Cupric bromide Property

Melting point:

498 °C(lit.)

Boiling point:

900 °C

Density 

4.77 g/mL at 25 °C(lit.)

Flash point:

900°C

storage temp. 

Store below +30°C.

solubility 

1200g/l

form 

Crystalline Powder

Specific Gravity

4.77

color 

Gray-blue

Water Solubility 

soluble

Sensitive 

Hygroscopic

Merck 

14,2629

Exposure limits

ACGIH: TWA 1 mg/m3
NIOSH: IDLH 100 mg/m3; TWA 1 mg/m3

Stability:

Stable. Incompatible with alkali metals, moisture. Reacts violently with potassium.

CAS DataBase Reference

7789-45-9(CAS DataBase Reference)

NIST Chemistry Reference

copper(II) dibromide(7789-45-9)

EPA Substance Registry System

Copper bromide (CuBr2) (7789-45-9)

Safety

Hazard Codes 

C,Xi

Risk Statements 

22-34-36/37/38

Safety Statements 

26-36/37/39-45-24/25

RIDADR 

UN 3260 8/PG 3

WGK Germany 

3

TSCA 

Yes

HS Code 

2827 59 00

HazardClass 

8

PackingGroup 

III

Hazardous Substances Data

7789-45-9(Hazardous Substances Data)

Toxicity

LD50 orally in Rabbit: 536 mg/kg

Hazard and Precautionary Statements (GHS)

Symbol(GHS)

Signal word

Danger

Hazard statements

H302Harmful if swallowed

H314Causes severe skin burns and eye damage

H410Very toxic to aquatic life with long lasting effects

Precautionary statements

P260Do not breathe dust/fume/gas/mist/vapours/spray.

P273Avoid release to the environment.

P280Wear protective gloves/protective clothing/eye protection/face protection.

P301+P312IF SWALLOWED: call a POISON CENTER or doctor/physician IF you feel unwell.

P303+P361+P353IF ON SKIN (or hair): Remove/Take off Immediately all contaminated clothing. Rinse SKIN with water/shower.

P305+P351+P338IF IN EYES: Rinse cautiously with water for several minutes. Remove contact lenses, if present and easy to do. Continuerinsing.

Cupric bromide Chemical Properties,Usage,Production

Description

Cupric bromide is a kind of inorganic compound obtained through the reaction between copper oxide and hydrobromic acid. It can be used in laser, generating pulse yellow and green light. The cupric bromide laser is an important technology used in dermatology for the treatment of pigmented lesion and vascular lesions. It can also be used in living radical polymerization and as an intensifier in photographic processing. It is also a brominating agent used in organic synthesis. In addition, it is a kind of highly efficient catalyst in the direct alkynylation of azoles.

Chemical Properties

Copper(II) bromide, CuBr2, [7789-45-9], MW 223.36, MP 498°C, d 4.77, is a black, deliquescent, monoclinic, crystalline material that obtains from warm aqueous solution. At temperatures below 29°C, the green tetrahydrate is produced. Copper(II) bromide is very soluble in water and soluble in alcohol and acetone.

Uses

Copper(II) bromide is used as a catalyst in organic reactions, as an intensifier in photography, and as a brominating agent.

Preparation

Copper(II) bromide is most easily prepared by neutralization of copper(II) oxide, carbonate, or hydroxide with hydrobromic acid. It can also be produced by oxidation of copper metal with bromine water or by reaction of bromine solutions in alcohol with copper powder.

References

Shen, Youqing, Shiping Zhu, and Robert Pelton. Macromolecules 34.10 (2001): 3182-3185.
Rothfleisch, Jeremy E., et al. Dermatologic clinics 20.1 (2002): 1- 18.
Huang, Jianhui, Simon JF Macdonald, and Joseph PA Harrity. Chemical Communications 4 (2009): 436-438.
Besselièvre, François, and Sandrine Piguel. Angewandte Chemie International Edition 48.50 (2009): 9553-9556.

Chemical Properties

Black crystal

Uses

Copper(II) bromide is used in photographic processing as an intensifier and as a brominating agent in organic synthesis. It is also used in the coupling of o-iodophenols and aryl acetylenes avoiding the use of palladium. It finds application in the preparation of NK1/NK2 receptor antagonists used in the regulation of tachykinin.

Uses

Some reported applications of copper bromide are:

• catalyst in cross coupling reactions.
• co-catalyst in Sonogashira coupling.
• Lewis acid in enantioselective addition of alkynes.
• reducing agent, when complexed by three molecules of pyridine initiators for the controlled polymerization of styrene, methyl acrylate and methyl methacrylate.

Reductive homocoupling of α-bromo- α- chlorocarboxylates to dimethyl α, α′ dichlorosuccinate derivatives in presence of CuBr/LiOCH₃ in methanol has been reported.

Uses

As intensifier in photography; as brominating agent in organic synthesis; as humidity indicator; as wood preservative; in solid-electrolyte battery; as stabilizer for acetylated polyformaldehyde.

General Description

Odorless black solid. Sinks and mixes with water.

Air & Water Reactions

Deliquescent. Water soluble.

Reactivity Profile

Acidic inorganic salts, such as Cupric bromide, are generally soluble in water. The resulting solutions contain moderate concentrations of hydrogen ions and have pH's of less than 7.0. They react as acids to neutralize bases. These neutralizations generate heat, but less or far less than is generated by neutralization of inorganic acids, inorganic oxoacids, and carboxylic acid. They usually do not react as either oxidizing agents or reducing agents but such behavior is not impossible. Many of these compounds catalyze organic reactions.

Health Hazard

Inhalation of dust causes irritation of throat and lungs. Ingestion of large amounts causes violent vomiting and purging, intense pain, collapse, coma, convulsions, and paralysis. Contact with solutions causes eye irritation; contact with solid causes severe eye surface injury and skin irritation.

Fire Hazard

Special Hazards of Combustion Products: Irritating hydrogen bromide gas may form in fire.

Flammability and Explosibility

Not classified

Purification Methods

Crystallise it twice by dissolving it in water (140mL/g), filtering to remove any Cu2Br2, and concentrating under vacuum at 30o until crystals appear. The cupric bromide is then allowed to crystallise by leaving the solution in a vacuum desiccator containing P2O5 [Hope et al. J Chem Soc 5226 1960, Glemser & Sauer in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol II p 1009 1965].