Do dipole-dipole interactions influence the evaporation of liquids and condensation of gases?
Butane and Acetone have almost the same molar mass. Butane is straight chain alkane with only C-C and C-H bonds and no double bonds. It only interacts with itself through London Dispersion forces (induced dipole induced dipole). It's melting point is -141C and boiling point -1C. So it will boil away in a snow storm.
Acetone is the most simple ketone - 3 carbons with a C=O bond, which is very polar. So it has London Dispersion forces and Dipole-Dipole interactions. Its melting point is -95C and boiling point is +56C.
The significant increase in boiling point can be attributed to polarity of the C=O bond. This molecule does not possess the ability to hydrogen bond with itself, so its increases in mp and bp can be attributed to the polarity of the carbonyl group.
Impact of this question
Creative Commons License