Nitrogen trichloride
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2008-07-03T23:16:17Z
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{{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>−1</sup>.mol<sup>−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> → 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]]