I'm pretty sure these molecules are polar

  1. Aug 29, 2013 #1
    Are there not dipole-dipole interactions between CHBr3, CH3Br, CH3Cl, and CHCl3? Assume they are all separate pure substances. My professor today said that the only intermolecular forces present were dispersion forces. Are the dipole attractions negligible due to fact they are too weak?
     
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  3. Aug 29, 2013 #2

    DrClaude

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    All these molecules are polar. It's hard for me to see how dipole-dipole interactions would be negligible compared to dispersion forces.
     
  4. Aug 29, 2013 #3
    That's what I thought. I'll approach her with this next class period. I don't see how someone with a doctorate could miss something so obvious. There must be more to it.
     
  5. Aug 29, 2013 #4

    chemisttree

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    There isn't.
     
  6. Aug 29, 2013 #5
    for example chloromethane is non-polar because it's a symmetrical molecule and its dipole moments cancel each other out...
     
  7. Aug 29, 2013 #6

    DrClaude

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    It has a C3 symmetry axis along the C-Cl bond, but that bond is highly polar. CH3Cl had a dipole moment of 1.9 D.
     
  8. Aug 29, 2013 #7

    DrClaude

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    I've heard PhDs say pretty stupid things!

    Depending on her particular field, this might be a subject she is less comfortable with.
     
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