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    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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    More e- therefore larger London dispersion forces.
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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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    (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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    (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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    (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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    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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