Nitrogen trichloride

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Nitrogen trichloride

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EC Number	Template:Unbulleted list
Template:Longitem	1840
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Template:Longitem	Template:Chem2
Molar mass	Template:Chem molar mass
Appearance	yellow oily liquid
Odor	chlorine-like
Density	1.653 g/mL
Melting point	Template:Chembox CalcTemperatures
Boiling point	Template:Chembox CalcTemperatures
Solubility	soluble in benzene, chloroform, [[carbon tetrachloride|Template:Chem2]], [[carbon disulfide|Template:Chem2]], [[phosphorus trichloride|Template:Chem2]]
Template:Longitem	orthorhombic (below −40 °C)
Template:Longitem	trigonal pyramidal
Template:Longitem	0.6 D
Template:Longitem	232 kJ/mol
NFPA 704 (fire diamond)	Template:NFPA 704 diamond
Template:Longitem	Template:Chembox CalcTemperatures
Template:Longitem	Nitrogen trifluoride Nitrogen tribromide Nitrogen triiodide
Template:Longitem	Phosphorus trichloride Arsenic trichloride
Template:Longitem	Monochloramine Dichloramine
Template:Longitem	Nitrosyl chloride

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.

Preparation and occurrence

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. 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, but this practice was banned in the United States in 1949 due to safety concerns.

Structure and properties

Like ammonia, Template:Chem2 is a pyramidal molecule. The N-Cl distances are 1.76 Å, and the Cl-N-Cl angles are 107°.

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 uses

The chemistry of Template:Chem2 has been well explored. 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.

$\mathrm{N}\mathrm{C}\mathrm{l}{\phantom{A}}_3+3\mathrm{H}{\phantom{A}}_2\mathrm{O}⟶\mathrm{N}\mathrm{H}{\phantom{A}}_3+3\mathrm{H}\mathrm{C}\mathrm{l}\mathrm{O}$

Concentrated samples of NCl₃ can explode to give N₂ and chlorine gas.

$2\mathrm{N}\mathrm{C}\mathrm{l}{\phantom{A}}_3⟶\mathrm{N}{\phantom{A}}_2+3\mathrm{C}\mathrm{l}{\phantom{A}}_2$

In the presence of aluminium trichloride, NCl₃ reacts with some branched hydrocarbons to produce, after a hydrolysis step, amines.

Safety

Nitrogen trichloride can irritate mucous membranes

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Template:Redirect category shellit is a lachrymatory agent, but has never been used as such. 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. 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.

See also

• List of food contamination incidents
• Nitrogen tribromide
• Nitrogen triiodide

External links

• OSHA - Nitrogen trichloride
• Nitrogen Trichloride - Health References