And so we can explain the states of matter by looking at the intermolecular forces that are present in these molecules. So if I think about one molecule of ethanol, I know that the bonds between oxygen and hydrogen is polarized. I know that oxygen is more electronegative. So it will be partially negative. And the hydrogen is partially positive as it loses some electron density. If that molecule of ethanol interacts with another molecule of ethanol, the second molecule of ethanol is also polarized.
The oxygen is partially negative. And the hydrogen is partially positive. And we know that opposite charges attract. So the partially positively-charged hydrogen is attracted to the partially negatively-charged oxygen like that. And there's going to be attraction between those two molecules.
And we call this intermolecular force hydrogen bonding, the strongest type of intermolecular force. So hydrogen bonding is present between molecules of ethanol. And this accounts for its large boiling point. Let's look at more details about hydrogen bonding here. So hydrogen bonding exists when you have hydrogen bonded to an electronegative atom like that to this oxygen.
But students forget that you also need another electronegative atom over here to give you more of a difference in charge and to make that hydrogen more partially positive. So it's really three atoms involved in hydrogen bonding there. Let's look at dimethyl ether and see why it does not exhibit hydrogen bonding. So if I were to draw one molecule of dimethyl ether here.
And think about the polarization between the oxygen and this carbon right here. Oxygen is more electronegative. This carbon will be partially positive like that. If I think about the interaction of that molecule of dimethyl ether with another molecule of dimethyl ether like that, you might be tempted to say, well there could be some hydrogen bonding because I know that this carbon right here has some hydrogens attached to it.
And so some students will say, oh there must be hydrogen bonding between this oxygen down here and this hydrogen. But that is not the case because this hydrogen right here, while it is interacting with an oxygen, this hydrogen is bonded to a carbon which is not very electronegative. And so there's no large differences in electronegativity in the bond between carbon and hydrogen. Even the carbon's a little bit more electronegative. There's not enough to make this a true hydrogen bond. And so really there's only a small amount of dipole-dipole interaction between two molecules of dimethyl ether.
So somewhere on this second molecule, there is a partial negative, partial positive. And so there will be a little bit of dipole-dipole interaction. But it's not very strong. And certainly nowhere near as strong as the hydrogen bonding exhibited on the left. Hydrogen bonding being just the super strong form of dipole-dipole interaction. And so dimethyl ether does not have as high of a boiling point as ethanol. Again, the answer is hydrogen bonding. Let's see what happens to the boiling point of ethers as we increase the number of carbons in the alkyl groups.
So if we're going to look at that dimethyl ether again, and let's compare that to an ether that has more carbons than the alkyl group, so diethyl ether. We've already seen the boiling point of dimethyl ether as approximately negative 25 degrees Celsius. Whereas diethyl ether is about 35 degrees Celsius. And so there's a large difference in boiling points diethyl ethers boiling point is just higher than room temperature.
So it is still a liquid at room temperature and pressure. So let's see if we can look at why diethyl ether has a higher boiling point. We know that ether molecules can't hydrogen bond with each other. So that cannot be the intermolecular force responsible for this increase in boiling point. So if we look at two molecules of diethyl ether interacting, one of the other intermolecular forces that we discussed was London dispersion forces. So London dispersion forces, you watched earlier video for more details.
But when you have these large alkyl groups, provides more surface area for a form of attraction called London dispersion. And so that increased attraction between alkyl groups means that it's harder to pull those molecules apart. It requires more energy to pull those molecules apart, requires more heat in order to do so. So to push this reaction to the right and form ether, add alcohol and remove ether and water as they form.
To push this reaction to the left and form alcohol, add water to ether and remove alcohol as it forms. How do you "remove something as it forms? The ether or alcohol boils off under the reduced pressure, and then recondenses in a separate piece of glassware. Sort of like in distillation. Water has a relatively high boiling point and so is difficult to remove under reduced pressure.
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