The bond dipole moment is a measure for the polarity of a chemical bond within a molecule. The bond dipole μ is given by: 3D (left and center) and 2D (right) representations of the terpenoid molecule atisane. ...

.

The bond dipole is modeled as +δ — δ- with a distance d between the partial charges +δ and δ-. It is a vector, pointing from minus to plus,^[1] that is parallel to the bond.

The SI unit for the bond dipole moment is coulomb-meter (1 C m = 2.9979 10²⁹ debye), δ is the amount of charge in coulomb, and d is in meter. The debye (symbol: D) is a non-SI and non-CGS unit of electrical dipole moment. ... The coulomb (symbol: C) is the SI unit of electric charge. ... The metre, or meter (symbol: m) is the SI base unit of length. ...

For a complete molecule the total molecular dipole moment may be approximated as the vector sum of individual bond dipole moments. Often bond dipoles are obtained by the reverse process: a known total dipole of a molecule can be decomposed into bond dipoles. The reason for doing this is the transfer of bond dipole moments to molecules that have the same bonds, but for which the total dipole moment is not yet known. The vector sum of the transferred bond dipoles gives an estimate for the total (unknown) dipole of the molecule.

The Bond Dipole is two atoms in a bond, such that the electronegativity of one atom changes and draws the electrons towards the other, causing a partial negative charge. There is an increase difference in polarity, and an increase in dipole.

Note

1. ^ Organic chemists use the opposite convention.