[non_compus_mentis]

You know how you're all just dying to explain polarity to me... ? Haha. Please. From the start.

[gregpawin]

http://www.chemicalforums.com/index.php?board=8;action=display;threadid=66

If you have more questions, please reply.

[Bob Bobson]

This may be a dumb question, but is ozone polar?  As far as I know, it does not have polar bonds but I know oxygen is paramagnetic (has unpaired electrons) and thus attracted to a magnetic field.  Also, I know ozone has a bent 120 degree shape--which is usually polar.  Any insight?

[jdurg]

I had always thought that polarity was caused by differing electronegativities of the atoms involved in a bond.  If you have two atoms of the same element bonded to each other, they both have the same electronegativity so they would have to be non-polar.  Is that correct?  

[Corvettaholic]

Based on a some recent reading today, I'd say you're right Jdurg. The way I understand it, you need differing electronegativty to be polar, and if its a big difference... the bond is no longer covalent but ionic.

[AWK]

polarity of ozone:

http://www.newton.dep.anl.gov/askasci/chem00/chem00707.htm

http://www.colby.edu/chemistry/webmo/ozone.html

[jdurg]

polarity of ozone:

http://www.newton.dep.anl.gov/askasci/chem00/chem00707.htm

http://www.colby.edu/chemistry/webmo/ozone.html

Heh.  This shows why polarity can be a bit of a pain to deal with.  On a bonding level, O₃ is completely non-polar.  But on a molecular level, it is indeed polar.  (I.E. all the bonds involved are completely non-polar as they are all the same atom, but the geometry of the molecule causes the electrons to seemingly gather at one end of the molecule).  I guess you could say everybody was right on this one.