Nitrogen trichloride
Template:Short description Template:Chembox Nitrogen trichloride, also known as trichloramine, is the chemical compound with the formula Template:Chem2. This yellow, oily, and explosive liquid is most commonly encountered as a product of chemical reactions between ammonia-derivatives and chlorine (for example, in swimming pools). Alongside monochloramine and dichloramine, trichloramine is responsible for the distinctive 'chlorine smell' associated with swimming pools, where the compound is readily formed as a product from hypochlorous acid reacting with ammonia and other nitrogenous substances in the water, such as urea from urine.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>
Preparation and occurrenceEdit
The compound is generated by treatment of ammonium chloride with calcium hypochlorite. When prepared in an aqueous-dichloromethane mixture, the trichloramine is extracted into the nonaqueous phase.<ref name=OS>Template:Cite journal</ref> Intermediates in this conversion include monochloramine and dichloramine, Template:Chem2 and Template:Chem2, respectively.
Nitrogen trichloride, trademarked as Agene, was at one time used to bleach flour,<ref>Template:Cite journal</ref> but this practice was banned in the United States in 1949 due to safety concerns.
Structure and propertiesEdit
Like ammonia, Template:Chem2 is a pyramidal molecule. The N-Cl distances are 1.76 Å, and the Cl-N-Cl angles are 107°.<ref>Template:Cite book</ref>
Nitrogen trichloride can form in small amounts when public water supplies are disinfected with monochloramine, and in swimming pools by disinfecting chlorine reacting with urea in urine and sweat from bathers.
Reactions and usesEdit
The chemistry of Template:Chem2 has been well explored.<ref>Template:Greenwood&Earnshaw2nd</ref> It is moderately polar with a dipole moment of 0.6 D. The nitrogen center is basic but much less so than ammonia. It is hydrolyzed by hot water to release ammonia and hypochlorous acid.
Concentrated samples of NCl3 can explode to give N2 and chlorine gas.Template:Cn
In the presence of aluminium trichloride, NCl3 react with some branch hydrocarbon to produce, after a hydrolysis step, amines.<ref name=OS/>
SafetyEdit
Nitrogen trichloride can irritate mucous Template:Nowrapit is a lachrymatory agent, but has never been used as such.<ref>Template:Cite book</ref><ref>Template:Cite journal</ref> The compound (rarely encountered) is a dangerous explosive, being sensitive to light, heat, even moderate shock, and organic compounds. Pierre Louis Dulong first prepared it in 1812, and lost several fingers and an eye in two explosions.<ref>Template:Cite journal</ref> In 1813, an Template:Chem2 explosion blinded Sir Humphry Davy temporarily, inducing him to hire Michael Faraday as a co-worker. They were both injured in another Template:Chem2 explosion shortly thereafter.<ref name="Thomas1991">Template:Cite book</ref>
See alsoEdit
ReferencesEdit
Further readingEdit
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External linksEdit
Template:Nitrogen compounds Template:Chlorine compounds Template:Nitrides Template:Chlorides