Hydrogen bonds are stronger than London Dispersion forces, which are the weakest intermolecular force.
Hydrogen bonds are stronger than dipole-dipole interactions, which are the second weakest of the intermolecular forces.
Hydrogen bonding begins with hydrogen binding to a highly electronegative atom, typically fluorine, oxygen, nitrogen, or in some cases carbon.
When hydrogen binds to a highly electronegative atom, it gains a partial positive charge because the electrons are pulled closer to the electronegative atom.
When an electronegative atom binds hydrogen, it gains a partial negative charge because the electrons are pulled closer to the electronegative atom.
The partial positive hydrogens interact with partial negative electronegative atoms on other molecules, so that multiple molecules are weakly bound together by the hydrogen bonds.
Hydrogen bonds increase the boiling point of substances because they are extra intermolecular forces that must be broken to pass into the gas phase.
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