Copper(II) hydroxide

Copper(II) hydroxide is the hydroxide of copper with the chemical formula of Cu(OH)2. It is a pale greenish blue or bluish green solid. Some forms of copper(II) hydroxide are sold as "stabilized" copper(II) hydroxide, although they likely consist of a mixture of copper(II) carbonate and hydroxide. Cupric hydroxide is a weak base.

Copper(II) hydroxide
Names
IUPAC name
Copper(II) hydroxide
Other names
Cupric hydroxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.039.817
KEGG
UNII
Properties
Cu(OH)2
Molar mass 97.561 g/mol
Appearance Blue or blue-green solid
Density 3.368 g/cm3, solid
Melting point 80 °C (176 °F; 353 K) (decomposes into CuO)
negligible
2.20 x 10−20[1]
Solubility insoluble in ethanol;
soluble in NH4OH
+1170.0·10−6 cm3/mol
Thermochemistry
108 J·mol−1·K−1
−450 kJ·mol−1
Hazards
Main hazards Skin, Eye, & Respiratory Irritant
Safety data sheet http://www.sciencelab.com/xMSDS-Cupric_Hydroxide-9923594
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
2
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1000 mg/kg (oral, rat)
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(II) oxide
Copper(II) carbonate
Copper(II) sulfate
Copper(II) chloride
Other cations
 Nickel(II) hydroxide
Zinc hydroxide
Iron(II) hydroxide
Cobalt hydroxide
Related compounds
 Copper(I) oxide
Copper(I) chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Occurrence

Copper(II) hydroxide has been known since copper smelting began around 5000 BC although the alchemists were probably the first to manufacture it by mixing solutions of lye (sodium or potassium hydroxide) and blue vitriol (copper(II) sulfate).[3] Sources of both compounds were available in antiquity.

It was produced on an industrial scale during the 17th and 18th centuries for use in pigments such as blue verditer and Bremen green.[4] These pigments were used in ceramics and painting.[5]

Laboratory synthesis

Copper(II) hydroxide can be produced by adding a sodium hydroxide to a dilute solution of copper(II) sulfate (CuSO4·5H2O).[6] The precipitate produced in this manner, however, often contains water and an appreciable amount of sodium hydroxide impurity. A purer product can be attained if ammonium chloride is added to the solution beforehand.[7] Alternatively, copper hydroxide is readily made by electrolysis of water (containing a little electrolyte such as sodium sulfate, or magnesium sulfate) with a copper anode.

Mineral

The mineral of the formula Cu(OH)2 is called spertiniite. Copper(II) hydroxide is rarely found as an uncombined mineral because it slowly reacts with carbon dioxide from the atmosphere to form a basic copper(II) carbonate. Thus copper slowly acquires a dull green coating in moist air by the reaction:

2 Cu(OH)2 + CO2 → Cu2CO3(OH)2 + H2O

The green material is in principle a 1:1 mole mixture of Cu(OH)2 and CuCO3.[8] This patina forms on bronze and other copper alloy statues such as the Statue of Liberty.

Structure

The structure of Cu(OH)2 has been determined by X-ray crystallography The copper center is square pyramidal. Four Cu-O distances in the plane range are 1.96 Å, and the axial Cu-O distance is 2.36 Å. The hydroxide ligands in the plane are either doubly bridging or triply bridging.[9]

Reactions

It is stable to about 100 °C.[6]

Copper(II) hydroxide reacts with a solution of ammonia to form a deep blue solution of tetramminecopper [Cu(NH3)4]2+ complex ion.


Copper(II) hydroxide catalyzes the oxidation of ammonia solutions in presence of dioxygen, giving rise to copper ammine nitrites, such as Cu(NO2)2(NH3)n.[10][11]

Copper(II) hydroxide is mildly amphoteric. It dissolves slightly in concentrated alkali, forming [Cu(OH)4]2−.[12][6]


Reagent for organic chemistry

Copper(II) hydroxide has a rather specialized role in organic synthesis. Often, when it is utilized for this purpose, it is prepared in situ by mixing a soluble copper(II) salt and potassium hydroxide.

It is sometimes used in the synthesis of aryl amines. For example, copper(II) hydroxide catalyzes the reaction of ethylenediamine with 1-bromoanthraquinone or 1-amino-4-bromoanthraquinone to form 1-((2-aminoethyl)amino)anthraquinone or 1-amino-4-((2-aminoethyl)amino)anthraquinone, respectively:[13]

Copper(II) hydroxide also converts acid hydrazides to carboxylic acids at room temperature. This conversion is useful in the synthesis of carboxylic acids in the presence of other fragile functional groups. The yields are generally excellent as is the case with the production of benzoic acid and octanoic acid:[13]

Uses

Copper(II) hydroxide in ammonia solution, known as Schweizer's reagent, possesses the interesting ability to dissolve cellulose. This property led to it being used in the production of rayon, a cellulose fiber.

It is also used widely in the aquarium industry for its ability to destroy external parasites in fish, including flukes, marine ich, brook and marine velvet, without killing the fish. Although other water-soluble copper compounds can be effective in this role, they generally result in high fish mortality.

Copper(II) hydroxide has been used as an alternative to the Bordeaux mixture, a fungicide and nematicide.[14] Such products include Kocide 3000, produced by Kocide L.L.C. Copper(II) hydroxide is also occasionally used as ceramic colorant.

Copper(II) hydroxide has been combined with latex paint, making a product designed to control root growth in potted plants. Secondary and lateral roots thrive and expand, resulting in a dense and healthy root system. It was sold under the name Spin Out, which was first introduced by Griffin L.L.C. The rights are now owned by SePRO Corp.[15] It is now sold as Microkote either in a solution you apply yourself, or as treated pots.

Other copper(II) hydroxides
Chemical structure of azurite, one of many copper(II) hydroxides (color code: red = O, green = Cu, gray = C, white = H).[16]

Together with other components, copper(II) hydroxides are numerous. Several copper(II)-containing minerals contain hydroxide. Notable examples include azurite, malachite, antlerite, and brochantite. Azurite (2CuCO3·Cu(OH)2) and malachite (CuCO3·Cu(OH)2) are hydroxy-carbonates, whereas antlerite (CuSO4·2Cu(OH)2) and brochantite (CuSO4·3Cu(OH)2) are hydroxy-sulfates.

Many synthetic copper(II) hydroxide derivatives have been investigated.[17]

References
  1. Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
  3. Richard Cowen, Essays on Geology, History, and People, Chapter 3: "Fire and Metals: Copper".
  4. Tony Johansen, Historic Artist's Pigments Archived 2009-06-09 at the Wayback Machine. PaintMaking.com. 2006.
  5. Blue verditer Archived 2007-09-27 at the Wayback Machine. Natural Pigments. 2007.
  6. O. Glemser and H. Sauer "Copper(II) Hydroxide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1013.
  7. Y. Cudennec, A. Lecerf (2003). "The transformation of Cu(OH)2 into CuO, revisited" (PDF). Solid State Sciences. 5 (11–12): 1471–1474. doi:10.1016/j.solidstatesciences.2003.09.009.
  8. Masterson, W. L., & Hurley, C. N. (2004). Chemistry: Principles and Reactions, 5th Ed. Thomson Learning, Inc. (p 331)"
  9. H. R. Oswald, A. Reller, H. W. Schmalle, E. Dubler (1990). "Structure of Copper(II) Hydroxide, Cu(OH)2". Acta Crystallogr. C46 (12): 2279–2284. doi:10.1107/S0108270190006230.CS1 maint: uses authors parameter (link)
  10. Y. Cudennec; et al. (1995). "Etude cinétique de l'oxydation de l'ammoniac en présence d'ions cuivriques". Comptes Rendus de l'Académie des Sciences, Série IIB. 320 (6): 309–316.
  11. Y. Cudennec; et al. (1993). "Synthesis and study of Cu(NO2)2(NH3)4 and Cu(NO2)2(NH3)2". European Journal of Solid State and Inorganic Chemistry. 30 (1–2): 77–85.
  12. Pauling, Linus (1970). General Chemistry. Dover Publications, Inc. (p 702).
  13. Tsuda, T. (2001). "Copper(II) Hydroxide". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rc228. ISBN 0471936235.
  14. Bordeaux Mixture. UC IPM online. 2007.
  15. "SePRO Corporation".
  16. Zigan, F.; Schuster, H.D. (1972). "Verfeinerung der Struktur von Azurit, Cu3(OH)2(CO3)2, durch Neutronenbeugung". Zeitschrift für Kristallographie, Kristallgeometrie, Kristallphysik, Kristallchemie. 135 (5–6): 416–436. doi:10.1524/zkri.1972.135.5-6.416.
  17. Kondinski, A.; Monakhov, K. (2017). "Breaking the Gordian Knot in the Structural Chemistry of Polyoxometalates: Copper(II)–Oxo/Hydroxo Clusters". Chemistry: A European Journal. 23 (33): 7841–7852. doi:10.1002/chem.201605876. PMID 28083988.
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