# Why does ozone have an electrostatic potential map similar to that of SO2?

This is the electrostatic potential for ozone.

This is the electrostatic potential for sulfur dioxide.

(Click to enlarge)

They look almost exactly the same except one is all oxygen atoms and the other has sulfur in the center instead of oxygen.

Why does ozone have an MEP (molecular electrostatic potential) similar to that of SO2?

• Because their outer orbitals are very similar. The bonding nature in these to molecules is exactly the same with slightly more electronic structure moved from central atom in $\ce{SO2}$. – permeakra Aug 9 '14 at 20:27
• yeah but 1 is polar(the sulfur dioxide) and the other is nonpolar with a positive charge(the ozone). I would expect that the positive charge of ozone would make the central oxygen pull harder in the bond(because of the positive charge it has) and thus the electrons spend less time around the terminal oxygens thus making the MEP more like the one of H2O – Caters Aug 9 '14 at 20:40
• Ozone is non-polar? You might want to rethink that. – Dissenter Aug 9 '14 at 20:50
• there is 0 dipole moment because all atoms in ozone have the same electronegativity. 0 dipole moment means nonpolar. However it is an ion to some degree because of the positively charged oxygen in the center. – Caters Aug 9 '14 at 20:56
• @caters Ozone has dipole moment of ~ 0.5 D. It is three times smaller than for sulfur dioxide, but still high enough. And I repeat, both have roughly same electron structure. – permeakra Aug 9 '14 at 21:22

Resonance structures of $\ce{SO2}$ and $\ce{O3}$.
As you can see from the diagram $\ce{O3}$ and $\ce{SO2}$ are isoelectric and have the same shape and this accounts for their very similar electrostatic potential maps. Both molecules are polar although $\ce{SO2}$, with a dipole moment of 1.62D, is more polar than $\ce{O3}$ (0.53D). As the diagram shows, the polarity of both molecules is due to the their trigonal planar shape with a formal positive charge on the central atom.