Multiple Choice
Which of the following should have the highest surface tension at a given temperature?
8. Gases, Liquids and Solids
Intermolecular Forces and Physical Properties
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Which of the following will have the lowest boiling point?
A
CH3–O–CH3
B
KI
C
C6H5OH
D
C6H14
E
C60
Verified step by step guidance1
Identify the types of intermolecular forces present in each compound. CH3–O–CH3 (dimethyl ether) has dipole-dipole interactions and London dispersion forces. KI (potassium iodide) is ionic and has strong ionic bonds. C6H5OH (phenol) has hydrogen bonding, dipole-dipole interactions, and London dispersion forces. C6H14 (hexane) has only London dispersion forces. C60 (buckminsterfullerene) also has London dispersion forces.
Recall that the strength of intermolecular forces affects the boiling point. Stronger intermolecular forces result in higher boiling points.
Compare the intermolecular forces: Ionic bonds in KI are the strongest, followed by hydrogen bonds in C6H5OH. Dipole-dipole interactions in CH3–O–CH3 are weaker than hydrogen bonds. London dispersion forces in C6H14 and C60 are the weakest.
Consider the molecular size and shape: Larger molecules with more surface area, like C60, can have stronger London dispersion forces compared to smaller molecules like C6H14.
Determine which compound has the weakest intermolecular forces and thus the lowest boiling point. Since C6H14 has only London dispersion forces and is smaller than C60, it will have the lowest boiling point among the given options.
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