from Wikipedia
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 between disinfecting chlorine and urea in urine from bathers). In pure form, NCl3 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 teargas.
Preparation and structure
The compound is prepared by treatment of ammonium salts, such as ammonium nitratewith chlorine:
- 4 NH3 + 3 Cl2 → NCl3 + 3 NH4Cl
Intermediates in this coversion include chloramine and dichloramine, NH2Cl and NHCl2, respectively.
Like ammonia, NCl3 is a pyramidal molecule. The N-Cl distances are 1.76 Â, and the Cl-N-Cl angles are 107°.[1] The electronegativitiesare 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 NCl3 blinded Sir Humphry Davy temporarily, inducing him to hire Michael Faraday as a coworker. Belgian researchers reported a possible link between NCl3 and rising numbers of childhood asthma cases.[2]
References
2. ^ Bernard A, Carbonnelle S, de Burbure C, Michel O, Nickmilder M (2006). “Chlorinated pool attendance, atopy, and the risk of asthma during childhood“. Environmental Health Perspectives 114 (10).
Further reading
- Jander, J. (1976). Adv. Inorg. Chem. Radiochem. 19: 2.
- P. Kovacic, M. K. Lowery, K. W. Field (1970). “Chemistry of N-bromamines and N-chloramines”. Chemical Reviews 70 (6). DOI:10.1021/cr60268a002.
- Hartl, H.;, Schoner, J.; Jander, J.; Schulz, H. (1975). “Structure of Solide Nitrogen-Trichloride (-125°C)”. Zeitschrift für Anorganische und Allgemeine Chemie 413 (1).
- Cazzoli, G.; Favero, P. G.; Dalborgo, A. (1974). “Molecula-Structure, Nuclear-Quadruple Coupling-Constant and Dipole-Moment of Nitrogen Trichloride from Microwave Spectroscopy”. Journal of Molecular Spectroscopy 50 (1-3).
- Bayersdo, L.; Engelhar, U., Fischer, J.; Hohne, K.; Jander, J. (1969). “Nitrogen-chlorine compounds: Infrared spectra and Raman spectra of nitrogen trichloride”. Zeitschrift für anorganische und allgemeine Chemie 366 (3-4).
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Posted by Why that 'clean swimming pool' smell is actually bad for your health - StuntFM 97.3 on March 3, 2017 at 11:52 am
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Posted by Why That Clean Swimming Pool Smell Is Actually Bad For Your Health - Get Well Naturally on March 7, 2017 at 11:41 pm
[…] Nitrogen trichloride, also known as trichloramine, is made when the urea in your pee reacts with chlorine the disinfectant widely used in swimming pool water. Nitrogen trichloride is largely made by accident in pools these days, but this compound was originally made for interest in 1812 by Pierre Louis DuLong. […]