629-46-9

Basic information

• Product Name: octyl nitrite
• Synonyms: Nitrous acid, octyl ester; Octyl nitrite
• CAS NO: 629-46-9
• Molecular Formula: C₈H₁₇NO₂
• Molecular Weight: 159.2261
• EINECS: 211-092-9
• Mol File: 629-46-9.mol
• Article Data: 6

Chemical Properties

• Boiling Point: 174°C at 760 mmHg
• Flash Point: 43.1°C
• Density: 0.94g/cm³
• Vapor Pressure: 1.65mmHg at 25°C
• Refractive Index: 1.44
• CAS DataBase Reference: octyl nitrite(CAS DataBase Reference)
• NIST Chemistry Reference: octyl nitrite(629-46-9)
• EPA Substance Registry System: octyl nitrite(629-46-9)

Safety Data

• Hazardous Substances Data: 629-46-9(Hazardous Substances Data)

Usage

General Description

Octyl nitrite, also known as 1-nitrooxyoctane, is a chemical compound commonly used as an additive in the production of perfumes and colognes, as well as in the creation of artificial fruit flavors. It is a clear, pale yellow liquid with a fruity odor, and is highly flammable and volatile. Octyl nitrite is also known for its recreational use as a popper, where it is inhaled for its vasodilating effects and potential to enhance sexual experiences. However, its use in this manner is associated with numerous health risks and is illegal in many countries. The chemical is considered toxic and should be handled with caution, as inhalation or ingestion can lead to harmful effects on the central nervous system, cardiovascular system, and respiratory system.

Upstream product

• 111-87-5 octanol 
• 629-27-6 1-Iodooctane 
• 111-86-4 n-Octylamine 
• 111-83-1 1-bromo-octane 
• 111-88-6 Octanethiol 
• 68-12-2 N,N-dimethyl-formamide 
• 67-68-5 dimethyl sulfoxide 
• 60-29-7 diethyl ether 
• 157870-43-4 9,10-Bis(octyloxy)-1,4:5,8-dimethano-1,2,3,4,5,6,7,8-octahydroanthracene 
• 112-14-1 n-octyl acetate 

Downstream Products

• 111-87-5 octanol 
• 4887-30-3 n-octyl hexanoate 
• 94-50-8 n-octyl benzoate 

Relevant articles and documents

Novel and highly selective conversion of alcohols and thiols to alkyl nitrites with triphenylphosphine/2,3-dichloro-5,6-dicyanobenzoquinone/Bu 4NNO2 system

Alkyl nitrites were prepared in good to excellent yields by treatment of alcohols and thiols with triphenylphosphine/2,3-dichloro-5,6- dicyanobenzoquinone/Bu4NNO2 in acetonitrile. This method is highly selective for the conversion of primary alcohols to alkyl nitrites in the presence of secondary and tertiary alcohols and thiols.

Oxidative Dealkylation of Hydroquinone Ethers with Nitrogen Dioxide in the Convenient Preparation of Quinones

Various Hydroquinone dialkyl ethers (R2Q) are effectively converted by nitrogen dioxide into the corresponding quinone (Q) and alkyl nitrite (RONO) in dichloromethane at room temperature or below.The preparative procedure for the isolation of crystalline quinones in quantitative yield merely involves the convenient removal of the low boiling solvent in vacuo.Isotopic labelling studies demonstrate that the oxidative dealkylation proceeds via alkoxy scission of the labile cation radical (R2Q-cation radical) formed via the oxidation of the hydroquinone ether by nitrogen dioxide ( as the disproportionated ion pair NO+NO3-).The electron-transfer mechanism is confirmed by the spectral observation of R2Q-cation radical (identified by the isolation of the crystalline salt R2Q-cation radical-SbCl6-) and its rapid conversion into quinone and alkyl nitrite by combination with nitrate (NO3-) and nitric oxide (NO).

Proton Acidity and Chemical Reactivity in Molten Salt Hydrates

Molten Ca(NO3)2*4H2O has been used as a model system for studies of proton acidity and chemical reactions (including ester hydrolyses and aromatic nitrations) in molten salt hydrates.Increases in proton acidity caused by addition of acidic hydrates such as AlCl3*6H2O and Cd(NO3)2*4H2O or of aqueous HNO3 can be quantified in terms of changes in Hammett acidity H0, but usually not by the downfield shifts observed in the NMR spectrum.The rates of hydrolysis of selected primary esters (e.g., n-octyl acetate) were found to be linearly dependent on nitric acid concentration, indicating that the acidity of these melts can be changed with little change in water activity.The measurement of kinetic parameters is complicated, however, by side reactions between the organic substrates and HNO2, NO2 (or NO2+) and other species originating from the nitrate ions in the melt.