Re: Why ozone (O(O2)) is not an anhydride? cfr. SO2 (amended)

On 4 Ott, 14:49, "Rob" <robbie.buckleyaoptusnet.com.au> wrote:
"Angelo" <patri...@xxxxxxxxx> wrote in message

news:25854257-d070-4b04-b6e8-a856f7543c16@xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx
On 3 Ott, 08:37, Angelo <patri...@xxxxxxxxx> wrote:
On 3 Ott, 08:04,Angelo <seir...@xxxxxxxxx> wrote:

[First of all, I should learn not to post anything
when I'm so badly tired :-(
Apologies to all readers and thanks tall responders.
Below an amended version of what I wanted
to write.]

As in the subject, what prevent, if any,
the ozone from behaving as an anhydride
in water solution, forming at least some
H2OO3 acid like SO2 does?
(albeit H2SO3 is not so stable to be
isolated from aqueous solutions).

IOW, it seems that O3 (OO2) is not a
sufficiently strong Lewis acid to
pick a H2O molecule and rearrange
to form te mentioned Broensted acid,
as do almost all anhydrides.

Any suggestion is welcome

Angelo

Where do you suggest the electron pair from the water molecule attaches
itself? SO2 is acidic because it can accept another electron pair (from the
0 atom of the water molecule). Ozone isn't because it can't.

Please, excuse me, but are you sure?
If you make a sketch of the O3 molecule
I bet that you'll find the central O capable
of accepting an electron pair, because you'll
see also that, at the same time, that O can
transfer one (bonding) electron pair to one
of the two other O's. Moreover, the central O
has a partial positive charge, and that may help.

Best regards
Angelo
.

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