Names | |
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IUPAC name
Nitrosyl chloride[citation needed]
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Identifiers | |
3D model (JSmol)
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ChemSpider | |
ECHA InfoCard | 100.018.430 |
EC Number |
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E number | E919 (glazing agents, ...) |
MeSH | nitrosyl+chloride |
PubChem CID
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RTECS number |
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UNII | |
UN number | 1069 |
CompTox Dashboard (EPA)
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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 | |
Std molar
entropy (S⦵298) |
261.68 J K−1 mol−1 |
Std enthalpy of
formation (ΔfH⦵298) |
51.71 kJ mol−1 |
Hazards | |
NFPA 704 (fire diamond) | |
Safety data sheet (SDS) | inchem.org |
Related compounds | |
Related compounds
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Nitrosyl chloride is the chemical compound with the formula NOCl. It is a yellow gas that is commonly encountered as a component of aqua regia, a mixture of 3 parts concentrated hydrochloric acid and 1 part of concentrated nitric acid. It is a strong electrophile and oxidizing agent. It is sometimes called Tilden's reagent, after William A. Tilden, who was the first to produce it as a pure compound.[1]
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 = 1.96 Å). The O=N–Cl angle is 113°.[2]
Nitrosyl chloride can be produced in many ways.
NOCl also arises from the combination of hydrochloric and nitric acids according to the following reaction:[6]
In nitric acid, NOCl is readily oxidized into nitrogen dioxide. The presence of NOCl in aqua regia was described by Edmund Davy in 1831.[7]
NOCl behaves as an electrophile and an oxidant in most of its reactions. With halide acceptors, for example antimony pentachloride, converts to nitrosonium salts:
In a related reaction, sulfuric acid gives nitrosylsulfuric acid, the mixed acid anhydride of nitrous and sulfuric acid:
NOCl reacts with silver thiocyanate to give silver chloride and the pseudohalogen nitrosyl thiocyanate:
Similarly, it reacts with silver cyanide to give nitrosyl cyanide.[8]
Nitrosyl chloride is used to prepare metal nitrosyl complexes. With molybdenum hexacarbonyl, NOCl gives the dinitrosyldichloride complex:[9]
It dissolves platinum:[10]
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.[11] The addition of NOCl follows the Markovnikov rule. Ketenes also add NOCl, giving nitrosyl derivatives:
Epoxides react with NOCl to give an α-chloronitritoalkyl derivatives. In the case of propylene oxide, the addition proceeds with high regiochemistry:[12]
It converts amides to N-nitroso derivatives.[13] NOCl converts some cyclic amines to the alkenes. For example, aziridine reacts with NOCl to give ethene, nitrous oxide and hydrogen chloride.
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 cyclohexanone oxime is converted to caprolactam, a precursor to nylon-6.[3]
Before the advent of modern spectroscopic methods for chemical analysis, informative chemical degradation and structure elucidation required the characterization of the individual components of various extracts. Notably, the aforementioned introduction of nitrosyl chloride by Tilden in 1875, as a reagent for producing crystalline derivatives of terpenes, e.g. α-pinene from oil of turpentine allowed investigators to readily distinguish one terpene from another.:[14]
Nitrosyl chloride is very toxic and irritating to the lungs, eyes, and skin.
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