3252-43-5

Basic information

• Product Name: DIBROMOACETONITRILE
• Synonyms: dibromo-acetonitril;DIBROMOACETONITRILE;DIBROMMETHYLCYANIDE;DIBROMOACETONITRILE, 1000MG, NEAT;Acetonitrile, dibromo-;dibrommethylcyanid;Dibromoacetonitrile,99%;Dibromoacetonitrile,97%
• CAS NO: 3252-43-5
• Molecular Formula: C₂HBr₂N
• Molecular Weight: 198.84
• EINECS: 221-843-2
• Product Categories: Aromatic Nitriles;Alpha Sort;BromoVolatiles/ Semivolatiles;Chemical Class;D;DAlphabetic;DIA - DIC;Halogenated
• Mol File: 3252-43-5.mol
• Article Data: 3

Chemical Properties

• Boiling Point: 67-69 °C (24 mmHg)
• Flash Point: 37°C
• Appearance: /
• Density: 2.29
• Vapor Pressure: 2.1mmHg at 25°C
• Refractive Index: 1.538-1.543
• Storage Temp.: 0-6°C
• Sensitive: Light Sensitive
• BRN: 1739037
• CAS DataBase Reference: DIBROMOACETONITRILE(CAS DataBase Reference)
• NIST Chemistry Reference: DIBROMOACETONITRILE(3252-43-5)
• EPA Substance Registry System: DIBROMOACETONITRILE(3252-43-5)

Safety Data

• Hazard Codes: Xn,T
• Statements: 20/21/22-36-22
• Safety Statements: 36/37-26
• RIDADR: 3275
• WGK Germany: 3
• RTECS: AL8450000
• TSCA: T
• HazardClass: 3
• PackingGroup: III
• Hazardous Substances Data: 3252-43-5(Hazardous Substances Data)

Usage

Chemical Properties

Clear colorless to yellow liquid

General Description

Clear amber oily liquid.

Air & Water Reactions

DIBROMOACETONITRILE may be sensitive to prolonged exposure to air and light. Slightly soluble in water.

Reactivity Profile

DIBROMOACETONITRILE is incompatible with strong acids, strong bases, strong oxidizing agents and strong reducing agents. . Nitriles may polymerize in the presence of metals and some metal compounds. They are incompatible with acids; mixing nitriles with strong oxidizing acids can lead to extremely violent reactions. Nitriles are generally incompatible with other oxidizing agents such as peroxides and epoxides. The combination of bases and nitriles can produce hydrogen cyanide. Nitriles are hydrolyzed in both aqueous acid and base to give carboxylic acids (or salts of carboxylic acids). These reactions generate heat. Peroxides convert nitriles to amides. Nitriles can react vigorously with reducing agents. Acetonitrile and propionitrile are soluble in water, but nitriles higher than propionitrile have low aqueous solubility. They are also insoluble in aqueous acids.

Fire Hazard

Literature sources indicate that DIBROMOACETONITRILE is nonflammable.

Safety Profile

Poison by intravenous route. Questionable carcinogen with experimental carcinogenic data. Experimental reproductive effects. Human mutation data reported. See also NITRILES and BROMIDES. When heated to decomposition it emits very toxic fumes of NO,, Br-, and CN-

InChI:InChI=1/C2HBr2N/c3-2(4)1-5/h2H

Upstream product

• 598-70-9 dibromoacetamide 
• 105-56-6 ethyl 2-cyanoacetate 
• 10222-01-2 2,2-dibromo-3-nitrilopropionamide 
• 10035-10-6 hydrogen bromide 
• 75-05-8 acetonitrile 
• 749251-98-7 azidoacetylene 
• 820-10-0 DL-methionine sulfone 
• 10097-32-2 bromide 
• 372-09-8 cyanoacetic acid 

Downstream Products

• 55106-50-8 (1-Bromo-cyclohexyl)-oxo-acetonitrile 
• 55106-46-2 Dibromo-(1-hydroxy-cyclohexyl)-acetonitrile 
• 53697-63-5 (+/-)-bromo-phenyl-acetic acid isopropyl ester 
• 6291-98-1 2-bromobutyric acid isopropyl ester 
• 10323-40-7 2-bromoisovaleric acid 
• 51368-55-9 isopropyl 2-bromo-2?methylpropanoate 
• 55106-47-3 2-bromo-2-methylpropanoyl cyanide 
• 29232-39-1 2,3-dibromo-5-methylpyridine 
• 598-70-9 dibromoacetamide 
• 30362-01-7 tris-dibromomethyl s-triazine 
• 4360-47-8 cinnamonitrile 
• 33863-75-1 1-Cyano-2-phenyloxirane 
• 37854-15-2 2-bromo-3-phenyl-2-propenenitrile 
• 14164-31-9 5-phenyl-2,4-pentadienenitrile 

Relevant articles and documents

Paired Electrosynthesis of Cyanoacetic Acid

Cyanoacetic acid is formed by cathodic reduction of CO2 and anodic oxidation of the tetraalkylammonium salt anion; the process is conduced in acetonitrile using a divided cell with a medium porosity glass-frit diaphragm. A mechanism for this paired electrochemical reaction is proposed.

Chemistry of the biosynthesis of halogenated methanes: C1-organohalogens as pre-industrial chemical stressors in the environment?

We have chemical evidence that in the biosynthesis of the halomethanes C1H(4-n),X(n) (n = 1-4) three different pathways of biogenic formation have to be distinguished. The formation of methyl chloride, methyl bromide, and methyl iodide, respectively, has to be considered as a methylation of the respective halide ions. The dihalo- and trihalomethanes are formed via the haloform and/or via the sulfo-haloform reaction. The possible formation of tetrahalomethanes may involve a radical mechanism. Methionine methyl sulfonium chloride used as substrate in the incubation together with chloroperoxidase (CPO) and H2O2 gave high yields of monohalomethanes only. We were able to show that next to the CPO/H2O2 driven haloform reaction of carbonyl activated methyl groups also methyl-sulphur compounds - e.g. dimethylsulfoxide, dimethylsulfone, and the sulphur amino acid methionine - can act as precursors for the biosynthesis of di- and trihalogenated methanes. Moreover, there is some but not yet very conclusive evidence for an enzymatic production of tetrahalogenated methanes. In our experiments with chloroperoxidase involving amino acids and complex natural peptide based substrates, dihalogenated acetonitriles and several other volatile halogenated but yet unidentified compounds were formed. On the basis of these experiments we like to suggest that biosynthesis of halogenated nitriles occurs in general and therefore a natural atmospheric background should exist for halogenated acetonitriles and halogenated acetaldehydes, respectively.