 Okay, so what I'm going to do is we built Zinx electron diagram, is everybody okay with that, right? So here's Zinx electron diagram. What we're going to learn now is which electrons are removed when you're making ions, okay? So remember what Chromium and Copper did where they took that S electron and moved it up into the Ds to make it more stable, the atom itself more stable. Well, in fact, there's a reason for that because the D orbitals, once they're filled, they become inner electrons. And you guys know that from calculating inner electrons, okay? So what you'll find is Zinc has an ion that we've used quite a bit in lab already. It's the Zinc 2 plus ion. It makes sense why it's 2 plus, okay? Because once the 3D orbitals, like we're saying, are filled up, they actually become inner electrons, okay? So once all this is filled up, the 4S orbital actually becomes higher in energy than the 3D orbitals, okay? So what happens is when we make the Zinc 2 plus ion, the electrons that are being removed are not the 3D electrons, not this electron and this electron, but they're actually the 4S electrons, okay? So the S electrons are removed before the D electrons if you're filled up, okay? If you're filled up D-wise, okay? So if I wanted to draw the electron configuration of Zinc 2 plus, it would be something like this. And again, some people would rather you put the 4S up here. Since you guys are in Gen Chem, we're just going to deal with it being the same way we just know that the 4S are in. This is not a rule I made up to make it harder on you guys. This is the way atoms behave, okay? So we fill up exactly the same way. The electrons that we lost, right? That's what the Zinc 2 plus ion looks like, okay? So again, once the D-shell is filled up, okay, it becomes more, or the D sub-shell fills up, it becomes more stable than the S previous, too, okay?