Copper(I) chloride

2008/9 Schools Wikipedia Selection. Related subjects: Chemical compounds

Copper(I) chloride
Copper(I) chloride
Unit cell of nantokite
IUPAC name Copper(I) chloride
Other names Cuprous chloride
CAS number [7758-89-6]
RTECS number GL6990000
Molecular formula CuCl
Molar mass 98.99 g/mol
Appearance white powder, slightly
green from oxidized impurities
Density 4.140 g/cm3, solid
Melting point

430 °C (703 K)

Boiling point

1490 °C (1760 K),

Solubility in water 0.0062 g/100 mL (20 °C)
Crystal structure Tetrahedral close packed
( Zinc blende structure)
Main hazards Irritant
NFPA 704
R/S statement R: 22, 50, 53 S: 22, 60/61
Related compounds
Other anions Copper(I) bromide
Copper(I) iodide
Other cations Copper(II) chloride
Silver(I) chloride
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references

Copper(I) chloride, commonly called cuprous chloride, is the lower chloride of copper, with the formula CuCl. This colorless solid is a versatile precursor to other copper compounds, including some of commercial significance. It occurs naturally as the rare mineral nantokite. Unlike other first-row transition metal halides, it forma a stable complexes with carbon monoxide. It crystallizes in a diamondoid motif, reflecting the tendency of copper(I) to form tetrahedral complexes.


Copper(I) chloride is produced industrially by the direct chlorination of copper:

2 Cu + Cl2 → 2 CuCl

In the laboratory, copper(I) chloride can be prepared by the reduction of copper(II) salts such as CuSO4 using sulfur dioxide, sodium bisulfite (NaHSO3), sodium metabisulfite, or copper metal.

2 CuCl2 + H2O + SO32- → 2 CuCl + SO42- + 2 Cl-

The white solid precipitates from the solution. Upon standing in moist air, samples of CuCl become green due to the formation of copper(II) chlorides.

Chemical properties

CuCl is more affordable and less toxic than other soft Lewis acids. In addition, copper can exist in multiple redox states, including I, II, and III. This combination of properties define some of the useful features of copper(I) chloride. It is a soft Lewis acid, classified as soft according to the Hard-Soft Acid-Base concept. Thus, it tends to form stable complexes with soft Lewis bases such as triphenylphosphine:

CuCl + P(C6H5)3 → [CuCl(P(C6H5)3)]4

Although CuCl is insoluble in water, it dissolves in aqueous solutions containing suitable donor molecules. It forms complexes with halide ions, for example forming H3O+ CuCl2- with concentrated hydrochloric acid. It also dissolves in solutions containing CN-, S2O32-, and NH3 to give complexes.

Solutions of CuCl in HCl or NH3 absorb carbon monoxide to form colourless complexes such as the chloride-bridged dimer [CuCl(CO)]2. The same hydrochloric acid solutions also react with acetylene gas to form [CuCl(C2H2)]. ammoniacal solutions of CuCl react with acetylenes to form the explosive copper(I) acetylide. Complexes of CuCl with alkenes can be prepared by reduction of CuCl2 by sulfur dioxide in the presence of the alkene in alcohol solution. Complexes with dienes such as 1,5-cyclooctadiene are particularly stable:

Structure of COD complex of CuCl

Although only poorly soluble in water, its aqueous solution are unstable with respect to disproportionation into Cu and CuCl2. In part for this reason samples assume a green coloration (see photograph in upper right).


The main use of copper(i) chloride is as a precursor to the fungicide copper oxychloride. For this purpose aqueous copper(I) chloride is generated by comproportionation and then air-oxidized:

Cu + CuCl2 → 2 CuCl
6 CuCl + 3/2 O2 + 3 H2O → 2 Cu3Cl2(OH)4 + CuCl2

Copper(I) chloride catalyzes a variety of organic reactions, as discussed above. Its affinity for carbon monoxide in the presence of aluminium chloride is exploited in the COPureSM process.

In organic synthesis

In the Sandmeyer reaction. Treatment of an arenediazonium salt with CuCl leads to an aryl chloride, for example:

(Example Sandmeyer reaction using CuCl) The reaction has wide scope and usually gives good yields.

Early investigators observed that copper(I) halides catalyse 1,4-addition of Grignard reagents to alpha,beta-unsaturated ketones led to the development of organocuprate reagents that are widely used today in organic synthesis:

(Addition of RMgX to C=C-C=O mediated by CuCl) This finding led to the development of organocopper chemistry. For example, CuCl reacts with methyllithium (CH3Li) to form " Gilman reagents" such as (CH3)2CuLi, which find extensive use in organic synthesis. Grignard reagents react similarly. Although other copper(I) compounds such as copper(I) iodide are now more often used for these types of reactions, copper(I) chloride is still recommended in some case:

(Alkylation of sorbate ester at 4-position mediated by CuCl) Here, Bu indicates an n- butyl group. Without CuCl, the Grignard reagent alone gives a mixture of 1,2- and 1,4-addition products (i.e., the butyl adds at the closer to the C=O).

In polymer chemistry

Copper(I) chloride is also an intermediate formed from copper(II) chloride in the Wacker process. CuCl is used as a catalyst in Atom Transfer Radical Polymerization (ATRP).

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