Abstract
It is striking and well known that most of the familiar cases of chemiluminescence in solution involve oxygen, bioluminescence being the foremost example (1). Yet it is clear that not one particular state of the oxygen molecule, nor one single mechanism can be given credit for this prevalence. Ground state triplet oxygen is involved in the many free-radical autoxidation processes which emit low yield luminescence. The step responsible here for the generation of electronically excited products is probably the disproportionation of two peroxy radicals, in what may be a concerted Russell chain termination (2). Singlet oxygen is itself directly the origin of the remarkable red chemiluminescence attending the heterolytic decomposition of hydrogen peroxide. Here the light emitting step is a unique energy pooling process combining the energies of two O2(l∆g) into one double-size quantum (3). Examples of such a pooling process followed by energy transfer to a fluorescer have been observed, but it is evident that such processes will have low quantum yields and can hardly be a general mechanism of chemiluminescence, as envisioned by Khan and Kasha (4). However, singlet oxygen is efficient at forming peroxides (3c,d), which are potential sources of luminescence. The superoxide ion is the likely intermediate in another class of peroxidation and in the decomposition of hydrogen peroxide catalyzed by some metal ions or by peroxidases (5). The dismutation of O2 may generate singlet oxygen (6), but here again such a step would give only very low yields of luminescence.
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Lee, D.CS., Wilson, T. (1973). Oxygen in Chemiluminescence. A Competitive Pathway of Dioxetane Decomposition Catalyzed by Electron Donors. In: Cormier, M.J., Hercules, D.M., Lee, J. (eds) Chemiluminescence and Bioluminescence. Springer, Boston, MA. https://doi.org/10.1007/978-1-4757-0638-3_20
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DOI: https://doi.org/10.1007/978-1-4757-0638-3_20
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