Tetrachloromethane/tetrafluoromethane boiling points

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jamesthelam
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#1
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#1
Explain why the boiling point of tetrachloromethane is higher than the boiling point of tetrafluoromethane.

Is this to do with larger dipoles from chlorine?
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Pigster
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More e- therefore larger London dispersion forces.
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Marrow
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(Original post by Pigster)
More e- therefore larger London dispersion forces.
Or to us simple-minded As-levellers, van der Waals forces!
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Pigster
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(Original post by Marrow)
Or to us simple-minded As-levellers, van der Waals forces!
It depends on which exam board you're taking.

I'll bet you're AQA.
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KaylaB
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(Original post by Pigster)
It depends on which exam board you're taking.

I'll bet you're AQA.
We call it van der Waals' forces too and I'm on OCR
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alow
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(Original post by Pigster)
It depends on which exam board you're taking.

I'll bet you're AQA.
I did OCR and I've never heard of "London dispersion forces".
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Pigster
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I made an assumption that the OP & Marrow are Y12.

This year is the last year of the current OCR A spec (F321-F326) and they called them VdW forces.

The new spec (Y12 kids doing currently) starting this year calls intermolecular forces as a group VdW forces and (correctly) calls just id-id forces as LDF.

OCR B has always done it correctly, I understand.
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