Copper(I) bromide

The following article will address the topic of Copper(I) bromide, which has currently generated great interest and debate. For a long time, Copper(I) bromide has been the subject of study and analysis by experts in the area, and its impact has reached various spheres of society. On this occasion, we will seek to thoroughly analyze the most relevant aspects of Copper(I) bromide, as well as address different perspectives that allow us to understand its importance and impact. Through a detailed and rigorous analysis, it is intended to offer a comprehensive view of Copper(I) bromide, in order to provide the reader with a broad and complete understanding of this topic.

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Copper(I) bromide
Sample of copper(I) bromide
Sample of copper(I) bromide
Structure of CuBr
Structure of CuBr
Names
Other names
Cuprous bromide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.210 Edit this at Wikidata
UNII
  • InChI=1S/BrH.Cu/h1H;/q;+1/p-1 checkY
    Key: NKNDPYCGAZPOFS-UHFFFAOYSA-M checkY
  • InChI=1/BrH.Cu/h1H;/q;+1/p-1
    Key: NKNDPYCGAZPOFS-REWHXWOFAY
  • Br
Properties
CuBr
Molar mass 143.45 g/mol
Appearance white powder (see text)
Density 4.71 g/cm3, solid
Melting point 492 °C (918 °F; 765 K)
Boiling point 1,345 °C (2,453 °F; 1,618 K)
insoluble;
slightly soluble in cold water
6.27×10−9[1]
Solubility soluble in HCl, HBr, ammonium hydroxide, acetonitrile
negligible in acetone, sulfuric acid
−49.0×10−6 cm3/mol
2.116
1.46 D
Hazards
Flash point Non-flammable
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 1 mg/m3 (as Cu)[2]
REL (Recommended)
 TWA 1 mg/m3 (as Cu)[2]
IDLH (Immediate danger)
 TWA 100 mg/m3 (as Cu)[2]
Related compounds
Other anions
 Copper(I) chloride
Copper(I) iodide
Other cations
 Silver(I) bromide
Copper(II) bromide
Mercury(I) bromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
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Copper(I) bromide is the chemical compound with the formula CuBr. This white diamagnetic solid adopts a polymeric structure akin to that for zinc sulfide. The compound is widely used in the synthesis of organic compounds and as a lasing medium in copper bromide lasers.

Preparation, basic properties, structure

The compound is white, although samples are often colored due to the presence of copper(II) impurities.[3] The copper(I) ion also oxidizes easily in air. It is commonly prepared by the reduction of cupric salts with sulfite in the presence of bromide.[4] For example, the reduction of copper(II) bromide with sulfite yields copper(I) bromide and hydrogen bromide:

2 CuBr2 + H2O + SO2−
3 → 2 CuBr + SO2−
4 + 2 HBr

CuBr is insoluble in most solvents due to its polymeric structure, which features four-coordinated, tetrahedral Cu centers interconnected by bromide ligands (ZnS structure). Upon treatment with Lewis bases, CuBr converts to molecular adducts. For example, with dimethyl sulfide, the colorless complex is formed:[5]

CuBr + S(CH3)2 → CuBr(S(CH3)2)

In this coordination complex, the copper is two-coordinate, with a linear geometry. Other soft ligands afford related complexes. For example, triphenylphosphine gives CuBr(P(C6H5)3), although this species has a more complex structure. Thermal excitation of copper(I) bromide vapour yields a blue-violet emission which is of greater saturation than known copper(I) chloride emission.[6] Copper(I) bromide is hence an advantageous emitter in pyrotechnic flames.

Applications in organic chemistry

In the Sandmeyer reaction, CuBr is employed to convert diazonium salts into the corresponding aryl bromides:[4]

ArN+
2 + CuBr → ArBr + N2 + Cu+

The aforementioned complex CuBr(S(CH3)2) is widely used to generate organocopper reagents.[5] Related CuBr complexes are catalysts for atom transfer radical polymerization and copper-catalyzed cross-dehydrogenative couplings (CDC).

See also

Copper(II) bromide

References

  1. ^ Rumble, John (June 18, 2018). CRC Handbook of Chemistry and Physics (99th ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
  2. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  4. ^ a b This report gives a procedure for generating CuBr: Hartwell, Jonathan L. (1955). "o-Chlorobromobenzene". Organic Syntheses; Collected Volumes, vol. 3, p. 185.
  5. ^ a b Jarowicki, K.; Kocienski, P. J.; Qun, L. "1,2-Metallate Rearrangement: (Z)-4-(2-Propenyl)-3-Octen-1-ol". Organic Syntheses. 79: 11; Collected Volumes, vol. 10, p. 662.
  6. ^ Koch, E.-C. (2015). "Spectral Investigation and Color Properties of Copper(I) Halides CuX (X=F, Cl, Br, I) in Pyrotechnic Combustion Flames". Propellants Explos. Pyrotech. 40 (6): 798–802. doi:10.1002/prep.201500231.
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