Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 24 - The Chemistry of Life: Organic and Biological Chemistry - Integrative Exercises - Page 1090: 24.95


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.
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