What compounds have dipole-dipole forces?

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Polar compounds have dipole-dipole forces.

Explanation:

Bond dipoles form when there is a large difference in electronegativity between two atoms joined by a covalent bond.

The atoms share the electrons unequally because the more electronegative atom pulls the shared electrons toward itself.

For example, #"H-Cl"# has a dipole. The electrons spend more of their time near the #"Cl"# atom.

That means that the #"Cl"# atom has a partial negative charge, and the #"H"# atom has a partial negative charge.

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We say that the #"HCl"# molecule is polar

Dipole-dipole forces are the attraction between two polar molecules.

When they approach each other, the negative end of one molecule attracts the positive end of the other.

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If there is more than one bond dipole, the molecules may or may not be polar.

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For example, #"CO"_2# has two #"C-O"# bond dipoles. The dipoles point in opposite directions, so they cancel. #"CO"_2# is a nonpolar molecule.

However, #"H"_2"O"# also has two #"O-H"# bond dipoles. The dipoles do not cancel, so #"H"_2"O"# is a polar molecule.

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