 So, let's build the structure carbon dioxide from its Lewis structures, okay? So, CO2 is carbon dioxide, everybody's cool with that, right? So, the first thing we want to do is write the three atoms, okay? So, which of these atoms can make the most bonds? Carbon or oxygen? Carbon. Carbon. Okay? So, that's probably going to be your central atom. And in fact, in this case, it will. So, let's draw Lewis structure of carbon, Lewis structure of oxygen. And again, I'm just drawing these in this particular way because I know how I'm going to bond them. So, how many bonds would you expect carbon and oxygen here? Two. Two, right? Why? Because oxygen needs its octave good, right? Is everybody okay with that? What about over here? Same. What will happen when you do both of these oxygens bonded to this carbon with double bonds? Yeah, so you'll have two double bonds, a double bond here and a double bond here, right? You'll have a full octet on this oxygen, full octet on this oxygen and also like you were saying, only the full octet on the carbon. Is everybody okay with that? So, yeah. You know it's a double bond because there's two of the other oxygens, right? So, there's two spaces here, right? And there's four spaces here, okay? So, let's just put it together and you'll see and see if you'll have that same question, okay? So, remember our fish oak arrows? So, again, if it's hard for you to do this, just go straight from just this kind of structure to bonding, you can do that intermediate thing like I was saying. Like they used to do in the early 1900s. They'll show you the like that, right? Is everybody okay with that? Now I know it looks very strange, right? But you can see 1, 2, 3, 4, 5, 6, 7, 8 around oxygen, right? 1, 2, 3, 4, 5, 6, 7, 8 around carbon. 1, 2, 3, 4, 5, 6, 7, 8 around oxygen. So, again, we want to draw it like a modern person, so that's carbon dioxide. So, some things that we'll learn about carbon dioxide in a little bit, but I'm going to give you a preview since we're recording this thing, is that when you look at the bonds, right, you should realize there's going to be a difference in electronegativity between carbon and oxygen. Is everybody cool with that? Yes, no? Yes. Okay, so yes, right? Which one of these is more electronegative? Oxygen. In fact, it's one of the more electronegative elements. That's one of those three that you might want to remember, the very electronegative ones, okay? So, if I said which way is the negative charge being pulled in each of these bonds, or if you want to think of which way is the partial positive and the partial negative in these bonds, right? So, carbon, when looking at this bond here, is going to have a partial positive and the oxygen will be a partial negative. Is everybody okay with that? Same thing over here, but partial positive and partial negative, there. Okay, is everybody okay with that? And also, the amount of pulling that this negative will have is the exact amount of pulling that that negative will have. Is everybody okay with that? Okay. So, this structure is a linear structure. All of these atoms are in the same plane, okay? They're in a line. Another way to depict this is through these vector arrows. The butt of the arrow has a plus sign, indicating that it's the positive section, okay? And the head of the arrow means negative. That's a negative picture in chemistry as arrow does. But notice, they're pulling equal but opposite in nature, right? So, even though, so would you say this bond is polar or non-polar? The bond is polar or non-polar? Polar, right? Why? It's because there's a difference in electronegativity. Yeah, there's partial charges, okay? The bond itself is polar. But if you asked if the whole molecule is polar, you would say no because they're pulling opposite charges. So, it's like pulling tug-of-war. Two people pulling tug-of-war that are of equal strength. You're not going. So, the bonds are polar, but the molecule itself is non-polar. We'll talk more. Yeah. Yeah, so it would be polar then because there would be a difference of electronegativity, right? So, we'll talk more about this. And in fact, this is a linear molecule. So, when we get other geometries of molecules, you'll see that they may be polar or non-polar just due to their various geometries, okay? Are there any other questions on this? Cool.