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These atoms are electronegative enough to cause a large partial positive charge on the hydrogen atom, yet small enough that their lone pairs of electrons can come close to hydrogen atoms.

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For a hydrogen bond to form, hydrogen must be
bonded to either a fluorine, oxygen, or nitrogen atom.

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Hydrogen bonds typically dominate both dispersion forces and dipole-dipole forces.

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A hydrogen bond is a dipole-dipole attraction that occurs between molecules containing a hydrogen atom bonded to a small, highly electronegative atom with at least one lone electron pair.

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Neighboring polar molecules orient themselves so that oppositely charged regions align.

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These attractions between oppositely charged regions of polar molecules are called dipole-dipole forces.

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Polar molecules contain permanent dipoles; that is, some regions of a polar molecule are always partially negative
and some regions of the molecule are always partially positive.

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Each molecule forms a temporary dipole. When temporary dipoles are close together, a weak dispersion force exists between oppositely charged regions of the dipoles.

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When two molecules are in close contact the electron cloud of one molecule repels the electron cloud of the other. The electron density around each nucleus is, for a moment, greater in one region of each cloud.

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Dispersion forces are the result of temporary shifts in the density of electrons in electron clouds.

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The force of attraction between oxygen molecules

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The attractive forces that hold particles together in ionic,
covalent, and metallic bonds are called intramolecular forces.