Dicopper chloride trihydroxide

Dicopper chloride trihydroxide is the chemical compound with the chemical formula Cu₂(OH)₃Cl. It is often referred to as tribasic copper chloride (TBCC), copper trihydroxyl chloride or copper hydroxychloride. It is a greenish crystalline solid encountered in mineral deposits, metal corrosion products, industrial products, art and archeological objects, and some living systems. It was originally manufactured on an industrial scale as a precipitated material used as either a chemical intermediate or a fungicide. Since 1994, a purified, crystallized product has been produced at the scale of thousands of tons per year, and used extensively as a nutritional supplement for animals.

Dicopper chloride trihydroxide

Names
IUPAC name Dicopper(II) chloride trihydroxide
Preferred IUPAC name Copper trihydroxyl chloride
Identifiers
CAS Number	1332-65-6^Y
3D model (JSmol)	Interactive image
ChemSpider	10142932
ECHA InfoCard	100.014.158
EC Number	215-572-9
PubChem CID	11969527
UNII	76712031PG
CompTox Dashboard (EPA)	DTXSID6034475
InChI InChI=1S/ClH.2Cu.3H2O/h1H;;;3*1H2/q;2*+2;;;/p-4 Key: SKQUUKNCBWILCD-UHFFFAOYSA-J
SMILES [OH-].[OH-].[OH-].[Cl-].[Cu+2].[Cu+2]
Properties
Chemical formula	Cu2(OH)3Cl
Molar mass	213.56 g·mol^−1
Appearance	Green crystalline solid
Density	3.5 g/cm^3
Melting point	250 °C; 482 °F; 523 K
Solubility in water	Insoluble in water (pH 6.9 measured by EPA method SW846-9045)
Solubility	Insoluble in organic solvents
Structure
Crystal structure	Atacamite: orthorhombic Paratacamite: rhombohedral Clinoatacamite: monoclinic Botallackite: monoclinic
Coordination geometry	Distorted octahedral
Hazards
NFPA 704 (fire diamond)	1 0 0
Flash point	Non-flammable
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1 mg/m^3 (as Cu)^[2]
REL (Recommended)	TWA 1 mg/m^3 (as Cu)^[2]
IDLH (Immediate danger)	TWA 100 mg/m^3 (as Cu)^[2]
Safety data sheet (SDS)	^[1]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is ^YN ?) Infobox references

Natural occurrence

Cu₂(OH)₃Cl occurs as natural minerals in four polymorphic crystal forms: atacamite, paratacamite, clinoatacamite, and botallackite. Atacamite is orthorhombic, paratacamite is rhombohedral, and the other two polymorphs are monoclinic. Atacamite and paratacamite are common secondary minerals in areas of copper mineralization and frequently form as corrosion products of Cu-bearing metals.^{[3][4][5][6][7][8][9]}

The most common Cu₂(OH)₃Cl polymorph is atacamite. It is an oxidation product of other copper minerals, especially under arid, saline conditions. It was found in fumarolic deposits, and a weathering product of sulfides in subsea black smoker deposits. It was named for the Atacama Desert in Chile. Its color varies from blackish to emerald green. It is the sugar-like coating of dark green glistening crystals found on many bronze objects from Egypt and Mesopotamia. It has also been found in living systems such as the jaws of the marine bloodworm Glycera dibranchiata. The stability of atacamite is evidenced by its ability to endure dynamic regimes in its natural geologic environment.^{[4][5][6][10]}

Paratacamite is another Cu₂(OH)₃Cl polymorph that was named for the Atacama Desert in Chile. It has been identified in the powdery light-green corrosion product that forms on a copper or bronze surface – at times in corrosion pustules. It can be distinguished from atacamite by the rhombohedral shape of its crystals.^[4][5][8]

Botallackite is the least stable of the four Cu₂(OH)₃Cl polymorphs. It is pale bluish-green in color. This rare mineral was first found, and later identified, in the Botallack Mine in Cornwall, England. It is also a rare corrosion product on archaeological finds. For instance, it was identified on an Egyptian statue of Bastet.^[4][5][7]

The fourth polymorph of Cu₂(OH)₃Cl family is clinoatacamite. It was found and identified around in Chuquicamata, Chile in 1996. It was named in allusion to its monoclinic morphology and relationship to atacamite. It too is pale green but has monoclinic crystals. Clinoatacamite can be easily confused with the closely related paratacamite. It is believed that clinoatacamite should replace most previously reported occurrences of paratacamite in the conservation literature.^[4][5][9]

Structure

Atacamite is orthorhombic, space group Pnma, with two crystallographically independent Cu and oxygen atoms of OH groups in the asymmetric unit. Both Cu atoms display characteristically Jahn-Teller distorted octahedral (4+2) coordination geometry: each Cu is bonded to four nearest OH groups with Cu-OH distance of 2.01 Å; in addition, one of Cu atoms is bonded to two Cl atoms (at 2.76 Å) to form a [Cu(OH)₄Cl₂] octahedron, and the other Cu atom is bonded to one Cl atom (at 2.75 Å) and a distant OH group (at 2.36 Å) to form a [Cu(OH)₅Cl] octahedron. The two different types of octahedron are edge-linked to form a three-dimensional framework with the [Cu(OH)₅Cl] octahedron cross-linking the [Cu(OH)₄Cl₂] octahedron layers parallel to (110) (Figure 1).^[4][5][6]

 

Figure 1. Cu coordination and bonding in atacamite

Botallackite crystallizes in monoclinic with space group P2₁/m. Like in atacamite, there are two different types of Cu coordination geometries: Jahn-Teller distorted octahedral [Cu(OH)₄Cl₂] and [Cu(OH)₅Cl]. But these octahedra assemble in different ways. Each octahedron shares six edges with surrounding octahedra, forming a two-dimensional sheet-type structure parallel to (100). The adjacent sheets are held together by hydrogen bonding between the hydroxyl oxygen atoms of one sheet and the opposing chlorine atoms in the other sheets. The resulting weak bonding between the sheets accounts for the perfect (100) cleavage and the typical platy habit of botallackite (Figure 2).^[4][5][7]

 

Figure 2. Cu coordination and bonding in botallackite

Paratacamite is rhombohedral, space group R3. It has a well-developed substructure with a’=a/2, c’=c, apparent space group R3m. There are four crystallographically independent Cu atoms in the asymmetric unit. The Cu atoms display three different types of octahedral coordination geometries. Three quarters of the Cu atoms are coordinated to four near OH groups and two distant Cl atoms, giving the expected (4+2) configuration [Cu(OH)₄Cl₂]. Three sixteenths of the Cu atoms are bonded to two near OH groups at 1.93 Å and four stretched OH groups at 2.20 Å to form an axially compressed (2+4) octahedral [Cu(OH)₆], and the remaining one sixteenth of the Cu atoms are bonded to six equivalent OH groups at 2.12 Å to form a regular octahedral [Cu(OH)₆]. The Jahn-Teller distorted [Cu(OH)₄Cl₂] octahedra share the edges and form partially occupied layers parallel to (001), and the compressed and regular [Cu(OH)₆] octahedra cross-link the adjacent [Cu(OH)₄Cl₂] octahedral layers to form a three-dimensional framework. The existence of the regular octahedral [Cu(OH)₆] is unusual, and it has been shown that partial substitution of Zn or Ni for Cu at this special site (3b) is necessary to stabilize paratacamite structure at ambient temperature. Due to the high symmetry of the special position, only about 2 wt% Zn is necessary to stabilize the rhombohedral structure. In fact, most of paratacamite crystals studied contain significant amounts of Zn or Ni (> 2 wt%) (Figure 3).^[4][5][8]

 

Figure 3. Cu coordination and bonding in paratacamite

Clinoatacamite is monoclinic, space group P2₁/m. The structure is very close to that of paratacamite. But the [Cu(OH)₆] octahedron is Jahn-Teller distorted. The Jahn-Teller distorted [Cu(OH)₄Cl₂] octahedra share the edges to form partially occupied layers parallel to (101). This layer is topologically the same as that in mica. Adjacent layers of octahedra are offset, such that vacant sites in one sheet align with occupied sites in the neighboring sheet. The [Cu(OH)₆] octahedra link the layers to form a 3-dimensional network (Figure 4).^[4][5][9]

 

Figure 4. Cu coordination and bonding in clinoatacamite

Thermodynamic data based on the free energy of formation indicates that the order of stability of these polymorphs is clinoatacamite>atacamite> botallackite. Spectroscopic studies show that the strength of hydrogen bonding in these polymorphs is in the order paratacamite >atacamite> botallackite. Studies on the formation of basic copper chloride indicate botallackite is a key intermediate and crystallizes first under most conditions; subsequent recrystallization of botallackite to atacamite or paratacamite depends on the nature of reaction medium.^[11][12][13]

Properties

Dicopper chloride trihydroxide Cu₂(OH)₃Cl is a green crystalline solid. It decomposes above 220 °C with elimination of hydrochloric acid to copper oxides. It is largely stable in neutral media, but decomposes by warming in alkaline media, yielding oxides. It is virtually insoluble in water and organic solvents, soluble in mineral acids yielding the corresponding copper salts (eq. 1), soluble in ammonia, amine and EDTA solutions under complex formation. It can easily be converted to copper(II) hydroxide by reacting with sodium hydroxide (eq. 2). Its pH in water is 6.9 measured by EPA method SW846-9045.^[14]

Cu₂(OH)₃Cl + 3 HCl → 2 CuCl₂ + 3 H₂O (eq.1)

Cu₂(OH)₃Cl + NaOH → 2 Cu(OH)₂ + NaCl (eq.2)

Most of the published scientific literature on the properties of the compound has focused on specimens found as natural minerals or corrosion products on copper alloys, or prepared under laboratory conditions.

Traditionally reported preparation routes

Hydrolysis of CuCl₂

Cu₂(OH)₃Cl can be prepared by hydrolysis of a CuCl₂ solution at pH 4 ~ 7. A variety of bases such as sodium carbonate, ammonia, calcium hydroxide, or sodium hydroxide may be used (eq. 3).^[3]

2 CuCl₂ + 3 NaOH → Cu₂(OH)₃Cl + 3 NaCl (eq.3)

Cu₂(OH)₃Cl can also be prepared by the reaction of a hot CuCl₂ solution with freshly precipitated CuO (eq. 4).

CuCl₂ + 3 CuO + 3 H₂O → 2 Cu₂(OH)₃Cl (eq.4)

If sufficient chloride ions are present in solution, hydrolysis of CuSO₄ with alkali also produces Cu₂(OH)₃Cl (eq. 5).

2 CuSO₄ + 3 NaOH + NaCl → Cu₂(OH)₃Cl + 2 Na₂SO₄ (eq.5)

Industrial production

Air oxidation of CuCl in brine solution

Prior to 1994, large scale industrial production of basic copper chloride was devoted to making either a fungicide for crop protection or an intermediate in the manufacture of other copper compounds.^[3] In neither of those applications was the polymorphic nature of the compound, or the size of individual particles of particular importance, so the manufacturing processes were simple precipitation schemes.

Cu₂(OH)₃Cl can be prepared by air oxidation of CuCl in brine solution. The CuCl solution is usually made by the reduction of CuCl₂ solutions over copper metal. A CuCl₂ solution with concentrated brine is contacted with copper metal until the Cu(II) is completely reduced. The resulting CuCl is then heated to 60 ~ 90 °C and aerated to effect the oxidation and hydrolysis. The oxidation reaction can be performed with or without the copper metal. The precipitated product is separated and the mother liquor containing CuCl₂ and NaCl, is recycled back to the process (eq. 6 ~ 7).

CuCl₂ + Cu + 2 NaCl → 2 NaCuCl₂ (eq.6)

12 NaCuCl₂ + 3 O₂ + 2 H₂O → 4 Cu₂(OH)₃Cl + 4 CuCl₂ + 12 NaCl (eq.7)

The product from this process is of fine particle with size of 1 ~ 5 µm and is usable as an agricultural fungicide.^[3]

Micronutrients process

In 1994, an unusually efficient, economic, reliable and green process was developed for commercial production of a purified and crystallized form of tribasic copper chloride.^[15][16] It results in a stable, free-flowing, non-dusty green powder with typical particle size of 30 ~ 100 microns. The combination of its density and particle size distribution results in blending and handling characteristics beneficial in preparation of uniform animal feed mixtures.

Initially, that new process was designed to utilize spent etchant streams from the electronic printed circuit board manufacturing industry as starting materials.

There are two types of spent etching solutions from printed circuit board manufacturing operations: an acidic cupric chloride solution (CuCl₂/HCl), and an alkaline tetraamminedichloridocopper(II) solution ([Cu(NH₃)₄Cl₂]). Tribasic copper chloride is generated by neutralization of either one of these two solutions (acidic or alkaline pathway), or by combination of these two solutions, a self-neutralization reaction.

In the acidic pathway, the cupric chloride solution can be neutralized with caustic soda, or ammonia, lime, or other base.

In the alkaline pathway, cuprammine chloride solution can be neutralized with HCl or other available acidic solutions (eq. 8).

2 [Cu(NH₃)₄Cl₂] + 5 HCl + 3 H₂O → Cu₂(OH)₃Cl + 8 [NH₄]Cl (eq. 8)

More efficiently, the two spent etching solutions are combined under mild acidic conditions, one neutralizing the other, to produce higher yield of basic copper chloride (eq. 9).

3 [Cu(NH₃)₄Cl₂] + 5 CuCl₂ + 12 H₂O → 4 Cu₂(OH)₃Cl + 12 [NH₄]Cl (eq. 9)

Seeding is introduced during crystallization. The production is operated continuously under well-defined conditions (pH, feeding rate, concentrations, temperature, etc.). Product with good particle size is produced and can be easily separated from background salt and other impurities in the mother liquor. After simple rinse with water and drying, pure, free-flowing, non-dusty green crystalline solid with typical particle size of 30 ~ 100 micron is obtained. The product from this process is predominantly atacamite and paratacamite, the stable crystal forms of basic copper chloride – and is called alpha basic copper chloride for simplicity. Careful control of process conditions to favor the alpha polymorphs results in a product that remains free flowing over extended storage times, thus avoiding caking as occurs with both copper sulfate and the botallackite crystal form - also called beta basic copper chloride. This process has been used to manufacture thousands of tons of tribasic copper chloride every year, and has been the predominant route of commercial production since it was introduced by Micronutrients in 1994.^[16]

Applications

As an agriculture fungicide

Fine Cu₂(OH)₃Cl has been used as a fungicidal spray on tea, orange, grape, rubber, coffee, cardamom, and cotton etc., and as an aerial spray on rubber for control of phytophthora attack on leaves.^[3][17]

As a pigment

Basic copper chloride has been used as a pigment and as a colorant for glass and ceramics. It was widely used as a coloring agent in wall painting, manuscript illumination, and other paintings by ancient people. It was also used in cosmetics by ancient Egyptians.^[18][19]

In pyrotechnics

Cu₂(OH)₃Cl has been used as a blue/green coloring agents in pyrotechnics.^[3]

As a catalyst

Cu₂(OH)₃Cl has been used in the preparation of catalysts and as a catalyst in organic synthesis for chlorination and/or oxidation.

Cu₂(OH)₃Cl has been shown to be a catalyst in the chlorination of ethylene.^[20]

Atacamite and paratacamite crystal forms of Cu₂(OH)₃Cl have been found to be active species in supported CuCl₂ catalyst systems for the oxidative carbonylation of methanol to dimethyl carbonate. A number of supported Cu₂(OH)₃Cl catalysts have also been prepared and studied in such conversion. Dimethyl carbonate is an environmentally benign chemical product and unique intermediate with versatile chemical reactivity.^[21][22]

Cu₂(OH)₃Cl has been identified as a new catalytically active material for the partial oxidation of n-butane to maleic anhydride.^[23]

A mixture of ultrafine powder CuO/Cu₂(OH)₃Cl has been shown to be good in photo-catalytic decolorization of dyes, such as amido black, and indigo carmine.^[24]

As a commercial feed supplement

Copper is one of the most critically important of the trace minerals that are essential elements in numerous enzymes that support metabolic functions in most organisms. Since the early 1900s, copper has routinely been added to animal feedstuffs to support good health and normal development. Starting in the 1950s, there was increasing focus on the issue of bioavailability of trace mineral supplements which led to copper sulfate pentahydrate becoming the predominant source. Because of its high water solubility, and thus hygroscopicity, CuSO₄ leads to destructive reactions in feed mixtures. These are notoriously destructive in hot, humid climates. Recognition that basic copper chloride would reduce feed stability problems led to issuance of patents on the use of the compound as a nutritional source.^[15]

Subsequently, animal feeding studies revealed that the alpha crystal form of basic copper chloride has a rate of chemical reactivity that is well matched to biological processes. The strength of the bonds holding copper in the alpha crystal polymorphs could prevent undesirable, anti-nutritive interactions with other feed ingredients while delivering controlled amounts of copper throughout the active zones in the digestive tract of an animal.

Success in producing alpha basic copper chloride on a large scale allowed for the widespread application of basic copper chloride in the feed thereby supplying the copper requirements of all major livestock groups. This form of the compound has proven to be particularly suitable as a commercial feed supplement for use in livestock and aquaculture due to its inherent chemical and physical characteristics. Compared to copper sulfate, the alpha crystal form of basic copper chloride provides many benefits including improved feed stability, less oxidative destruction of vitamins and other essential feed ingredients; superior blending in feed mixtures, and reduced handing costs. It has been widely used in feed formulations for most species, including chickens, turkeys, pigs, beef and dairy cattle, horses, pets, aquaculture and exotic zoo animals.^{[25][26][27][28][29][30][31][32][33][34][35][36]}

References

1. http://www.pyrodata.com/sites/default/files/Copper%20oxychloride.pdf ^{[bare URL PDF]}
2. NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
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5. (a) http://webmineral.com/data/Atacamite.shtml; (b) http://webmineral.com/data/Botallackite.shtml; (c) http://webmineral.com/data/Paratacamite.shtml; (d) http://webmineral.com/data/clinoatacamite.shtml.
6. (a) Wells, A. F. The crystal structure of atacamite and the crystal chemistry of cupric compounds. Acta Crystallogr. 1949, 2, 175-80. (b) Paris, J. B; Hyde, B. G. The structure of atacamite and its relationship to spinel. Crystal. Struc. Comm. 1986, C42(10), 1277-80.
7. Hawthorne, F. C. Refinement of the crystal structure of botallackite. Mineral Mag. 1985, 49, 87- 89.
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29. Engle, T. E.; Spears, J. W.; Armstrong, T. A.; Wright, C. L.; Odle, J. "Effects of Dietary Copper Source and Concentration on Carcass Characteristics and Lipid and Cholesterol Metabolism in Growing and Finishing Steers". J. Anim. Sci. 2000, 78, 1053-1059.
30. Hooge, D. M.; Steward, F. A.; McNaughton, J. L. "Efficacy of Dietary Tribasic Copper Chloride (TBCC) versus Copper Sulfate Pentahydrate for Improving Productive Performance of Broiler Chickens". Paper presented at the International Poultry Scientific Forum, Atlanta, GA, U.S.A., January 17, 2000.
31. Hooge, D. M.; Steward, F. A.; McNaughton, J. L. "Bioavailability of Copper from Tribasic Copper Chloride (TBCC) Compared to Copper Sulfate Pentahydrate in Broiler Chicken Diets". Paper presented at the International Poultry Scientific Forum, Atlanta, GA, U.S.A., January 17, 2000.
32. Hooge, D. M.; Steward, F. A.; McNaughton, J. L. "Improved Stabilities of Vitamins A, D3, E and Riboflavin with Tribasic Copper Chloride (TBCC) Compared to Copper Sulfate Pentahydrate in Crumbled Broiler Starter Feed". Paper presented at the 89th Annual Meeting of the Poultry Science Association, Palais de Congress, Montreal, Quebec, Canada, August 19, 2000.
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34. Klasing, K. C.; Naziripour, A. Effect of dietary copper source and level on GI copper levels and ileal E. coli survival in broiler chicks. ADSA.PSA.AMPA.CSAS.WSASAS.ASAS Joint Annual Meeting, Jul 11-15, 2010, Denver, CO.
35. Fry, R. S.; Ashwell, M. S.; Flowers, W. L; Stewart, K. R.; Spears, J. W. Effect of level and source of dietary copper on copper metabolism in the small intestine of weanling pigs. ADSA.PSA.AMPA.CSAS.WSASAS.ASAS Joint Annual Meeting, Jul 11-15, 2010, Denver, CO.
36. Klasing, K. C.; Naziripour, A. Bioavailability of copper sources to broiler chicks when fed below the copper requirement. ADSA.PSA.AMPA.CSAS.WSASAS.ASAS Joint Annual Meeting, Jul 11-15, 2010, Denver, CO.