The discussion centers around the polarity of certain molecules (CHBr3, CH3Br, CH3Cl, and CHCl3) and the nature of intermolecular forces present in these substances, specifically dipole-dipole interactions versus dispersion forces. Participants explore the implications of molecular symmetry on polarity and the validity of claims made by a professor regarding intermolecular forces.
Participants generally disagree on the assessment of intermolecular forces in the discussed molecules, with some asserting the presence of significant dipole-dipole interactions while others support the professor's view of dispersion forces being predominant. The discussion remains unresolved regarding the validity of these claims.
There is a lack of consensus on the definitions and implications of molecular symmetry and polarity, as well as the strength of different types of intermolecular forces. Some assumptions about the professor's expertise and the nature of the molecules are not fully explored.
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.janhaa said:for example chloromethane is non-polar because it's a symmetrical molecule and its dipole moments cancel each other out...
aclark609 said:I don't see how someone with a doctorate could miss something so obvious.