Multiple Choice
Which of the following should have the highest surface tension at a given temperature?
12. Liquids, Solids, and Intermolecular Forces
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 type of intermolecular forces present in each compound. For example, CH3–O–CH3 (dimethyl ether) has dipole-dipole interactions and London dispersion forces, KI (potassium iodide) has ionic bonds, C6H5OH (phenol) has hydrogen bonding, C6H14 (hexane) has London dispersion forces, and C60 (buckminsterfullerene) has London dispersion forces.
Understand that the strength of intermolecular forces affects boiling points. Ionic bonds are generally stronger than hydrogen bonds, which are stronger than dipole-dipole interactions, which are stronger than London dispersion forces.
Consider the molecular size and shape. Larger molecules with more surface area typically have stronger London dispersion forces due to increased electron cloud interactions.
Compare the compounds based on the type and strength of their intermolecular forces. Ionic compounds like KI usually have high boiling points due to strong ionic bonds. Hydrogen bonding in C6H5OH also leads to a higher boiling point compared to compounds with only London dispersion forces.
Determine that C6H14, which only has London dispersion forces and is relatively small compared to C60, will have the lowest boiling point among the given options.
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