Dipole moment

         The product of magnitude of the negative or positive charge (q) and the distance (d) between their centres of positive and negative charges is known as dipole moment.

         μ = Electric charge *  bond length

         As q is in the order of 10^-10 esu and d is in the order of 10^-8 cm, m is in the order of 10^-18 esu cm. The dipole moment can be measured in "Debye" (D) unit. 1 D = 10^-18 esu cm = 3.33 * 10^-30 coulomb metre (In S.I. unit).

         Dipole moment is indicated by the arrow having the symbol of () pointing towards negative end. The Dipole moment has both magnitude and direction and hence it is a vector quantity.

Symmetrical polyatomic molecules are not polar so they do not have any value of dipole moment.

Unsymmetrical polyatomic molecules always have the net value of dipole moment, hence such molecules are polar in nature. H₂O, CH₃Cl, NH₃, etc are polar molecules as they have some positive values of dipole moments.

μ ≠ 0 due to unsymmetry   

(1) The dipole moment is a significant factor in determining the geometry of molecules.

: 3.1 Molecular geometry and dipole moment

(2) Each and every ionic compound possessing some percentage of the covalent character according to the Fajan's rule. The percentage of ionic character in the compound having some covalent character can be measured by the following equation.

         The % ionic character . 

(3) The trans isomer commonly possesses either zero dipole moment or very low value in the comparison to cis-form                                                        

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