Nitrosyl chloride

Nitrosyl chloride
Names
Preferred IUPAC name
Nitrosyl chloride
Systematic IUPAC name
Nitrooyl chloride
Other names
  • Nitrogen oxychloride
  • Nitrosonium chloride
  • Tildens Reagent
Identifiers
2696-92-6 YesY
3D model (Jmol) Interactive image
ChemSpider 16641 YesY
ECHA InfoCard 100.018.430
EC Number 220-273-1
E number E919 (glazing agents, ...)
MeSH nitrosyl+chloride
PubChem 17601
RTECS number QZ7883000
UN number 1069
Properties
NOCl
Molar mass 65.459 g mol−1
Appearance Yellow gas
Density 2.872 mg mL−1
Melting point −59.4 °C (−74.9 °F; 213.8 K)
Boiling point −5.55 °C (22.01 °F; 267.60 K)
Reacts
Structure
Dihedral, digonal
Hybridisation sp2 at N
1.90 D
Thermochemistry
261.68 J K−1 mol−1
51.71 kJ mol−1
Hazards
Safety data sheet inchem.org
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
0
3
1
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Nitrosyl chloride is the chemical compound with the formula NOCl. It is a yellow gas that is most commonly encountered as a decomposition product of aqua regia, a mixture of hydrochloric acid and nitric acid. It is a strong electrophile and oxidizing agent.

Structure and synthesis

The molecule is bent. A double bond exists between N and O (distance = 1.16 Å) and a single bond between N and Cl (distance = 1.69 Å). The O–N–Cl angle is 113°.[1]

Production

Since nitrosyl chloride is chemically simple and stable at room temperature and below, it can be produced in many ways.

HCl + NOHSO4H2SO4 + NOCl
HNO2 + HCl → H2O + NOCl
Pd + HNO3 + 3 HCl → PdCl2 + 2 H2O + NOCl
Cl2 + 2 NO → 2NOCl
N2 + O2 + Cl2 → 2 NOCl 2 NO + Cl2

Occurrence in aqua regia

NOCl also arises from the combination of hydrochloric and nitric acids according to the following reaction:[4]

HNO3 + 3 HCl → Cl2 + 2 H2O + NOCl

In nitric acid, NOCl is readily oxidized into nitrogen dioxide. The presence of NOCl in aqua regia was described by Edmund Davy in 1831.[5]

Reactions

NOCl behaves as an electrophile and an oxidant in most of its reactions. With halide acceptors, for example antimony pentachloride, converts to nitrosonium salts:

NOCl + SbCl5 → [NO]+[SbCl6]

In a related reaction, sulfuric acid gives nitrosylsulfuric acid, the mixed acid anhydride of nitrous and sulfuric acid:

ClNO + H2SO4 → ONHSO4 + HCl

NOCl reacts with silver thiocyanate to give silver chloride and the pseudohalogen nitrosyl thiocyanate:

ClNO + AgSCN → AgCl + ONSCN

Nitrosyl chloride is used to prepare metal nitrosyl complexes. With molybdenum hexacarbonyl, NOCl gives the dinitrosyldichloride complex:[6]

Mo(CO)6 + 2 NOCl → MoCl2(NO)2 + 6 CO

Applications in organic synthesis

Aside from its role in the production of caprolactam, NOCl finds some other uses In organic synthesis. It adds to alkenes to afford α-chloro oximes.[7] The initial addition of NOCl follows the Markovnikov rule. Ketenes also add NOCl, giving nitrosyl derivatives:

H2C=C=O + NOCl → ONCH2C(O)Cl

Propylene oxide also undergoes electrophilic addition with NOCl to give an α-chloronitritoakyl derivative:

It converts amides to N-nitroso derivatives.[8] NOCl converts some cyclic amines to the alkenes. For example, aziridine reacts with NOCl to give ethene, nitrous oxide and hydrogen chloride.

Industrial applications

NOCl and cyclohexane react photochemically to give cyclohexanone oxime hydrochloride. This process exploits the tendency of NOCl to undergo photodissociation into NO and Cl radicals. The oxide is converted to caprolactam, a precursor to Nylon-6.[2]

Safety

Nitrosyl chloride is very toxic and irritating to the lungs, eyes, and skin. Use safety mask while working with this chemical.

References

  1. Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 0-12-352651-5.
  2. 1 2 Ritz, Josef; Fuchs, Hugo; Kieczka, Heinz; Moran, William C. (2002). "Caprolactam". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a05_031.
  3. Morton, J. R.; Wilcox, H. W. (1953). "Nitrosyl Chloride". Inorganic Syntheses. 48: 52. doi:10.1002/9780470132357.ch16.
  4. Beckham, L. J.; Fessler, W. A.; Kise, M. A. (1951). "Nitrosyl Chloride". Chemical Reviews. 48 (3): 319–396. doi:10.1021/cr60151a001.
  5. Edmund Davy (1830–1837). "On a New Combination of Chlorine and Nitrous Gas. [Abstract]". Abstracts of the Papers Printed in the Philosophical Transactions of the Royal Society of London,. JSTOR. 3: 27–29. JSTOR 110250.
  6. Johnson, B. F. G.; Al-Obadi, K. H. (1970). "Dihalogenodinitrosylmolybdenum and Dihalogenodinitrosyltungsten". Inorg. Synth. 12: 264–266. doi:10.1002/9780470132432.ch47.
  7. Ohno, M.; Naruse, N.; Terasawa, I. (1973). "7-cyanoheptanal". Org. Synth.; Coll. Vol., 5, p. 266
  8. Van Leusen, A. M.; Strating, J. (1977). "p-Tolylsulfonyldiazomethane". Org. Synth. 57: 95. doi:10.15227/orgsyn.057.0095.
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