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When comparing boiling point of h2o, h2s, h2se, and h2te, the trend is h2o>h2te>h2se>h2s. I understand that the greater molecular weight allows greater van der waals forces, but doesn't h2s have a greater dipole than h2te? H2o should definitely be first because of hydrogen bonding but I do not understand the trend for rest.
When you compare boiling points of molecules, does London dispersion usually beat dipole dipole forces unless it was hydrogen bonding?
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When you compare boiling points of molecules, does London dispersion usually beat dipole dipole forces unless it was hydrogen bonding?
Sent from my iPhone using SDN mobile