Ethanol molecules have stronger dipole-dipole interactions than dimethyl ether because ethanol demonstrates hydrogen bonding. CH2F2 is polar and larger, allowing it to have dipole-dipole interactions and strong London Dispersion Forces.
Work Step by Step
The molecular structure of ethanol because contains O-H, allowing hydrogen bonds to form, unlike its isomer dimethyl ether. This causes more heat energy to be required to vaporize it. The electronegativity differences between C and F in CH2F2 allow for stronger dipole attractions. In addition, since CH2Fs, there are more electrons to form instantaneous dipoles, which cause London Dispersion Forces.