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Today we will have a look at intermolecular forces and focus our attention at the factors that cause intermolecular forces to be stronger in certain molecules.
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And we will do this by looking at three different molecules.
00:14
So let's look at these three molecules, carbon tetrafluoride, ammonia, and boron trichloride.
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I would recommend pausing the video right now and looking at these three molecules and thinking what the dominant intermelecular force would be in each molecule, and then coming back to see if you got it right or not.
00:33
So for carbon tetrafluoride, the dominant intramalcular force found is london dispersion forces.
00:41
And you might be wondering, why is it that? because there's obviously a very great difference in electronegativity between the bond of a carbon and a fluorine, since fluorine is the most electrode negative, a molecule in the periodic table.
00:57
So there's obviously going to be a dipole right, but a fluoride, it's because the dipoles cancel out.
01:11
As i'm going to show you here, they cancel out from one another.
01:23
So the main reasons for the existence of non -polarity in carbon tetral fluoride, despite the individual bonds being extremely polar, is the canceling of the dipole moments, as i've just shown you...