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Which statement best explains why oil and water do not mix?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
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Which one of the following molecules would have the largest dispersion (London) forces?
A
CO2
B
CCl4
C
NH3
D
CH4
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Understand that dispersion (London) forces are a type of intermolecular force that arise due to temporary fluctuations in electron density, creating instantaneous dipoles. These forces generally increase with the size and polarizability of the molecule.
Compare the molecular sizes and molar masses of the given molecules: CO\_2, CCl\_4, NH\_3, and CH\_4. Larger molecules with more electrons tend to have stronger dispersion forces.
Recognize that CCl\_4 has the largest molar mass and the most electrons among the options, which means it is more polarizable and will exhibit stronger dispersion forces.
Note that although NH\_3 has hydrogen bonding (a stronger intermolecular force), the question specifically asks about dispersion forces, so we focus on molecular size and electron cloud polarizability.
Conclude that CCl\_4, being the largest and most polarizable molecule, will have the largest dispersion (London) forces among the given molecules.
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