Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: non_compus_mentis on April 10, 2004, 06:51:51 AM
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You know how you're all just dying to explain polarity to me... ? Haha. Please. From the start.
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http://www.chemicalforums.com/index.php?board=8;action=display;threadid=66 (http://www.chemicalforums.com/index.php?board=8;action=display;threadid=66)
If you have more questions, please reply.
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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?
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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?
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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.
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polarity of ozone:
http://www.newton.dep.anl.gov/askasci/chem00/chem00707.htm
http://www.colby.edu/chemistry/webmo/ozone.html
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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. ;D