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|Other names||2λ4-trioxidiene; catena-trioxygen|
|Molar mass||47.98 g mol-1|
|Appearance||Colourless to pale blue gas<|
|Density||2.144 mg cm−3 (at 0 °C)|
-192 °C, 81 K, -314 °F
-112 °C, 161 K, -170 °F
|Solubility in water||1.05 g L−1 (at 0 °C)|
|Solubility in other solvents||Very soluble in CCl4, sulfuric acid|
|Vapor pressure||55.7 atm (−12.15 °C or 10.13 °F; 261.00 K)[a]|
|Refractive index (nD)||1.2226 (liquid), 1.00052 (gas, STP, 546 nm — note high dispersion)|
|Hybridisation||sp2 for O1|
|Dipole moment||0.53 D|
| Std enthalpy of
|142.67 kJ mol−1|
| Standard molar
|238.92 J K−1 mol−1|
| U.S. Permissible
exposure limit (PEL)
|TWA 0.1 ppm (0.2 mg/m3)|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)|
Ozone, or trioxygen, is a chemical with the symbol O3. This means one molecule of ozone is made of three oxygen atoms. Ozone is rarely called trioxygen, even though this is its IUPAC systematic name. Ozone is formed from oxygen gas (O2) by the action of ultraviolet light and also atmospheric electrical discharges. It is present in low concentrations throughout the Earth's atmosphere. In total, ozone makes up only 0.6 ppm (parts per million) of the atmosphere by volume.
Ozone is important to life on planet Earth. There is a portion of the stratosphere with a high concentration of ozone, called the ozone layer. The ozone layer filters out damaging ultraviolet radiation from the Sun, like a kind of sun screen. Without this ozone layer things would not have been able to live on the surface of our planet. The ozone layer also absorbs a lot of heat from the sun's rays.
However, ozone is toxic to animals and plants above concentrations of about 0.1 ppm. In humans, it can cause nasal and throat irritation, and nausea. Extended exposure can cause lung oedema. 0.100 ppm is the maximum allowable limit for industrial, public, or occupied spaces in England, Japan, France, the Netherlands and Germany. The Ozone layer is in the 10 to 50 kilometer range of the Earth's atmosphere.
- Gas Encyclopedia; Ozone
- Cuthbertson, Clive; Cuthbertson, Maude (1914). "On the Refraction and Dispersion of the Halogens, Halogen Acids, Ozone, Steam Oxides of Nitrogen, and Ammonia". Philosophical Transactions of the Royal Society A 213 (497–508): 1–26. . https://archive.org/stream/philtrans08506476/08506476#page/n17/mode/1up. Retrieved 4 February 2016.
- Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005. RSC Publishing. 2005. IR-3.4.3. . http://old.iupac.org/publications/books/rbook/Red_Book_2005.pdf. Retrieved 16 June 2020. "7. Formula ... O3 ... Systematic name ... trinitrogen ... Acceptable alternative name ... ozone".
- "Stratospheric ozone". Ministry for the Environment (New Zealand). 2013-07-18. https://www.mfe.govt.nz/environmental-reporting/atmosphere/levels-stratospheric-ozone-indicator/report-card-2012.html. Retrieved 2014-03-03.
- "Ozone Safety Limits". Understanding Ozone. http://www.understandingozone.com/limits.asp. Retrieved 2013-11-21.