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3F.5 part b (7th Ed.) Melting point
Posted: Wed Nov 28, 2018 12:55 pm
by Julia Lindner 1I
This problem asks which has the higher melting point, C2H5OC2H5 (diethyl ether) or C4H9OH (butanol). The answer is butanol, but I don't understand why. Anyone know?
Re: 3F.5 part b (7th Ed.) Melting point
Posted: Wed Nov 28, 2018 1:17 pm
by Patrick Cai 1L
Butanol is a somewhat polar molecule, as evident by the presence of its alcohol functional group (-OH), whereas diethyl ether is a non-polar molecule. The stronger intermolecular forces that come along with butanol as a result of its polar nature make it have a higher melting point than diethyl ether.
Re: 3F.5 part b (7th Ed.) Melting point
Posted: Wed Nov 28, 2018 1:20 pm
by Searra Harding 4I
Butanol has stronger interactions therefore the melting point is higher. H bonding can usually explain a higher melting point.
Re: 3F.5 part b (7th Ed.) Melting point
Posted: Sun Dec 02, 2018 11:36 am
by Milena Aragon 2B
It's mainly because Butanol has the ability to form hydrogen bonds whereas diethyl ether cannot. This additional bond that butanol can form means it has a higher melting point. Just think of it as more/stronger bonds=harder to break apart and thus higher melting/boiling point.
Re: 3F.5 part b (7th Ed.) Melting point
Posted: Sun Dec 02, 2018 7:58 pm
by Tony Chung 2I
it has a stronger IMF, resulting in a higher melting point
Re: 3F.5 part b (7th Ed.) Melting point
Posted: Thu Nov 11, 2021 1:32 pm
by Katie 3H
How does butane have Hydrogen bonding and the other one not? They both have oxygens that can be involved no?