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, $\text{H-Cl}$ has a dipole. The electrons spend more of their time near the $\text{Cl}$ atom.

That means that the $\text{Cl}$ atom has a partial negative charge, and the $\text{H}$ atom has a partial negative charge.

We say that the $\text{HCl}$ 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.

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

For example, ${\text{CO}}_{2}$ has two $\text{C-O}$ bond dipoles. The dipoles point in opposite directions, so they cancel. ${\text{CO}}_{2}$ is a nonpolar molecule.

However, $\text{H"_2"O}$ also has two $\text{O-H}$ bond dipoles. The dipoles do not cancel, so $\text{H"_2"O}$ is a polar molecule.

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