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Can someone explain how to differentiate a molecule that has dipole-dipole interaction vs. dipole-induced interactions? I understand that dipole-induced interactions occur when an electric dipole and an instantaneous dipole induces a nonpolar molecule, but how can we identify that a molecule does in fact have dipole-induced interactions?
Every molecule has the potential to form dipole induced dipole induced interactions. Dispersion forces, or dipole induced interactions, are when electrons in the electron cloud randomly, by chance, can shift to one side creating a temporary dipole moment. The partial positives and partial negatives can cause a nearby molecule to form dipoles, and the attraction between oppositely charged molecules will cause the formation of dispersion forces. Dipole-dipole forces are only between molecules that are polar, while dipole induced interactions are between molecules that can be polar or nonpolar
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