Chapter 11, Problem 73FP

In Chapter 10, we saw that electronegativity differences determine whether bond dipoles exist in a molecule and that molecular shape determines whether bond dipoles cancel (nonpolar molecules) or combine to produce a resultant dipole moment (polar molecules). Thus, the ozone molecule, ${\text{O}}_2$ , has no bond dipoles because all the atoms are alike. Yet, ${\text{O}}_2$ does have a resultant dipole moment: $\mu =0.534D$ . The electrostatic potential map for ozone is shown below. Use the electrostatic potential map to decide the direction of the dipole. Using the ideas of delocalized bonding in molecules, can you rationalize this electrostatic potential map?