This is an audio version of the Wikipedia Article:
00:01:54 1 Nomenclature
00:03:07 2 History
00:06:19 3 Physical properties
00:07:45 4 Structure
00:08:37 5 Reactions
00:09:46 5.1 With metals
00:10:00 5.2 With nitrogen and carbon compounds
00:10:23 5.3 With sulfur compounds
00:11:32 5.4 With alkenes and alkynes
00:12:40 5.5 Other substrates
00:13:39 5.6 Combustion
00:14:17 5.7 Reduction to ozonides
00:15:10 5.8 Applications
00:16:30 6 Spectroscopic properties
00:17:37 7 Ozone in Earth's atmosphere
00:19:27 7.1 Ozone layer
00:20:01 7.1.1 Location and production
00:20:09 7.1.2 Importance to surface-dwelling life on Earth
00:23:00 7.2 Low level ozone
00:23:47 7.2.1 Ozone cracking
00:25:33 7.2.2 Ozone as a greenhouse gas
00:26:51 8 Health effects
00:28:40 8.1 Ozone air pollution
00:28:49 8.1.1 Heat waves
00:34:18 8.2 Physiology
00:34:50 8.3 Safety regulations
00:37:12 9 Production
00:39:10 9.1 Corona discharge method
00:40:33 9.2 Ultraviolet light
00:41:41 9.3 Cold plasma
00:43:23 9.4 Electrolytic
00:44:38 9.5 Special considerations
00:45:48 9.6 Incidental production
00:48:10 9.7 Laboratory production
00:49:30 10 Applications
00:51:27 10.1 Industry
00:51:36 10.2 Consumers
00:55:59 10.3 Aquaculture
00:59:07 10.4 Agriculture
01:00:22 10.5 Medical
01:01:33 11 See also
01:01:50 12 Notes
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"The only true wisdom is in knowing you know nothing."
Ozone , or trioxygen, is an inorganic molecule with the chemical formula O3. It is a pale blue gas with a distinctively pungent smell. It is an allotrope of oxygen that is much less stable than the diatomic allotrope O2, breaking down in the lower atmosphere to O2 or dioxygen. Ozone is formed from dioxygen by the action of ultraviolet light (UV) and electrical discharges within the Earth's atmosphere. It is present in very low concentrations throughout the latter, with its highest concentration high in the ozone layer of the stratosphere, which absorbs most of the Sun's ultraviolet (UV) radiation.
Ozone's odour is reminiscent of chlorine, and detectable by many people at concentrations of as little as 0.1 ppm in air. Ozone's O3 structure was determined in 1865. The molecule was later proven to have a bent structure and to be diamagnetic. In standard conditions, ozone is a pale blue gas that condenses at progressively cryogenic temperatures to a dark blue liquid and finally a violet-black solid. Ozone's instability with regard to more common dioxygen is such that both concentrated gas and liquid ozone may decompose explosively at elevated temperatures or fast warming to the boiling point.
It is therefore used commercially only in low concentrations.
Ozone is a powerful oxidant (far more so than dioxygen) and has many industrial and consumer applications related to oxidation. This same high oxidising potential, however, causes ozone to damage mucous and respiratory tissues in animals, and also tissues in plants, above concentrations of about 0.1 ppm. While this makes ozone a potent respiratory hazard and pollutant near ground level, a higher concentration in the ozone layer (from two to eight ppm) is beneficial, preventing damaging UV light from reaching the Earth's surface.