Nitrogen trichloride

Nitrogen trichloride

Structural formula of nitrogen trichloride Space-filling model of nitrogen trichloride
Nitrogen trichloride
Names
Other names Trichloramine Agene Nitrogen(III) chloride Trichloroazane Trichlorine nitride
Identifiers
CAS Number	10025-85-1 N
ChEBI	CHEBI:37382 Y
ChemSpider	55361 Y
EC Number	233-045-1
Jmol 3D model	Interactive image
PubChem	61437
RTECS number	QW974000
InChI InChI=1S/Cl3N/c1-4(2)3 Y Key: QEHKBHWEUPXBCW-UHFFFAOYSA-N Y InChI=1/Cl3N/c1-4(2)3 Key: QEHKBHWEUPXBCW-UHFFFAOYAZ
SMILES ClN(Cl)Cl
Properties
Chemical formula	Cl3N
Molar mass	120.36 g·mol−1
Appearance	yellow oily liquid
Odor	chlorine-like
Density	1.653 g/mL
Melting point	−40 °C (−40 °F; 233 K)
Boiling point	71 °C (160 °F; 344 K)
Solubility in water	immiscible slowly decomposes
Solubility	soluble in benzene, chloroform, CCl4, CS2, PCl3
Structure
Crystal structure	orthorhombic (below −40 °C)
Molecular shape	trigonal pyramidal
Dipole moment	0.6 D
Thermochemistry
Std enthalpy of formation (ΔfHo298)	232 kJ/mol
Vapor pressure	{{{value}}}
Related compounds
Other anions	Nitrogen trifluoride Nitrogen tribromide Nitrogen triiodide
Other cations	Phosphorus trichloride Arsenic trichloride
Related chloramines	Chloramine Dichloramine
Related compounds	Nitrosyl chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Nitrogen trichloride, also known as trichloramine, is the chemical compound with the formula NCl₃. This yellow, oily, pungent-smelling liquid is most commonly encountered as a byproduct of chemical reactions between ammonia-derivatives and chlorine (for example, in swimming pools).

Preparation and structure

The compound is prepared by treatment of ammonium salts, such as ammonium nitrate with chlorine.

Intermediates in this conversion include chloramine and dichloramine, NH₂Cl and NHCl₂, respectively.

Like ammonia, NCl₃ 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 from bathers. Nitrogen trichloride, trademarked as Agene, was used to artificially bleach and age flour, but was banned in 1949: In humans Agene was found to cause severe and widespread neurological disorders leading to its banning in 1947. Dogs that ate bread made from treated flour suffered epileptic-like fits; the toxic agent was methionine sulfoximine.

Reactions

Despite the similarities of the Pauling electronegativities of nitrogen and chlorine, this molecule has moderate polarity with negative charges residing on nitrogen. So the nitrogen in NCl₃ is often considered to have the −3 oxidation state and the chlorine atoms are considered to be in the +1 oxidation state.
It is hydrolyzed by hot water to release ammonia and hypochlorous acid.

NCl₃ + 3 H₂O → NH₃ + 3 HOCl

Safety

Nitrogen trichloride can irritate mucous membranes—it is a lachrymatory agent, but has never been used as such. The pure substance (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 two fingers and an eye in two explosions. In 1813, an NCl₃ explosion blinded Sir Humphry Davy temporarily, inducing him to hire Michael Faraday as a co-worker. They were both injured in another NCl₃ explosion shortly thereafter.

See also

• List of food contamination incidents

External links

• OSHA - Nitrogen trichloride
• Nitrogen Trichloride - Health References