[KAJLogic]

what is the reason O₃ can't just have three single bonds all to one another. A reason I found is that if the pz and py were in connection then the px(s) would be in similar distance with one another which would force a repulsion. Is there more involved in why it cannot simply bond all three in a triangular fashion, and are the things I said accurate.

[billnotgatez]

http://en.wikipedia.org/wiki/Ozone#Structure
Is this what you are looking for

[KAJLogic]

I was kind of just trying to understand why
             O
            /  \
          O --O                   isn't possible

[Archer]

http://en.m.wikipedia.org/wiki/Cyclic_ozone

This suggests that it does exist, in tiny amounts.

[KAJLogic]

Well then can I ask why it is less frequently formed like that?

[Archer]

It's really not my area of expertise, but reading the references on the wiki page it looks as though the energy needed to bend acyclic O₃ into the correct conformation so that it could form a new bond is very high.

I suppose it's rather like getting a really, really strong spring with hooks on either end to make a loop, it is possible but a lot of energy is required.

Someone please correct me if this sounds absurd.

[magician4]

"small angle strain" is the magic expression: look at your triangle, where all bonds are 60° (which requires very unfavourable hybridization to achieve)
also, there is considerable torsional strain, as all free electron pairs are forced to be eclipsed here

you might wish to compare this situation to cyclopropane (and those "banana bonds" involved there) vs. propene


regards

Ingo