put our 3d9, so let's do that by using all of our rules, right, off balance, poly exclusion, so 1, 2, 3, 4, 5, 6, 7, 8, 9, like that, so that would be copper's normal electron configuration, but copper is one of these anomalous filling elements, right, so what is it like to do, well because it's one away from having a full D shell, and remember when you have a full D shell you become very, very stable, so what it does is it takes that 4s electron and moves it up into it's 3d subset, sub-shows, okay, is everybody okay with that, so let's just show that here, and now let's show what it's real electron configuration is, so 1s2, 2s2, 2p6, 3s2, 3p6, what is this, 4s1 and 3d, okay, is everybody okay with doing this, okay, so again you've got to remember those 5 atoms that do this, or just remember that tungsten doesn't do this with that W, right, questions on this, can I kill it, okay.