Chemistry Multiple Choice

Chemistry Multiple Choice-86
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So we can see that TFP does have these carbon-fluorine bonds, and we know that a carbon-hydrogen bond isn't all that polar, and fluorine is pretty electronegative, so this is true. So this is true, but does it explain the boiling point trend? So we're saying that if the carbon-fluorine bond is more polar than these bonds here, we're saying that if TFP has more polar bonds, that would normally suggest it has stronger intermolecular forces, which would mean you would predict it to have a higher boiling point.

And so, that's the opposite of what we're actually seeing here.

So, answer choice A says, the carbon-fluorine bond is easier to break than the carbon-hydrogen bond.

And we know this is a wrong answer, because this has nothing to do with intermolecular forces.

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Even though our TFP has more polar C-F bonds, it actually has a lower boiling point, so this observation, which is true, still doesn't explain what we're trying to explain.

(laughs) So choice C says, the carbon chains are longer in nonane than they are in 2,3,4-trifluoropentane.

We have nine carbons versus one, two, three, four, five carbons. We know that even though the molar mass here is the same, the length of the chain is actually related to the London dispersion forces.

So as the length of the chain goes up, that actually means that the London dispersion forces, so the intermolecular forces that happen when you get these tiny instantaneous dipoles, those forces also go up.

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