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Because the reaction 3O2 → 2O3 requires energy input, so it absorbs photons.The reverse reaction 2O3 → 3O2 requires the presence of a "third body" to remove the heat of reaction. It is not spontaneous (ozone is stable in the absence of any oxidisable substances or catalysts) so won't emit or absorb a photon. I have a feeling that your school textbook has got it wrong.
I've learnt in school that the energy required to break Ozone O3 into O2 +O is equivalent to a UV-Phtoton with a wavelength of 220-310 nm. Why is it that when O+O2 bond to become O3, a photon with a wavelength of 220-310 nm isn't emited?
A matter of interpretation! I read "may decompose explosively" as fairly stable, but then I play with stuff like positronium which selfannihilates in femtoseconds or less, so I assume that if someone has actually described and photographed a blue liquid using ordinary garden photons and a test tube, it's "stable"! I withdraw my assertion.