Nitrogen trichloride
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| Other names | Trichloramine Agene Nitrogen(III) chloride Trichloroazane |
| Identifiers | |
| CAS number | [10025-85-1] |
| RTECS number | QW974000 |
| Properties | |
| Molecular formula | NCl3 |
| Molar mass | 120.36 g/mol |
| Appearance | yellow oily liquid |
| Density | 1.635 g/mL, liquid |
| Melting point |
-40 °C (233 K) |
| Boiling point |
71 °C (344 K) |
| Solubility in water | Immiscible slowly decomposes |
| Viscosity | ? mPa·s at ? °C |
| Structure | |
| Molecular shape | trigonal pyramidal |
| Dipole moment | 0.6 D |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
+232 kJ/mol |
| Standard molar entropy S |
? J.K−1.mol−1 |
| Hazards | |
| EU classification | not listed |
| NFPA 704 |
 0
2
4
OX
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| 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 noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Nitrogen trichloride, also known as trichloramine, trichlorine nitride 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.[citation needed]
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[edit] Preparation and structure
The compound is prepared by treatment of ammonium salts, such as ammonium nitrate with 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 electronegativities are very similar for nitrogen (3.04) and chlorine (3.16).
[edit] 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]
[edit] References
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ 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).
[edit] 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): 639. doi:.
- 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): 82. doi:.
- 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).
