Dicopper chloride trihydroxide

Last updated
Dicopper chloride trihydroxide
Alpha Crystal-TBCC.PNG
Names
IUPAC name
Dicopper(II) chloride trihydroxide
Preferred IUPAC name
Copper trihydroxyl chloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.014.158 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 215-572-9
PubChem CID
UNII
  • InChI=1S/ClH.2Cu.3H2O/h1H;;;3*1H2/q;2*+2;;;/p-4
    Key: SKQUUKNCBWILCD-UHFFFAOYSA-J
  • [OH-].[OH-].[OH-].[Cl-].[Cu+2].[Cu+2]
Properties
Cu2(OH)3Cl
Molar mass 213.56 g·mol−1
AppearanceGreen crystalline solid
Density 3.5 g/cm3
Melting point 250 °C; 482 °F; 523 K
Insoluble in water (pH 6.9 measured by EPA method SW846-9045) [1]
Solubility Insoluble in organic solvents
Structure
Distorted octahedral
Hazards
NFPA 704 (fire diamond)
NFPA 704.svgHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
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]
Safety data sheet (SDS) [3]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yes check.svgY  verify  (what is  Yes check.svgYX mark.svgN ?)

Dicopper chloride trihydroxide is the chemical compound with the chemical formula Cu 2(O H)3 Cl . 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.[ citation needed ]

Contents

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, soluble in ammonia, amine and EDTA solutions under complex formation:

Cu2(OH)3Cl + 3 HCl → 2 CuCl2 + 3 H2O

It can easily be converted to copper(II) hydroxide by reacting with sodium hydroxide:

Cu2(OH)3Cl + NaOH → 2 Cu(OH)2 + NaCl

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: [4]

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

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

CuCl2 + 3 CuO + 3 H2O → 2 Cu2(OH)3Cl[ citation needed ]

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

2 CuSO4 + 3 NaOH + NaCl → Cu2(OH)3Cl + 2 Na2SO4 [ citation needed ]

Industrial production

Air oxidation of Copper(I) chloride 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. [4] 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 (140–194 °F) 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:

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

The product from this process is of fine particle with size of 1 ~ 5  μm and is usable as an agricultural fungicide. [4]

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 [5] 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, the 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:

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

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:

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

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 is 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 Steward in 1994. [5]

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. [4] [6]

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. [7] [8] [ page needed ]

In pyrotechnics

Cu2(OH)3Cl has been used as a blue/green coloring agents in pyrotechnics. [4]

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. [9]

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. [10] [11]

Cu2(OH)3Cl has been identified as a new catalytically active material for the partial oxidation of n-butane to maleic anhydride. [12]

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. [13]

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.

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. [14] [15] [16]

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. [4]

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. [17]

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. [18]

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. [19]

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. [20]

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[ by whom? ] with the closely related paratacamite. It is believed[ by whom? ] that clinoatacamite should replace most previously reported occurrences of paratacamite in the conservation literature.

Structure of Naturally Occuring Forms

Atacamite is orthorhombic, space group Pnma, with two crystallographically independent Copper and Oxygen atoms of hydroxyl 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).

Figure 1. Cu coordination and bonding in atacamite AtacamiteB.png
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).

Figure 2. Cu coordination and bonding in botallackite BotallackiteB.png
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 Copper 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).

Figure 3. Cu coordination and bonding in paratacamite Paratacamite.png
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).

Figure 4. Cu coordination and bonding in clinoatacamite Clinoatacamite.png
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. [21] [22] [23]


Related Research Articles

<span class="mw-page-title-main">Hydroxide</span> Chemical compound

Hydroxide is a diatomic anion with chemical formula OH−. It consists of an oxygen and hydrogen atom held together by a single covalent bond, and carries a negative electric charge. It is an important but usually minor constituent of water. It functions as a base, a ligand, a nucleophile, and a catalyst. The hydroxide ion forms salts, some of which dissociate in aqueous solution, liberating solvated hydroxide ions. Sodium hydroxide is a multi-million-ton per annum commodity chemical. The corresponding electrically neutral compound HO• is the hydroxyl radical. The corresponding covalently bound group –OH of atoms is the hydroxy group. Both the hydroxide ion and hydroxy group are nucleophiles and can act as catalysts in organic chemistry.

<span class="mw-page-title-main">Copper(I) oxide</span> Chemical compound – an oxide of copper with formula Cu2O

Copper(I) oxide or cuprous oxide is the inorganic compound with the formula Cu2O. It is one of the principal oxides of copper, the other being copper(II) oxide or cupric oxide (CuO). Cuprous oxide is a red-coloured solid and is a component of some antifouling paints. The compound can appear either yellow or red, depending on the size of the particles. Copper(I) oxide is found as the reddish mineral cuprite.

<span class="mw-page-title-main">Copper(II) nitrate</span> Chemical compound

Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO3)2(H2O)x. The hydrates are blue solids. Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C. Common hydrates are the hemipentahydrate and trihydrate.

<span class="mw-page-title-main">Lead(II) chloride</span> Chemical compound

Lead(II) chloride (PbCl2) is an inorganic compound which is a white solid under ambient conditions. It is poorly soluble in water. Lead(II) chloride is one of the most important lead-based reagents. It also occurs naturally in the form of the mineral cotunnite.

<span class="mw-page-title-main">Copper(II) oxide</span> Chemical compound – an oxide of copper with formula CuO

Copper(II) oxide or cupric oxide is an inorganic compound with the formula CuO. A black solid, it is one of the two stable oxides of copper, the other being Cu2O or copper(I) oxide (cuprous oxide). As a mineral, it is known as tenorite. It is a product of copper mining and the precursor to many other copper-containing products and chemical compounds.

<span class="mw-page-title-main">Manganese(II) chloride</span> Chemical compound

Manganese(II) chloride is the dichloride salt of manganese, MnCl2. This inorganic chemical exists in the anhydrous form, as well as the dihydrate (MnCl2·2H2O) and tetrahydrate (MnCl2·4H2O), with the tetrahydrate being the most common form. Like many Mn(II) species, these salts are pink, with the paleness of the color being characteristic of transition metal complexes with high spin d5 configurations.

<span class="mw-page-title-main">Copper(I) chloride</span> Chemical compound

Copper(I) chloride, commonly called cuprous chloride, is the lower chloride of copper, with the formula CuCl. The substance is a white solid sparingly soluble in water, but very soluble in concentrated hydrochloric acid. Impure samples appear green due to the presence of copper(II) chloride (CuCl2).

<span class="mw-page-title-main">Copper(II) chloride</span> Chemical compound

Copper(II) chloride, also known as cupric chloride, is an inorganic compound with the chemical formula CuCl2. The monoclinic yellowish-brown anhydrous form slowly absorbs moisture to form the orthorhombic blue-green dihydrate CuCl2·2H2O, with two water molecules of hydration. It is industrially produced for use as a co-catalyst in the Wacker process.

<span class="mw-page-title-main">Octahedral molecular geometry</span> Molecular geometry

In chemistry, octahedral molecular geometry, also called square bipyramidal, describes the shape of compounds with six atoms or groups of atoms or ligands symmetrically arranged around a central atom, defining the vertices of an octahedron. The octahedron has eight faces, hence the prefix octa. The octahedron is one of the Platonic solids, although octahedral molecules typically have an atom in their centre and no bonds between the ligand atoms. A perfect octahedron belongs to the point group Oh. Examples of octahedral compounds are sulfur hexafluoride SF6 and molybdenum hexacarbonyl Mo(CO)6. The term "octahedral" is used somewhat loosely by chemists, focusing on the geometry of the bonds to the central atom and not considering differences among the ligands themselves. For example, [Co(NH3)6]3+, which is not octahedral in the mathematical sense due to the orientation of the N−H bonds, is referred to as octahedral.

<span class="mw-page-title-main">Metal ammine complex</span> Class of chemical compounds

In coordination chemistry, metal ammine complexes are metal complexes containing at least one ammonia ligand. "Ammine" is spelled this way for historical reasons; in contrast, alkyl or aryl bearing ligands are spelt with a single "m". Almost all metal ions bind ammonia as a ligand, but the most prevalent examples of ammine complexes are for Cr(III), Co(III), Ni(II), Cu(II) as well as several platinum group metals.

Technetium compounds are chemical compounds containing the chemical element technetium. Technetium can form multiple oxidation states, but often forms in the +4 and +7 oxidation states. Because technetium is radioactive, technetium compounds are extremely rare on Earth.

<span class="mw-page-title-main">Botallackite</span> Halide mineral

Botallackite, chemical formula Cu2(OH)3Cl is a secondary copper mineral, named for its type locality at the Botallack Mine, St Just in Penwith, Cornwall. It is polymorphous with atacamite, paratacamite and clinoatacamite.

<span class="mw-page-title-main">Halide mineral</span> Minerals with a dominant fluoride, chloride, bromide, or iodide anion

Halide minerals are those minerals with a dominant halide anion. Complex halide minerals may also have polyatomic anions.

<span class="mw-page-title-main">Boleite</span>

Boleite is a complex halide mineral with formula: KPb26Ag9Cu24(OH)48Cl62. It was first described in 1891 as an oxychloride mineral. It is an isometric mineral which forms in deep-blue cubes. There are numerous minerals related to boleite, such as pseudoboleite, cumengite, and diaboleite, and these all have the same complex crystal structure. They all contain bright-blue cubic forms and are formed in altered zones of lead and copper deposits, produced during the reaction of chloride bearing solutions with primary sulfide minerals.

<span class="mw-page-title-main">Calumetite</span>

Calumetite is a natural rarely occurring mineral. It was discovered in 1963 at the Centennial Mine near Calumet, Michigan, United States. Calumetite was first discovered along with anthonyite. It has a chemical formula of Cu(OH,Cl)
2•2(H
2O).

<span class="mw-page-title-main">Zinc chloride hydroxide monohydrate</span> Chemical compound

Zinc chloride hydroxide monohydrate or more accurately pentazinc dichloride octahydroxide monohydrate is a zinc hydroxy compound with chemical formula Zn5(OH)8Cl2·H2O. It is often referred to as tetrabasic zinc chloride (TBZC), basic zinc chloride, zinc hydroxychloride, or zinc oxychloride. It is a colorless crystalline solid insoluble in water. Its naturally occurring form, simonkolleite, has been shown to be a desirable nutritional supplement for animals.

<span class="mw-page-title-main">Cornubite</span> Copper arsenate mineral

Cornubite is a rare secondary copper arsenate mineral with formula: Cu5(AsO4)2(OH)4. It was first described for its discovery in 1958 in Wheal Carpenter, Gwinear, Cornwall, England, UK. The name is from Cornubia, the medieval Latin name for Cornwall. It is a dimorph of cornwallite, and the arsenic analogue of pseudomalachite.

Magnesium hydroxychloride is the traditional term for several chemical compounds of magnesium, chlorine, oxygen, and hydrogen whose general formula xMgO·yMgCl2·zH2O, for various values of x, y, and z; or, equivalently, Mgx+y(OH)2xCl2y(H2O)z−x. The simple chemical formula that is often used is Mg(OH)Cl, which appears in high school subject, for example.Other names for this class are magnesium chloride hydroxide, magnesium oxychloride, and basic magnesium chloride. Some of these compounds are major components of Sorel cement.

<span class="mw-page-title-main">Ammineite</span>

Ammineite is the first recognized mineral containing ammine groups. Its formula is [CuCl2(NH3)2]. The mineral is chemically pure. It was found in a guano deposit in Chile. At the same site other ammine-containing minerals were later found:

Chrysothallite is a rare thallium-bearing chloride mineral with the formula K6Cu6Tl3+Cl17(OH)4•H2O. Chrysothallite is unique in being only the second mineral with essential trivalent thallium, a feature shared with natural thallium(III) oxide, avicennite. Another examples of natural thallium chlorides are steropesite, Tl3BiCl6, and lafossaite, TlCl. Chrysothallite is one of numerous fumarolic minerals discovered among fumarolic sites of the Tolbachik volcano, Kamchatka, Russia The mineral is named in allusion to its colour and thallium content.

References

  1. ↑ US EPA, OLEM (8 December 2015). "SW-846 Test Method 9045D: Soil and Waste pH". www.epa.gov.
  2. 1 2 3 NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
  3. ↑ http://www.pyrodata.com/sites/default/files/Copper%20oxychloride.pdf [ bare URL PDF ]
  4. 1 2 3 4 5 6 Handbook of copper compounds and applications. New York: Marcel Dekker. 1997. ISBN   0-8247-8998-9.
  5. 1 2 Steward, F. A. (4 October 2013). "Development and Manufacture of an Innovative Mineral Feed Ingredient Produced from Recycled Copper". Recycling of Metals and Engineercd Materials: 643–654. doi:10.1002/9781118788073.ch55.
  6. ↑ Lubej, Andrej; Koloini, Tine; Pohar, Ciril (June 16, 2004). "Industrial Precipitation of Cupric Hydroxy-Salts" (PDF). Acta Chim. Slov. 51: 751–768.
  7. ↑ Scott, David A. (2000). "A Review of Copper Chlorides and Related Salts in Bronze Corrosion and as Painting Pigments". Studies in Conservation. 45 (1): 39. doi:10.2307/1506682.
  8. ↑ Eastaugh, Nicholas; Walsh, Valentine; Chaplin, Tracey; Siddall, Ruth (30 March 2007). Pigment Compendium: A Dictionary of Historical Pigments (PDF). doi:10.4324/9780080473765. ISBN   0080473768.
  9. ↑ Lamberti, Carlo; Prestipino, Carmelo; Bonino, Francesca; Capello, Luciana; Bordiga, Silvia; Spoto, Giuseppe; Zecchina, Adriano; Diaz Moreno, Sofia; Cremaschi, Barbara; Garilli, Marco; Marsella, Andrea; Carmello, Diego; Vidotto, Sandro; Leofanti, Giuseppe (3 July 2002). "The Chemistry of the Oxychlorination Catalyst: an In Situ, Time-Resolved XANES Study". Angewandte Chemie International Edition. 41 (13): 2341–2344. doi:10.1002/1521-3773(20020703)41:13<2341::AID-ANIE2341>3.0.CO;2-P.
  10. ↑ Ren, Jun; Li, Zhong; Liu, Shusen; Lu, Xinglu; Xie, Kechang (March 2010). "Study on the formation and role of copper chloride hydroxide in the oxidative carbonylation of methanol to dimethyl carbonate". Kinetics and Catalysis. 51 (2): 250–254. doi:10.1134/S0023158410020138.
  11. ↑ Zhang, Zhen; Ma, Xinbin; Zhang, Pingbo; Li, Yeming; Wang, Shengping (April 2007). "Effect of treatment temperature on the crystal structure of activated carbon supported CuCl2–PdCl2 catalysts in the oxidative carbonylation of ethanol to diethyl carbonate". Journal of Molecular Catalysis A: Chemical. 266 (1–2): 202–206. doi:10.1016/j.molcata.2006.11.009.
  12. ↑ Davies, M.J.; Chadwick, D.; Cairns, J.A. (1990). "Identification of A Catalytically Active Copper Oxychloride Phase for The Synthesis of Maleic Anhydride". Studies in Surface Science and Catalysis. 55: 595–603. doi:10.1016/S0167-2991(08)60191-3.
  13. ↑ Deng, FZ; Zhu, AX; Yang, R (February 2006). "[Study on preparation of CuO/Cu2 (OH)3Cl powder and its spectrum behavior for photodegradation decoloration of dyes]". Guang pu xue yu guang pu fen xi = Guang pu. 26 (2): 299–301. PMID   16826911.
  14. ↑ Miles, R.D.; O'Keefe, S.F.; Henry, P.R.; Ammerman, C.B.; Luo, X.G. (March 1998). "The effect of dietary supplementation with copper sulfate or tribasic copper chloride on broiler performance, relative copper bioavailability, and dietary prooxidant activity". Poultry Science. 77 (3): 416–425. doi:10.1093/ps/77.3.416.
  15. ↑ Cromwell, G L; Lindemann, M D; Monegue, H J; Hall, D D; Orr, D E (1998). "Tribasic copper chloride and copper sulfate as copper sources for weanling pigs". Journal of Animal Science. 76 (1): 118. doi:10.2527/1998.761118x.
  16. ↑ Arthington, J. D.; Spears, J. W. (1 March 2007). "Effects of tribasic copper chloride versus copper sulfate provided in corn-and molasses-based supplements on forage intake and copper status of beef heifers1". Journal of Animal Science. 85 (3): 871–876. doi:10.2527/jas.2006-518.
  17. ↑ Wells, A. F. (2 June 1949). "The crystal structure of atacamite and the crystal chemistry of cupric compounds". Acta Crystallographica. 2 (3): 175–180. doi:10.1107/S0365110X49000461.
  18. ↑ Lichtenegger, Helga C.; Schöberl, Thomas; Bartl, Michael H.; Waite, Herbert; Stucky, Galen D. (11 October 2002). "High Abrasion Resistance with Sparse Mineralization: Copper Biomineral in Worm Jaws". Science. 298 (5592): 389–392. doi:10.1126/science.1075433.
  19. ↑ Fleet, M. E. (1 January 1975). "The crystal structure of paratacamite, Cu 2 (OH) 3 Cl". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry. 31 (1): 183–187. doi:10.1107/S0567740875002324.
  20. ↑ Hawthorne, F. C. (March 1985). "Refinement of the crystal structure of botallackite". Mineralogical Magazine. 49 (350): 87–89. doi:10.1180/minmag.1985.049.350.12.
  21. ↑ Frost, R.L. (April 2003). "Raman spectroscopy of selected copper minerals of significance in corrosion". Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy. 59 (6): 1195–1204. doi:10.1016/S1386-1425(02)00315-3.
  22. ↑ Sharkey, J.B.; Lewin, S.Z. (January 1972). "Thermochemical properties of the copper(ii) hydroxychlorides". Thermochimica Acta. 3 (3): 189–201. doi:10.1016/0040-6031(72)85029-9.
  23. ↑ Pollard, A. M.; Thomas, R. G.; Williams, P. A. (December 1989). "Synthesis and stabilities of the basic copper(II) chlorides atacamite, paratacamite and botallackite". Mineralogical Magazine. 53 (373): 557–563. doi:10.1180/minmag.1989.053.373.06.
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.