Diethyl ether has a boiling point of 34.5 degree C and 1-butanol has a boiling p

Question

Diethyl ether has a boiling point of 34.5 degree C and 1-butanol has a boiling point of 117 degree C. Both compounds have the same molecular weight and same molecular formula (C_4H_10O). Which statement best explains the difference in boiling points? a. The strength of London dispersion forces is greater in 1-butanol b. Oxygen is toward the end of the structure in 1-butanol and in the middle of the structure in Diethyl ether c. The 1-butanol molecules can form strong hydrogen bonds with other 1-butanol molecules. Diethyl ether forms dipole-dipole intermolecular forces, which are not as strong as hydrogen bonds d. The Diethyl ether molecules have more hydrogen atoms in place to form strong hydrogen bonds with other Diethyl ether molecules. 1-butanol also forms hydrogen bonds, but not as many as Diethyl ether.

Explanation / Answer

statement 3 is correct

n-butanol has OH group it can form hydrogen bond with other butanol.

where as the diethyl ether has only london disperson forces only.

so due to strong hydrogen bonding butanol has higher boiling point

So statement 3 is correct

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