Multiple Choice
Which molecules would most likely cause a liquid to have the lowest viscosity?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces and Physical Properties
Multiple Choice
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.
