Ozone

From Wikipedia, the free encyclopedia
Jump to navigation Jump to search
Ozone
Ball and stick model of ozone
Spacefill model of ozone
Names
IUPAC name
Trioxygen
Other names
4-trioxidiene; catena-trioxygen
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.030.051
EC Number 233–069–2
Gmelin Reference 1101
MeSH {{{value}}}
PubChem {{{value}}}
RTECS number RS8225000
UNII
SMILES {{{value}}}
Properties
O3
Molar mass 48.00 g·mol−1
Appearance Colourless to pale blue gas<
Odor Pungent
Density 2.144 mg cm−3 (at 0 °C)
Melting point −192.2 °C; −313.9 °F; 81.0 K
Boiling point −112 °C; −170 °F; 161 K
1.05 g L−1 (at 0 °C)
Solubility in other solvents Very soluble in CCl4, sulfuric acid
Vapor pressure 55.7 atm[1] (−12.15 °C or 10.13 °F or 261.00 K)[a]
+6.7·10−6 cm3/mol
1.2226 (liquid), 1.00052 (gas, STP, 546 nm — note high dispersion)[2]
Structure
C2v
Digonal
Dihedral
Hybridisation sp2 for O1
0.53 D
Thermochemistry
Std enthalpy of
formation
ΔfHo298
142.67 kJ mol−1
Standard molar
entropy
So298
238.92 J K−1 mol−1
Hazards
NFPA 704

NFPA 704.svg

0
4
4
 
U.S. Permissible
exposure limit (PEL)
TWA 0.1 ppm (0.2 mg/m3)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

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[3]. 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,[4] 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.[5] Extended exposure can cause lung oedema.[5] 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.[5]

References[change | change source]

  1. Gas Encyclopedia; Ozone
  2. 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. Bibcode:1914RSPTA.213....1C. doi:10.1098/rsta.1914.0001. Retrieved 4 February 2016.
  3. Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005 (PDF). RSC Publishing. 2005. IR-3.4.3. ISBN 0-85404-438-8. Archived from the original (PDF) on 2019-12-19. Retrieved 16 June 2020. 7. Formula ... O3 ... Systematic name ... trinitrogen ... Acceptable alternative name ... ozone
  4. "Stratospheric ozone". Ministry for the Environment (New Zealand). 2013-07-18. Retrieved 2014-03-03.
  5. 5.0 5.1 5.2 "Ozone Safety Limits". Understanding Ozone. Retrieved 2013-11-21.

Notes

  1. This vapor pressure is for the critical temperature, which is below room temperature.