The first one has Van der Waals interactions since the entire molecule is nonpolar. The lack of ionic/polar interactions is what makes the boiling point so low since there aren\'t really any forces that need to be overcome. The second has a dipole at the carbonyl, which pulls electron density toward the oxygen. The third is polar and can form hydrogen bonds with other molecules of itself. This is why its boiling point is the highest, since hydrogen bonds are the strongest intermolecular forces. Solution The first one has Van der Waals interactions since the entire molecule is nonpolar. The lack of ionic/polar interactions is what makes the boiling point so low since there aren\'t really any forces that need to be overcome. The second has a dipole at the carbonyl, which pulls electron density toward the oxygen. The third is polar and can form hydrogen bonds with other molecules of itself. This is why its boiling point is the highest, since hydrogen bonds are the strongest intermolecular forces..

1. The first one has Van der Waals interactions since the entire molecule is nonpolar.
The lack of ionic/polar interactions is what makes the boiling point so low since there aren't
really any forces that need to be overcome. The second has a dipole at the carbonyl, which pulls
electron density toward the oxygen. The third is polar and can form hydrogen bonds with other
molecules of itself. This is why its boiling point is the highest, since hydrogen bonds are the
strongest intermolecular forces.
Solution
The first one has Van der Waals interactions since the entire molecule is nonpolar.
The lack of ionic/polar interactions is what makes the boiling point so low since there aren't
really any forces that need to be overcome. The second has a dipole at the carbonyl, which pulls
electron density toward the oxygen. The third is polar and can form hydrogen bonds with other
molecules of itself. This is why its boiling point is the highest, since hydrogen bonds are the
strongest intermolecular forces.