 I changed my mind. Let's build NCL3. OK, so NCL3. So N metal or nonmetal? What's that? N metal and nonmetal, right? CL? Nonmetal. So is this going to be a covalent or ionic compound? Covalent. OK, so already we've started that. So how do we build something like that? What we do is we draw the Lewis structures of the atoms that are involved in this compound. The other thing we've got to think about is which one is going to be the central atom. The central atom is the one that's going to be able to make the most bonds. So if you think about chlorine, chlorine is only missing one electron. So it can only make one bond. Nitrogen, on the other hand, is missing three electrons. So it can actually single bond to three different atoms. So everybody OK with what I'm saying before we draw it out? OK, so let's just picture these atoms kind of in that array with nitrogen in the middle. So nitrogen's going to be there. Draw its Lewis structure. One, two, three, four, five. Why do I draw them like this? So it can have spaces on each side to grab each one of those quarens. But quarens, I'll draw them normal, like I'm supposed to do. One, two, three, four, five, six, seven. So one, one, two, three, four, five, six, seven. I keep switching the sides because I keep wanting to end up with a space closest to the range. Let's see if I can do it right this time. One, two, three, four, five, six, seven. OK, so now what are we going to do? Remember our fish hook arrows, OK? So those are the arrows with like half a little arrow head. So instead of the electron transferring going from the chlorine to the nitrogen, we're going to have a meat in the middle. It's kind of antiquated, late of drawing it. But it's good for you guys to see for the first time when you do these kinds of things. If you want to think of them all as stuck to each other, like really stuck to each other, you can draw them in the old way of drawing molecules. So now you can see this is a good way of drawing them for you guys when you're starting off, because you can put your hands over each one of these atoms and say, OK, that thing's got a full octet, right? See that? That one's got a full octet. That one's got a full octet. That one's got a full octet. Is everybody OK with that? Again, that's antiquated, meaning old fashioned. So we're going to draw it the normal way, with bonds represented as lines. And if you watch these videos, I actually did one more step. We're not there yet. I used Vesper's theory to actually show why this kind of is in that pyramid shape as opposed to a t-shape. But the pyramid is the way it's actually supposed to look. But we haven't gotten there yet. So for you guys, if you could draw it to that, specifications, you're good. So is everybody OK with each one of these atoms having a full octet? And why this is a covalent as opposed to an ionic compound? Everybody OK with that? Any other questions? OK, cool.