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Copper(II) bromide

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Title: Copper(II) bromide  
Author: World Heritage Encyclopedia
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Subject: Copper(II) fluoride, Inorganic compounds by element, Copper, Caesium hexafluorocuprate(IV), Potassium hexafluorocuprate(III)
Collection: Bromides, Copper Compounds, Metal Halides
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Copper(II) bromide

Copper (II) bromide
Copper (II) bromide
Other names
Cupric bromide
ChemSpider  Y
Jmol-3D images Image
Molar mass 223.37 g/mol
Appearance grayish black crystals
Density 4.710 g/cm3, solid
Melting point 498 °C (928 °F; 771 K)
Boiling point 900 °C (1,650 °F; 1,170 K)
55.7 g/100 mL (20 °C)
Solubility in soluble
Solubility in insoluble
NFPA 704
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 1 mg/m3 (as Cu)[1]
REL (Recommended)
TWA 1 mg/m3 (as Cu)[1]
TWA 100 mg/m3 (as Cu)[1]
Related compounds
Other anions
Copper(II) fluoride
Copper(II) chloride
Other cations
Nickel(II) bromide
Copper(I) bromide
Zinc bromide
Cadmium bromide
Mercury(II) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 Y  (: Y/N?)

Copper(II) bromide (

  1. ^ a b c "NIOSH Pocket Guide to Chemical Hazards #0150".  
  2. ^ Huang, Jianhui; Macdonald, Simon J. F.; Harrity, Joseph P. A. (2009). "A cycloaddition route to novel triazole boronic esters".  
  3. ^ Livingstone, E. S.; Maitland, A. "A high power, segmented metal, copper bromide laser". Measurement Science and Technology 2 (11): 1119.  
  4. ^ Breitinger, D. K.; Herrmann, W. A., eds. (1999). Synthetic methods of Organometallic and Inorganic Chemistry. New York: Thieme Medical Publishers.  
  5. ^ 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.
  6. ^ Helmholz, Lindsay (1947). "The Crystal Structure of Anhydrous Cupric Bromide".  
  7. ^ Conry, Rebecca R. (2006). "Copper: Inorganic & Coordination Chemistry". Encyclopedia of Inorganic Chemistry (2nd ed.). John Wiley & Sons.  
  8. ^ King, L. Carroll; Ostrum, G. Kenneth (1964). "Selective Bromination with Copper(II) Bromide".  
  9. ^ Rodebaugh, Robert; Debenham, John S.; Fraser-Reid, Burt J.; Snyder, James P. (1999). "Bromination of Alkenyl Glycosides with Copper(II) Bromide and Lithium Bromide: Synthesis, Mechanism, and DFT Calculations".  
  10. ^ McCoy, S.; Hanna, M.; Anderson, P.; McLennan, G.; Repacholi, M. (June 1996). "An evaluation of the copper-bromide laser for treating telangiectasia". Dermatol Surg. 22 (6): 551–7.  
  11. ^ Davis P., Town G., Haywards H. A practical comparison of IPLs and the Copper Bromide Laser for photorejuvenation, acne and the treatment of vascular&pigmented lesions.
  12. ^ Diane Heppner The Focal Encyclopedia of Photography, Inc. Elsevier 20074th edition
  13. ^ George McKedy US Patent Application Publication, Pub.No.: US2010/0252779 A1


See also

Copper(II) bromide is harmful if swallowed. It affects the central nervous system, brain, eyes, liver, and kidneys. It causes irritation to skin, eyes, and respiratory tract.


Copper(II) bromide lasers produce pulsed yellow and green light and have been studied as a possible treatment for cutaneous lesions.[10] Experiments have also shown copper bromide treatment to be beneficial for skin rejuvenation.[11] It has been widely used in photography as its solution was used as the bleaching step for intensifying collodion and gelatin negatives.[12] Copper(II)bromide has also been proposed as a possible material in humidity indicator cards.[13]


Dibromination of NPGs, n-pentenyl glycosides, using CuBr2/LiBr reagent combination was performed in order for an NPG to serve as a glycosyl acceptor during halonium-promoted couplings. Such reaction gives high yield of the dibromides from alkenyl sugars that are resistant to a direct reaction with molecular bromine.[9]

Copper (II) bromide in chloroform-ethyl acetate reacts with ketones resulting in the formation of alpha-bromo ketones. The resulting product can be directly used for the preparation of derivatives. This heterogeneous method is reported to be the most selective and direct method of formation of α-bromo ketones.[8]


In the solid state CuBr2 has a polymeric structure, with CuBr4 planar units connected on opposite sides to form chains. The crystal structure is monoclinic, space group C2/m, with lattice constants a = 714 pm, b = 346 pm, c = 718 pm, e ß = 121° 15'.[6] CuBr2 monomeric units are present in the gas phase at high temperature.[7]

Molecular and crystal structure

Copper(II) bromide is purified by crystallisation twice from water, filtration to remove any CuBr and concentration under vacuum. This product is dehydrated using phosphorus pentoxide.[5]


CuO + 2HBr → CuBr2 + H2O.

Copper(II) bromide can be obtained by combining copper oxide and hydrobromic acid:[4]



  • Synthesis 1
  • Purification 2
  • Molecular and crystal structure 3
  • Reactions 4
  • Usage 5
  • Safety 6
  • See also 7
  • References 8

It is also used in the copper vapor laser, a class of laser where the medium is copper bromide vapour formed in situ from hydrogen bromide reacting with the copper discharge tube.[3] Producing yellow or green light, it is used in dermatological applications.


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