Question

Which of the following best explains why 1-butanol, CH₃CH₂CH₂CH₂OH, has a higher surface tension than its isomer, diethyl ether, CH₃CH₂OCH₂CH₃?

(A) the higher density of 1-butanol
(B) the lower specific heat of 1-butanol
(C) the lack of hydrogen bonding in 1-butanol
(D) the higher molecular mass of 1-butanol
(E) the presence of hydrogen bonding in 1-butanol

Answer 1

1-butanol has a higher surface tension than diethyl ether because of the presence of hydrogen bonding in 1-butanol, which is due to its -OH group. So the correct option is E.

Step-by-step explanation:

The reason why 1-butanol, CH3CH2CH2CH2OH, has a higher surface tension than its isomer, diethyl ether, CH3CH2OCH2CH3, is due to the presence of hydrogen bonding in 1-butanol. Hydrogen bonds are a strong type of intermolecular force that occurs when a hydrogen atom covalently bonded to a highly electronegative atom, such as oxygen, is attracted to another electronegative atom in a different molecule. 1-butanol can form hydrogen bonds because of its -OH group, leading to increased surface tension in comparison to diethyl ether which mainly exhibits weaker London dispersion forces due to its lack of hydrogen-bonding capacity.

Answer 2

As the H bond of the butanol is more effective and strong than Van der Waals forces of the ether the surface tension in alcohol is more intensive.

So the correct answer is e)