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AleksandrR [38]
3 years ago
12

For molecules of comparable mass, why are dipole-dipole forces stronger than dispersion forces?

Chemistry
1 answer:
Leviafan [203]3 years ago
7 0
Dispersion forces, otherwise known as induced dipole-induced dipole interactions, polarize a molecule slightly into weak negative and weak positive charges. Then coulombs law dictates their electrostatic attractions. However, in dipole-dipole, these molecules are already polarized permanently and typically of a much larger magnitude than an induced dipole for a molecule of the same molar mass. This means that the electrostatic attractions are significantly stronger than the London Dispersion force's.
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