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Hydrogen bonds are essentially just extremely strong dipole-dipole forces. They occur when a hydrogen bonded to an N, O, or F comes near a lone pair on another molecule. They are classified as their own time of intermolecular force because the bonds created are much stronger than regular dipole-dipole forces.
605357751 wrote:Are hydrogen bonds also considered a dipole dipole interaction?
Yes - hydrogen bonds are also considered a dipole-dipole interaction. Thus, if you ever observe hydrogen bonding, there is also dipole-dipole interactions.
You can also think about it this way: In a polar molecule, Hydrogen will have a slightly positive charge. On the other hand, a highly electronegative atom, such as F, O, N, will have a slightly negative charge. Thus, there is a dipole-dipole interaction.
Hydrogen bonds are a type of dipole-dipole interaction that are set apart simply because they are much stronger than regular ones. Their strength comes from the high electronegativity of the nitrogen, oxygen, and fluorine atoms they are bonded to.
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