 Let's just continue our discussion of structural isomers. So recall that isomers are compounds that have identical molecular formulas, but are different structurally. So these structural isomers are isomers whose atoms are bonded in different patterns, right? So we can do an example of some structural isomers by doing this molecule, this molecular formula here, C2H6O. Remember the H's always have to be on the outside of the molecule because they can only make one bond, okay? So you know that the carbons and oxygens have to be linked as what we've been calling like the backbone chain or whatever, okay? So you can imagine since there's, we have two carbons and an oxygen, we can arrange them, carbon, carbon, oxygen like that, or we could arrange them, carbon, oxygen, carbon. Is there any other way that we could arrange those? I can't see it, so, okay? So then if we look, right, we've got the six hydrogens. We know that carbon likes to make how many bonds? Four bonds, right? So help me out, guys, that everybody's here today, so I know it's all early in the morning, but so carbon, remember, likes to make four bonds, right? Four bonds. And oxygen, right, likes to make how many bonds? Two bonds, right? And there's the two, what, lone pairs, right? Okay, so let's show those four bonds. So there's four bonds to carbon, four bonds to carbon, right? I'm just going to show those two bonds to oxygen on opposite sides because we're doing like the Lewis structure now. We can just show these same thing. Oxygen already has its two bonds. To finish up these bond line formulas, right, we just got to stick in our hydrogens. And we can see one, two, three, four, five, six, right? Molecules here. I think we talked about these at the very end. We kind of had a kind of interrupted discussion because we were trying to go fast at the very end, right? But this molecule here is ethanol. This is the stuff that's in like beer or vodka or whatever that, you know, gets you inebriated. And this stuff here has a different name, of course, because it's a different thing, right? This is called dimethyl. We can do the condensed structures if you guys wanted to. Let's do the condensed structures first. Remember, condensed structures, we just squish everything together, right? So it's just like as if you were needing to write it on a typewriter or something like that, right? So the condensed structure of this one would be, you guys can help me. CH3, right? What would be next? CH2, right? OH, very good, guys. I'm sleepy too, so it's all right. So this one would be what? How do we do this? CH3, OH, CH3, OK? I might have said we could do it at CH3, 2, 0, but it's kind of confusing when the things are on opposite sides, OK? So if you did this, this is totally cool. I'll use the condensed structure. Let's draw the bottom line formulas for this, OK? So bottom line formula for ethanol, remember it's like that Charlie Brown, right? Like up, down, up, down, up, down. So one carbon, carbon 1, carbon 2, and then the oxygen, like that, OK? And then for the H there, that's the bottom line formula. You could if you wanted to, the H like that, that's fine too, OK? Remember, so notice we're not showing our H's on the carbons. They're implied, right? So you know how many there should be because of how many bonds carbon has to it. But you have to put your H's on your heteroac, OK? So let's try to do the same thing over here with dimethyl ether. Let's see if I can, if I've brought enough carbons. We could build these guys really quick. You guys can see it hopefully, right? Oh, so that's it. Pick the bottom line formula, right? There's a ball and stick model of it, right? And let's change it to dimethyl ether so we can tell their different structures if we have to break bonds and make bonds, OK? Why? Because that's a reaction when you break bonds and make bonds. Is everybody cool with that? That's what we've been talking about for a long time now, right? So let's try to do this. Well, if we twist it all around, nope, we can't change it into the other thing so we're going to have to break a bond, right? Bam, we broke a bond, that's a reaction. We've got to break this other bond, stick these atoms back together. Just like magic, correct? Go off the screen and now it's a different compound. So you can see that's much different than the other one, right? So if we wanted to show it like the bottom line structure that we got up there, it's that, right? So that's dimethyl ether. Well, this stuff is a gas at room temperature, OK? And this stuff, well, is essentially a liquid at room temperature, OK? Like if you got some Everglare or something like that, right? This stuff, if you smell too much of it, it'll kill you, you know? So, I mean, that stuff will, too, you know, but not as quickly, you know? So this does no good for you. About the other stuff, you know? I guess if you drink a glass of wine a day or something, it's good for your heart. So there are any questions on this stuff? The other thing you can see, so, yeah, so it says there's some more things. Ethanol is completely soluble in water, right? Dimethyl ether is partially soluble in water. So these kind of physical characteristics prove that they're two different compounds. They have different melting points, different boiling points, so on and so forth, OK? So are there any questions about this one? I think that's a pretty good video.