Multiple Choice
Which molecules would most likely cause a liquid to have the lowest viscosity?
13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces and Physical Properties
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Which of the following molecules will have the highest melting point?
(i) CH3−CH2−CH2−CH3
(ii)CH3−CH2−O−CH2−CH3
(iii) CH3−CH2−CH2−CH2−OH
A
(i)
B
(ii)
C
(iii)
D
Cannot be determined.
E
All will have the same melting point.
Verified step by step guidance1
Identify the types of intermolecular forces present in each molecule. For (i) CH3−CH2−CH2−CH3, the molecule is nonpolar and will primarily exhibit London dispersion forces.
For (ii) CH3−CH2−O−CH2−CH3, the molecule contains an ether group, which introduces dipole-dipole interactions due to the presence of the oxygen atom.
For (iii) CH3−CH2−CH2−CH2−OH, the molecule contains an alcohol group, which allows for hydrogen bonding, a stronger intermolecular force compared to London dispersion and dipole-dipole interactions.
Consider the strength of the intermolecular forces: hydrogen bonding is generally stronger than dipole-dipole interactions and London dispersion forces, leading to higher melting points.
Conclude that the molecule with the strongest intermolecular forces, which is (iii) CH3−CH2−CH2−CH2−OH due to hydrogen bonding, will have the highest melting point.
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Textbook Question
Three identical tubes are filled with different liquids; water, ethylene glycol, and olive oil. A small steel sphere was dropped into the tube, and the time it took to fall to the bottom was recorded. Which property of liquids is responsible for the differences in time for the sphere to fall through the liquid? (LO 11.1)(a) Surface tension(b) Boiling point(c) Viscosity(d) Vapor pressure
