How do dipole dipole forces arise?

Because of the uneven distribution of electrons among the atoms in a compound, dipole-dipole forces develop.

Every molecular dipole moment has a positive and a negative end. A dipole moment is a measurement of the distance between the oppositely charged ends of a dipole.

In a polar compound, the most stable arrangement has the positive end of one dipole close to the negative end of another; thus, in a solution of chloromethane, we would expect the molecules to orient in such a way that the partially negative-charged Cl of one molecule is aligned with the partially positive-charged C of another, and so on. Now, it can be easy to forget that there are always multiple molecules of a compound in whatever substance you might be dealing with.

In conclusion, dipole-dipole forces are intermolecular forces that are typically attractive and arise from the attraction between the positive and negative ends of polar molecules' dipole moments (1).

Dipole-dipole forces arise due to the attraction between the positive end of one polar molecule and the negative end of another polar molecule. This attraction occurs because polar molecules have regions of partial positive and partial negative charge, known as dipoles, due to differences in electronegativity between atoms within the molecule. The orientation of these dipoles results in an overall attractive force between the molecules, which is known as a dipole-dipole force.