Nitrogen trichloride 1041015 223408726 2008-07-03T23:16:17Z DOI bot 6652755 Citation maintenance. Formatted: doi. You can [[WP:DOI|use this bot]] yourself! Please [[User:DOI_bot/bugs|report any bugs]]. {{Chembox new | Name = Nitrogen trichloride | ImageFile = Nitrogen-trichloride-2D.png | ImageSize = 100px | ImageName = Nitrogen trichloride | ImageFile1 = Nitrogen-trichloride-3D-vdW.png | ImageSize1 = 100px | ImageName1 = Nitrogen trichloride | OtherNames = Trichloramine<br />Agene<br />Nitrogen(III) chloride<br />Trichloroazane | Name = '''Safety data''' | Section1 = {{Chembox Identifiers | CASNo = 10025-85-1 | RTECS = QW974000 }} | Section2 = {{Chembox Properties | Formula = NCl<sub>3</sub> | MolarMass = 120.36 g/mol | Appearance = yellow oily liquid | Density = 1.635 g/mL, liquid | Solubility = Immiscible<br />slowly decomposes | MeltingPt = -40 °C (233 K) | BoilingPt = 71 °C (344 K) | Viscosity = ? [[pascal second|mPa·s]] at ? °C }} | Section3 = {{Chembox Structure | MolShape = trigonal pyramidal | Dipole = 0.6 [[Debye|D]] }} | Section4 = {{Chembox Thermochemistry | DeltaHf = +232 kJ/mol | Entropy = ? J.K<sup>&minus;1</sup>.mol<sup>&minus;1</sup> }} | Section7 = {{Chembox Hazards | EUClass = not listed | NFPA-H = 2 | NFPA-F = 0| NFPA-R = 4 | NFPA-O = Ox }} | Section8 = {{Chembox Related | OtherAnions = [[Nitrogen trifluoride]]<br />[[Nitrogen tribromide]]<br />[[Nitrogen triiodide]] | OtherCations = [[Phosphorus trichloride]]<br />[[Arsenic trichloride]] | Function = [[chloramine]]s | OtherFunctn = [[Chloramine]]<br />[[Dichloramine]] | OtherCpds = [[Nitrosyl chloride]]}} }} '''Nitrogen trichloride''', also known as '''trichloramine''', '''trichlorine nitride''' is the [[chemical compound]] with the [[chemical formula|formula]] NCl<sub>3</sub>. This yellow, oily, pungent-smelling liquid is most commonly encountered as a byproduct of [[chemical reaction]]s between [[ammonia]]-derivatives and [[chlorine]] (for example, in [[swimming pool]]s between disinfecting chlorine and [[urea]] in urine from bathers). In pure form, NCl<sub>3</sub> is highly reactive. Nitrogen trichloride can form in small amounts when public water supplies are disinfected with [[monochloramine]]. Nitrogen trichloride was trademarked as '''Agene''' and used to artificially bleach and age [[flour]]. It has been used as a [[Lachrymatory_agent|tear gas]].{{Fact|date=May 2008}} ==Preparation and structure== The compound is prepared by treatment of ammonium salts, such as [[ammonium nitrate]] with chlorine: :4 NH<sub>3</sub> + 3 Cl<sub>2</sub> &rarr; NCl<sub>3</sub> + 3 NH<sub>4</sub>Cl Intermediates in this coversion include [[chloramine]] and [[dichloramine]], NH<sub>2</sub>Cl and NHCl<sub>2</sub>, respectively. Like ammonia, NCl<sub>3</sub> is a pyramidal molecule. The N-Cl distances are 1.76 Â, and the Cl-N-Cl angles are 107°.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> The [[electronegativity|electronegativities]] are very similar for nitrogen (3.04) and chlorine (3.16). ==Safety== Nitrogen trichloride is a dangerous explosive, being sensitive to light, heat, and organic compounds. [[Pierre Louis Dulong]] first prepared it in 1812, and lost two fingers and an eye in two separate explosions. An explosion from NCl<sub>3</sub> blinded Sir [[Humphry Davy]] temporarily, inducing him to hire [[Michael Faraday]] as a coworker. Belgian researchers reported a possible link between NCl<sub>3</sub> and rising numbers of childhood [[asthma]] cases.<ref> {{cite journal | title = Chlorinated pool attendance, atopy, and the risk of asthma during childhood | author= Bernard A, Carbonnelle S, de Burbure C, Michel O, Nickmilder M | journal= Environmental Health Perspectives | year= 2006 | volume = 114 | issue= 10 |url =http://www.ehponline.org/members/2006/8461/8461.pdf | pages = 1567–1573 }}</ref> ==References== <references/> ==Further reading==<!-- would be nice to have titles! and ISBNs--> *Jander, J. (1976). ''Adv. Inorg. Chem. Radiochem.'' '''19''': 2. *{{cite journal | title = Chemistry of N-bromamines and N-chloramines | author= P. Kovacic, M. K. Lowery, K. W. Field | journal= Chemical Reviews | year= 1970 | volume = 70 | issue= 6 | doi = 10.1021/cr60268a002| pages = 639 }} *{{cite journal | title = Structure of Solide Nitrogen-Trichloride (-125°C) | author= Hartl, H.;, Schoner, J.; Jander, J.; Schulz, H. | journal= Zeitschrift für Anorganische und Allgemeine Chemie | year= 1975 | volume = 413 | issue= 1 | pages = 61–71 | doi = 10.1002/zaac.19754130108 }} *{{cite journal | title = Molecula-Structure, Nuclear-Quadruple Coupling-Constant and Dipole-Moment of Nitrogen Trichloride from Microwave Spectroscopy | author= Cazzoli, G.; Favero, P. G.; Dalborgo, A. | journal= Journal of Molecular Spectroscopy | year= 1974 | volume = 50 | issue= 1-3 | pages = 82 | doi = 10.1016/0022-2852(74)90219-7 }} *{{cite journal | title = Nitrogen-chlorine compounds: Infrared spectra and Raman spectra of nitrogen trichloride | author= Bayersdo, L.; Engelhar, U., Fischer, J.; Hohne, K.; Jander, J. | journal= Zeitschrift für anorganische und allgemeine Chemie | year= 1969 | volume = 366 | issue= 3-4 | pages = 169- | doi = 10.1002/zaac.19693660308 }} ==External links== * [http://www.osha.gov/dts/chemicalsampling/data/CH_257450.html OSHA - Nitrogen trichloride] [[Category:Nitrogen compounds]] [[Category:Chlorides]] [[Category:Nonmetal halides]] [[de:Stickstofftrichlorid]] [[fr:Trichlorure d'azote]] [[hr:Dušikov triklorid]] [[lt:Azoto trichloridas]] [[hu:Nitrogén-triklorid]] [[nl:Stikstoftrichloride]] [[ja:塩化窒素]] [[pt:Tricloreto de nitrogênio]]