Which would be expected to have the higher boiling point? Explain. a. 1-butanol

Question

Which would be expected to have the higher boiling point? Explain.
a. 1-butanol (CH3CH2CH2CH2OH) or diethyl ether(CH3CH2OCH2CH3) b. t-butyl alcohol ((CH3)3COH) or 1-butanol(CH3CH2CH2CH2OH) c. 1-propanol (CH3CH2CH2OH) or 1-butanol(CH3CH2CH2CH2OH)
Explain as best you can! Will give credit to all but most tothe person who responds with best answer!!
a. 1-butanol (CH3CH2CH2CH2OH) or diethyl ether(CH3CH2OCH2CH3) b. t-butyl alcohol ((CH3)3COH) or 1-butanol(CH3CH2CH2CH2OH) c. 1-propanol (CH3CH2CH2OH) or 1-butanol(CH3CH2CH2CH2OH)
Explain as best you can! Will give credit to all but most tothe person who responds with best answer!!

Explanation / Answer

a. diethyl ether boils WAY lower than n-butanol. it is anether and the H bonds between ethers are way weaker than between OHgroups b. t-butyl ol will boil LOWER than n-butanol because itis bulkier (think of a bunch of them packing together) thus willhave less favourable H-bonding interactions. n-butanol (it isnormal, after all) will pack nicely and have many H-bonds as wellas dipole dipole and london dispersion. c. n-propanol boils LOWER, it is a shorter chain alkaneand longer chains = larger surface area for londondispersion/electrostatic dispersion forces, which will increase theboiling point. (more forces=more energy needed to boil) Hope this helps. Your ochem textbook will have lots moreexamples of these classic problems...

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