Ozone - Wikipedia

Ozone - Wikipedia Jump to content Main menu Main menu move to sidebar hide Navigation Main page Contents Current events Random article About Wikipedia Contact us Contribute Help Learn to edit Community portal Recent changes Upload file Special pages Search Search Appearance Donate Create account Log in Personal tools Donate Create account Log in Contents move to sidebar hide (Top) 1 Nomenclature 2 History 3 Physical properties 4 Structure 5 Reactions Toggle Reactions subsection 5.1 With metals 5.2 With nitrogen and carbon compounds 5.3 With sulphur compounds 5.4 With alkenes and alkynes 5.5 Other substrates 5.6 Combustion 5.7 Ozone decomposition 5.7.1 Types of ozone decomposition 5.7.2 Kinetics of ozone decomposition into molecular oxygen 5.8 Reduction to ozonides 5.9 Applications 6 Spectroscopic properties 7 Ozone in Earth's atmosphere Toggle Ozone in Earth's atmosphere subsection 7.1 Ozone layer 7.1.1 Location and production 7.1.2 Importance to surface-dwelling life on Earth 7.2 Ground-level ozone 7.2.1 Ground-level ozone in urban areas 7.2.2 Ozone cracking 7.3 Ozone as a greenhouse gas 8 Carbon filtering 9 Health effects Toggle Health effects subsection 9.1 Vulnerable populations 9.2 Acute ozone exposure 9.3 Chronic ozone exposure 9.4 Ozone produced by air cleaners 9.5 Ozone air pollution 9.5.1 Heat waves 9.6 Physiology 9.7 Impact on plant growth and crop yields 9.8 Safety regulations 10 Production Toggle Production subsection 10.1 Corona discharge method 10.2 Ultraviolet light 10.3 Cold plasma 10.4 Electrolytic 10.5 Special considerations 10.6 Incidental production 10.7 Laboratory production 11 Applications Toggle Applications subsection 11.1 Industry 11.2 Water disinfection 11.3 Consumers 11.4 Aquaculture 11.5 Agriculture 11.6 Effect on pollinators 11.7 Alternative medicine 12 See also 13 References 14 Further reading 15 External links Toggle the table of contents Ozone 103 languages Afrikaans Aragonés अंगिका العربية অসমীয়া Asturianu Azərbaycanca تۆرکجه Башҡортса Беларуская (тарашкевіца) Беларуская Български भोजपुरी বাংলা Brezhoneg Bosanski Català کوردی Čeština Cymraeg Dansk Deutsch Ελληνικά Esperanto Español Eesti Euskara فارسی Suomi Français Frysk Gaeilge Galego ગુજરાતી עברית हिन्दी Hrvatski Hornjoserbsce Kreyòl ayisyen Magyar Հայերեն Jaku Iban Bahasa Indonesia Ido Íslenska Italiano 日本語 ქართული Қазақша ಕನ್ನಡ 한국어 Кыргызча Latina Lietuvių Latviešu Македонски മലയാളം मराठी Bahasa Melayu မြန်မာဘာသာ नेपाली Nederlands Norsk nynorsk Norsk bokmål Occitan Oromoo ଓଡ଼ିଆ ਪੰਜਾਬੀ Polski پنجابی پښتو Português Runa Simi Română Русский Русиньскый Scots Srpskohrvatski / српскохрватски Simple English Slovenčina Slovenščina Anarâškielâ Shqip Српски / srpski Sunda Svenska Kiswahili தமிழ் తెలుగు ไทย Tagalog Türkçe Українська اردو Oʻzbekcha / ўзбекча Tiếng Việt Winaray 吴语 IsiXhosa 閩南語 / Bân-lâm-gí 粵語中文 IsiZulu Edit links Article Talk English Read Edit View history Tools Tools move to sidebar hide Actions Read Edit View history General What links here Related changes Upload file Permanent link Page information Cite this page Get shortened URL Switch to legacy parser Print/export Download as PDF Printable version In other projects Wikimedia Commons Wikidata item Appearance move to sidebar hide From Wikipedia, the free encyclopedia Triatomic oxygen molecule For other uses, see Ozone (disambiguation). "Oxygen 3" redirects here. For the Jean-Michel Jarre album, see Oxygène 3. 4-trioxidiene; ''catena''-trioxygen"},"SystematicName":{"wt":"Trioxygen"},"Section1":{"wt":"{{Chembox Identifiers\n| IUPHAR_ligand = 6297\n| CASNo = 10028-15-6\n| CASNo_Ref = {{cascite|correct|CAS}}\n| PubChem = 24823\n| ChemSpiderID = 23208\n| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}\n| UNII = 66H7ZZK23N\n| UNII_Ref = {{fdacite|correct|FDA}}\n| EINECS = 233–069–2\n| MeSHName = Ozone\n| RTECS = RS8225000\n| ChEBI_Ref = {{ebicite|correct|EBI}}\n| ChEBI = 25812\n| Gmelin = 1101\n| SMILES = [O-][O+]=O\n| StdInChI = 1S/O3/c1-3-2\n| StdInChI_Ref = {{stdinchicite|correct|chemspider}}\n| InChI = 1/O3/c1-3-2\n| StdInChIKey = CBENFWSGALASAD-UHFFFAOYSA-N\n| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}\n| InChIKey = CBENFWSGALASAD-UHFFFAOYAY\n}}"},"Section2":{"wt":"{{Chembox Properties\n| Solvent = other solvents\n| O=3\n| Appearance = Colourless to pale blue gas<ref name=PGCH/>\n| Odour = Pungent, metallic, dry<ref name=PGCH/>\n| Density = 2.144 g/L (at 0 °C)\n| Solubility = 1.05 g L−1 (at 0 °C)\n| SolubleOther = Very soluble in [[carbon tetrachloride|CCl4]], [[sulphuric acid]], Slightly soluble in [[water]].\n| MeltingPtK = 81\n| BoilingPtK = 161\n| RefractIndex = 1.2226 (liquid), 1.00052 (gas, STP, 546 nm—note high dispersion)<ref>{{cite journal |last1=Cuthbertson |first1=Clive |last2=Cuthbertson |first2=Maude |date=1914 |title=On the Refraction and Dispersion of the Halogens, Halogen Acids, Ozone, Steam Oxides of Nitrogen, and Ammonia |url=https://archive.org/stream/philtrans08506476/08506476#page/n17/mode/1up |journal=[[Philosophical Transactions of the Royal Society A]] |volume=213 |issue=497–508 |pages=1–26 |bibcode=1914RSPTA.213....1C |doi=10.1098/rsta.1914.0001 |access-date=4 February 2016 |doi-access=free}}</ref>\n| VaporPressure = 55.7 atm<ref>Gas Encyclopedia; [https://encyclopedia.airliquide.com/ozone Ozone]</ref> ({{convert|−12.15|C|F K|disp=or}}){{efn|This vapor pressure is for the [[critical temperature]], which is below [[room temperature]].}}\n| MagSus = +6.7·10−6 cm3/mol\n| ConjugateAcid = [[Protonated ozone]]\n}}"},"Section3":{"wt":"{{Chembox Structure\n| SpaceGroup = C2v\n| Coordination = Digonal\n| MolShape = Dihedral\n| OrbitalHybridisation = ''sp''2 for O1\n| Dipole = 0.53 D\n}}"},"Section4":{"wt":"{{Chembox Thermochemistry\n| DeltaHf = 142.67 kJ mol−1\n| Entropy = 238.92 J K−1 mol−1\n}}"},"Section5":{"wt":"{{Chembox Hazards\n| GHSPictograms = {{GHS exploding bomb}}{{GHS flame over circle}}{{GHS gas cylinder}}{{GHS corrosion}}{{GHS skull and crossbones}}{{GHS exclamation mark}}{{GHS health hazard}}{{GHS environment}}\n| GHSSignalWord = Danger\n| HPhrases = {{H-phrases|270|314|330|335|341|361|370|410}}\n| PPhrases = {{P-phrases|203|220|244|260|264+265|270|271|273|280|284|301+330+331|302+361+354|304+340|305+351+338|308+316|362+364|370+376|391|403+233|405}}\n| NFPA-H = 4\n| NFPA-F = 0\n| NFPA-R = 4\n| NFPA-S = Ox\n| IDLH = 5 ppm<ref name=\"PGCH\">{{PGCH|0476}}</ref>\n| REL = C 0.1 ppm (0.2 mg/m3)<ref name=PGCH/>\n| PEL = TWA 0.1 ppm (0.2 mg/m3)<ref name=PGCH/>\n| LCLo = 12.6 ppm (mouse, 3 hr) 50 ppm (human, 30 min) 36 ppm (rabbit, 3 hr) 21 ppm (mouse, 3 hr) 21.8 ppm (rat, 3 hr) 24.8 ppm (guinea pig, 3 hr) 4.8 ppm (rat, 4 hr)<ref>{{IDLH|10028156|Ozone}}</ref>\n}}"},"Section6":{"wt":""},"Section8":{"wt":"{{Chembox Related\n| OtherCompounds = [[Sulphur dioxide]] [[Trisulphur]] [[Disulphur monoxide]] [[Cyclic ozone]]\n}}"}},"i":0}}]}'> Ozone Structural formula of ozone with partial charges shown Resonance structures of ozone with lone pairs indicated Ball and stick model of ozone Spacefill model of ozone Names IUPAC name Ozone Systematic IUPAC name Trioxygen Other names 2λ4-trioxidiene; catena-trioxygen Identifiers CAS Number 10028-15-6 Y 3D model (JSmol) Interactive image ChEBI CHEBI:25812 Y ChemSpider 23208 Y ECHA InfoCard 100.030.051 EC Number 233–069–2 Gmelin Reference 1101 IUPHAR/BPS 6297 MeSH Ozone PubChem Compound ID"}]]}'>CID 24823 RTECS number RS8225000 UNII 66H7ZZK23N Y CompTox Dashboard (U.S. Environmental Protection Agency"}]]}'>EPA) DTXSID0021098 InChI InChI=1S/O3/c1-3-2 Y Key: CBENFWSGALASAD-UHFFFAOYSA-N Y InChI=1/O3/c1-3-2 Key: CBENFWSGALASAD-UHFFFAOYAY SMILES [O-][O+]=O Properties Chemical formula O3 Molar mass 47.997 g·mol−1 Appearance Colourless to pale blue gas[1] Odor Pungent, metallic, dry[1] Density 2.144 g/L (at 0 °C) Melting point −192.2 °C; −313.9 °F; 81.0 K Boiling point −112 °C; −170 °F; 161 K Solubility in water 1.05 g L−1 (at 0 °C) Solubility in other solvents Very soluble in CCl4, sulphuric acid, Slightly soluble in water. Vapor pressure 55.7 atm[2] (−12.15 °C or 10.13 °F or 261.00 K)[a] Conjugate acid Protonated ozone Magnetic susceptibility (χ) +6.7·10−6 cm3/mol Refractive index (nD) 1.2226 (liquid), 1.00052 (gas, STP, 546 nm—note high dispersion)[3] Structure Space group C2v Coordination geometry Digonal Molecular shape Dihedral Hybridisation sp2 for O1 Dipole moment 0.53 D Thermochemistry Std molar entropy (S⦵298) 238.92 J K−1 mol−1 Std enthalpy of formation (ΔfH⦵298) 142.67 kJ mol−1 Hazards GHS labelling: Pictograms Signal word Danger Hazard statements H270, H314, H330, H335, H341, H361, H370, H410 Precautionary statements P203, P220, P244, P260, P264+P265, P270, P271, P273, P280, P284, P301+P330+P331, P302+P361+P354, P304+P340, P305+P351+P338, P308+P316, P362+P364, P370+P376, P391, P403+P233, P405 NFPA 704 (fire diamond) 4 0 4 OX Lethal dose or concentration (LD, LC): LCLo (lowest published) 12.6 ppm (mouse, 3 hr) 50 ppm (human, 30 min) 36 ppm (rabbit, 3 hr) 21 ppm (mouse, 3 hr) 21.8 ppm (rat, 3 hr) 24.8 ppm (guinea pig, 3 hr) 4.8 ppm (rat, 4 hr)[4] NIOSH (US health exposure limits): PEL (Permissible) TWA 0.1 ppm (0.2 mg/m3)[1] REL (Recommended) C 0.1 ppm (0.2 mg/m3)[1] IDLH (Immediate danger) 5 ppm[1] Related compounds Related compounds Sulphur dioxide Trisulphur Disulphur monoxide Cyclic ozone Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references Chemical compound Ozone (/ˈoʊzoʊn/ ⓘ), also called trioxygen, is an inorganic molecule with the chemical formula O 3. It is a pale-blue gas with a distinctively pungent odour. It is an allotrope of oxygen that is much less stable than the diatomic allotrope O 2, breaking down in the lower atmosphere to O 2 (dioxygen). Ozone is formed from dioxygen by the action of ultraviolet (UV) light and electrical discharges within the Earth's atmosphere. It is present in very low concentrations throughout the atmosphere, 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 weakly diamagnetic. At standard temperature and pressure, ozone is a pale blue gas that condenses at 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, physical shock, or fast warming to the boiling point.[5][6] It is therefore used commercially only in low concentrations. Ozone is a powerful oxidising agent (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 ei…