Why does O3 have a dipole moment?
Ozone is not a linear molecule; therefore, the "two dipole" of Oleft to Omiddle and O middle to Oright don't cancel. You can read about it here.
http://www.newton.dep.anl.gov/askasci/chem00/chem00707.htm
O3, or ozone, is a molecule that consists of three oxygen atoms bonded together. It has a bent molecular geometry with a central oxygen atom and two terminal oxygen atoms. The reason why O3 has a dipole moment, or is polar, is because of the uneven distribution of electron density within the molecule.
To understand this concept, we need to consider the electronegativity (tendency of an atom to attract electrons) of the oxygen atoms. Oxygen is more electronegative than most other elements, and in O3, one oxygen atom (the central atom) tends to pull the electron density towards itself more strongly than the other two oxygen atoms.
As a result, there is an unequal sharing of electrons between the central oxygen atom and the terminal oxygen atoms, creating partial positive charges on the terminal oxygen atoms and a partial negative charge on the central oxygen atom. This separation of positive and negative charges gives rise to the dipole moment in O3.
To calculate or determine the dipole moment of O3, you would need to know the magnitude and direction of the partial charges on the oxygen atoms, as well as the molecular geometry of the molecule. Experimental measurements such as spectroscopy or theoretical calculations using quantum mechanics can be used to determine the dipole moment of O3.