|Jmol-3D images||Image 1|
|Molar mass||120.37 g mol−1|
|Appearance||yellow oily liquid|
|Melting point||−40 °C (−40 °F; 233 K)|
|Boiling point||71 °C (160 °F; 344 K)|
|Solubility in water||immiscible
|Solubility||soluble in benzene, chloroform, CCl4, CS2, PCl3|
|Crystal structure||rhombohedral (below −40 °C)|
|Molecular shape||trigonal pyramidal|
|Dipole moment||0.6 D|
Std enthalpy of
|EU classification||not listed|
|Autoignition temperature||93 °C (199 °F; 366 K)|
|Other anions||Nitrogen trifluoride
|Other cations||Phosphorus trichloride
|Related compounds||Nitrosyl chloride|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
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.
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: Dogs that ate bread made from treated flour suffered epileptic-like fits; the toxic agent was methionine sulfoxide.
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
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 both got injured in an NCl3 explosion shortly thereafter.
In 2006, Belgian researchers reported a possible link between NCl3 and rising numbers of childhood asthma cases, in what they call the pool chlorine hypothesis, as an alternative to the hygiene hypothesis with a closer causal link.
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