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In order for a dipole-dipole interaction to be classified as ?, the molecule must contain O-H, N-H or H-F bonds!

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Final answer:

A dipole-dipole interaction is classified as a hydrogen bond when the molecule contains bonds between hydrogen and highly electronegative atoms like F, O, or N, leading to strong intermolecular forces and unique properties.

Step-by-step explanation:

In order for a dipole-dipole interaction to be classified as a hydrogen bond, the molecule must contain O-H, N-H, or H-F bonds. These bonds are unique due to the high electronegativity of F, O, and N compared to hydrogen, creating a significant dipole with a dense positive charge on the smaller hydrogen atom.

Hydrogen can penetrate into tighter spaces, allowing strong interactions between hydrogen's delta positive (δ+) and the delta negative (δ−) of an adjacent electronegative atom. Hydrogen bonds are significantly stronger than other types of dipole-dipole interactions, which gives substances like water high boiling points and excellent solvent properties due to the strong intermolecular forces.

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