Chemical Forums
Chemistry Forums for Students => Organic Chemistry Forum => Topic started by: Cooper on November 09, 2012, 02:29:03 PM
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Hello,
I've been reading about ozonolysis and radicals and my textbook keeps mentioning how weak oxygen-oxygen bonds are, like in ozanides. Why are these bonds so weak? I think it's from electron repulsion. But then why aren't other bonds like Br-Br bonds weak (or are they?), they have more valence electrons. ???
Thanks,
~Cooper
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Why are O-O bonds so weak? Good question. I think this is part of what Pauling was attempting to explain when he created electronegativity theory. If you look as homolytic bond strength, I-I<Br-Br<Cl-Cl>F-F. Why are I-I bonds weak and why aren't F-F bonds stronger? From bond energy, more energy is released upon breakage of the bonds of the smaller atoms. If the bond is also weaker, fluorine is very reactive. I expect oxygen should be similar. At this point, I find it easier to simply remember this than to provide a universal principle that can explain it.