Gases, liquids and solids are all made up of atoms molecules and or irons, but the behavior of these particles do differ within the three phases so fast. We were looking at bro mean pence of fluoride, that B r f five, so Penta meaning five. So what we have is a central bro mean bonded to five fluoride in a square parameter geometry. So we see that bromine has one lone power of electrons. So this does distort the geometry ever so slightly. So because this molecule is polar, we have permanent dipole dipole forces that are present as well as dispassion forces. And the next example, we're looking at acetone. So that is C two 86 oh, so what we have here is a carbon, I'll group on the central carbon. And so of course, we have a permanent dye pole with that group with a C double Bondo. And so because the carbon is double bound to the more electro negative oxygen are, electrons will be attracted to the oxygen. This makes the acetone polar, however, because the oxygen does not have a hydrogen group attached, we don't see hydrogen bonding, even though we do have hydrogen is present in the structure they're attached to the carbon. And so what we have is dipole dipole forces again, and of course, dispassion. Finally, we have formaldehyde H two C. O. So it's a very simple carbon, I'll, so it has a carbon double bond to an oxygen. So again, we have another polar compound. So because it's polar, we can have dipole dipole, we can have discussion. So all three of these molecules have the same into molecular interaction types.