 Okay, so let's go ahead and predict whether these are polar or non-polar. So the first thing you want to do is predict the structural formula of these molecules. And you can do that by doing the Lewis-Dott structure first. So I'm assuming that you know how to do Lewis-Dott structure, so we'll just take it from there to structural formulas, okay? So the structural formula for this molecule, CO2, looks like that, okay? And even though oxygen, the oxygen carbon bond here is polar because oxygen is 3.5 vice, carbon is 2.5, okay? What you'll find is that even though this dipole arrow goes that way, okay? And this dipole arrow goes that way, so you have two polar bonds. They're both exactly one divide in this direction and one divide in this direction, so they cancel each other out. So this is a linear molecule, of course. Those are directly opposite from each other, so they cancel each other out. So this is non-polar. CO2 is a non-polar. So let's go ahead and look at SCL2 now. So SCL2 has a similar shape to H2O with S being the central atom and of course CLs being the outside atoms, okay? So it has this bent geometry due to its four electron groups, two of them being lone pairs. So this bond angle here is approximately 104.5 degrees. What you find is if you do the difference in electromegativity, you'll find that S has a 2.5 electromegativity and CL has a 3.0. So the arrow, dipole arrow for that bond goes that way and then for that bond goes that way. So what we need to do for this one is add them both up, okay? Add these two vectors up. What you find is that it goes straight through the middle. So that's the overall dipole of the molecule. So these bonds themselves, they're polar bonds, but the molecule is polar in such a way that the bottom is positively charged, are negatively charged and the top is positively charged. BRCL, that's of course a simple diatomic molecule. There's no bond angle here. So BR is 2.8 and CL is 3.0. So you see that CL is more electronegative than BR by 0.2 divided. Remember we said anything lower or 0.4 or lower we're going to consider non-polar, okay? So even though this is a slightly polar bond, we would consider this non-polar molecule. Non-polar because it's lower. SCL. One second, let's record the video and then you can ask all your questions, okay? Let's just do that. So SCS2 now, the same structure as CO2, okay? Remember where S is in relation to O on the periodic table. So C2.5, S is 2.5. Okay, so we don't need to have any polar bonds in this thing. So even if we did, they would be pulling in opposite directions. So this is also a non-polar.