Hi.
1-hexanol has a boiling point of about 158 degrees.
1-pentanol has a boiling point of about 137 degrees.
1-propanol has a boiling point of about 97.1 degrees.
Methanol has a boiling point of about 64.7 degrees.
This reveals that the intermolecular forces are stronger as the a chain of hydrogen and carbon gets longer.
If hydrogen bonds are strong dipole-dipole bonds, dipole-dipole are stronger than London Dispersion forces, and the OH group in an alcohol is responsible for the hydrogen bonding, then why wouldn't a jar full of 1-propanol have stronger intermolecular forces than a jar full of 1-hexanol? Wouldn't there be more hydrogen bonds in a jar full of 1-propanol?
I realize that dispersion forces increase as the electron cloud gets larger, are therefore usually more mass means stronger dispersion forces. But aren't dispersion forces significantly weaker than hydrogen bonds?
Thank you for any replies.