| Revision as of 15:47, 24 June 2011 editMerlIwBot (talk | contribs)27,490 editsm robot Adding: ar:كربونات النحاس الثنائي Modifying: de:Basisches Kupfercarbonat← Previous edit |
Latest revision as of 05:08, 4 August 2024 edit undo76.14.33.76 (talk) Removed Greenium from the list of "Other Names." Greenium is not another name for Basic Copper Carbonate. I've looked online, and the only sources are those that scraped Misplaced Pages. I looked in Google Books for any chemistry book that uses the name Greenium in any context and there were none. If you believe that the common name Greenium should be added back, please include a source. |
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{{short description|Chemical compound}} |
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{{For|the neutral compound|Copper(II) carbonate}} |
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{{chembox |
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{{chembox |
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| Verifiedfields = changed |
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| verifiedrevid = 399730272 |
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| Watchedfields = changed |
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| Name = Copper(II) carbonate |
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| verifiedrevid = 435993456 |
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| ImageFile = Copper carbonate basic.jpg |
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| ImageSize = 200px |
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| Name = |
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| ImageName = Copper (II) carbonate |
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| ImageFile = Copper carbonate basic.jpg |
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| OtherNames = copper carbonate, cupric carbonate, basic copper carbonate |
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| ImageName = Basic copper carbonate |
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| ImageFile2 = Malachite-formula-unit-and-coordination-fade-25-from-xtal-3D-bs-17-25.png |
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| Section1 = {{Chembox Identifiers |
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| ImageCaption2 = ] of part of the ] of ], highlighting the formula unit |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| IUPACName = Dicopper carbonate dihydroxide |
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| ChemSpiderID = 13799 |
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| OtherNames = copper carbonate hydroxide, cupric carbonate, copper carbonate |
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| InChI = 1/CH2O3.Cu/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 |
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| SystematicName = |
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| InChIKey = GEZOTWYUIKXWOA-NUQVWONBAA |
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| Section1 = {{Chembox Identifiers |
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| SMILES = .C()=O |
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| PubChem = 25503 |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| ChemSpiderID = 23796 |
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| StdInChI = 1S/CH2O3.Cu/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 |
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| SMILES = C(=O)().... |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| InChI = 1/CH2O3.2Cu.2H2O/c2-1(3)4;;;;/h(H2,2,3,4);;;2*1H2/q;2*+2;;/p-4 |
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| StdInChIKey = GEZOTWYUIKXWOA-UHFFFAOYSA-L |
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| InChIKey = ZMMDPCMYTCRWFF-XBHQNQODAP |
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| CASNo = 1184-64-1 |
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| StdInChI = 1S/CH2O3.2Cu.2H2O/c2-1(3)4;;;;/h(H2,2,3,4);;;2*1H2/q;2*+2;;/p-4 |
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| PubChem = 14452 |
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| StdInChIKey = ZMMDPCMYTCRWFF-UHFFFAOYSA-J |
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| RTECS = FF950000 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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}} |
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| CASNo = 12069-69-1 |
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| Section2 = {{Chembox Properties |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| Formula = CuCO<sub>3</sub> |
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| UNII = GIK928GH0Y |
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| MolarMass = 123.555 g/mol |
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| RTECS = |
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| Density = 3.9 g/cm<sup>3</sup> |
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}} |
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| Solvent = other solvents |
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| Section2 = {{Chembox Properties |
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| SolubleOther = insoluble in water, found effective in melting ice, soluble in ethanoic acid |
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| Formula = Cu<sub>2</sub>(OH)<sub>2</sub>CO<sub>3</sub> |
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| MeltingPt = 200 °C |
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| MolarMass = 221.114 g/mol |
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| BoilingPt = decomposes at 290 °C |
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| pKsp = 9.85 }} |
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| Appearance = green powder |
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| Density = 4 g/cm<sup>3</sup> |
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| Section7 = {{Chembox Hazards |
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| Solubility = insoluble |
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| ExternalMSDS = }} |
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| MeltingPtC = 200 |
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}} |
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| BoilingPtC = 290 |
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'''Copper(II) carbonate''' (often called '''copper carbonate''' or '''cupric carbonate''') is a blue-green ] (chemical formula CuCO<sub>3</sub>) forming part of the ] ] that is found on weathered ], ], and ]. The colour can vary from bright blue to green, because there may be a mixture of both copper carbonate and basic copper carbonate in various stages of ]. It was formerly much used as a ], and is still in use for artist's colours. |
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| BoilingPt_notes = decomposes |
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It has also been used in some types of make-up, like ], although it can also be toxic to humans. It also has been used for many years as an effective algaecide in farm ponds and in aquaculture operations. Copper carbonate was the first compound to be broken down into several, separate elements (copper, carbon, and oxygen). It was broken down in 1794 by the French chemist ] (1754–1826). When burnt, it thermally decomposes to form CO<sub>2</sub> and CuO, a black solid. It can be used to ] a ] surface by adding sulfuric acid and heat it (to produce ]) then passing a charge through it with the metal in the liquid. This process is known as ]. |
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| SolubilityProduct = 7.08·10<sup>−9</sup> |
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}} |
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| Section3 = |
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| Section4 = {{Chembox Thermochemistry |
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| DeltaHf = −595 kJ/mol |
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| Entropy = 88 J/mol·K |
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}} |
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| Section5 = |
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| Section6 = |
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| Section7 = {{Chembox Hazards |
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| ExternalSDS = |
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| LD50 = 159 mg/kg (rat, oral) |
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| MainHazards = |
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| GHSPictograms = {{GHS07}}<ref name="sigma"></ref> |
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| GHSSignalWord = Warning |
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| HPhrases = {{H-phrases|302|315|319|335}}<ref name="sigma" /> |
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| PPhrases = {{P-phrases|261|305+351+338}}<ref name="sigma" /> |
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| PEL = TWA 1 mg/m<sup>3</sup> (as Cu)<ref name=PGCH>{{PGCH|0150}}</ref> |
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| REL = TWA 1 mg/m<sup>3</sup> (as Cu)<ref name=PGCH/> |
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| IDLH = TWA 100 mg/m<sup>3</sup> (as Cu)<ref name=PGCH/> |
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}} |
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}} |
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'''Basic copper carbonate''' is a chemical compound, more properly called '''copper(II) carbonate hydroxide'''. It can be classified as a ] or a ]. It consists of ] bonded to ] and ] with formula {{chem2|Cu2(CO3)(OH)2}}. It is a green solid that occurs in nature as the mineral ]. It has been used since antiquity as a ], and it is still used as such in artist paints, sometimes called '''verditer''', '''green bice''', or '''mountain green'''.<ref name=Ullmann>{{cite book |doi=10.1002/14356007.a07_567.pub2 |chapter=Copper Compounds |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2016 |last1=Zhang |first1=Jun |last2=Richardson |first2=H. Wayne |pages=1–31 |isbn=978-3-527-30673-2 }}</ref> |
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Sometimes basic copper carbonate refers to {{chem|Cu|3}}({{chem|C|O|3}})<sub>2</sub>({{chem|OH}})<sub>2</sub>, a blue crystalline solid also known as the mineral ]. It too has been used as pigment, sometimes under the name '''mountain blue''' or '''blue verditer'''. |
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] on roofs of ].]] |
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Both ] and ] can be found in the ] ] that is found on weathered ], ], and ]. The composition of the patina can vary, in a maritime environment depending on the environment a basic chloride may be present, in an urban environment basic sulfates may be present.<ref>Encyclopedia Of Corrosion Technology (Google eBook), Philip A. Schweitzer P.E.; CRC Press, 2004, {{ISBN|08247-4878-6}}</ref> |
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Copper in moist air slowly acquires a dull green coating because its top layer has oxidised with the air. Some architects use this material on rooftops for this interesting colour. The green material is a 1:1 mole mixture of ] and CuCO<sub>3</sub>:<ref>Masterson, W. L., & Hurley, C. N. (2004). ''Chemistry: Principals and Reactions, 5th Ed''. Thomson Learning, Inc. (p 498).</ref> |
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This compound is often improperly called (even in chemistry articles) '''copper carbonate''', '''cupric carbonate''', and similar names. The true (neutral) ] CuCO<sub>3</sub> is not known to occur naturally.<ref>{{Holleman&Wiberg|page=1263}}</ref> It is decomposed by water or moisture from the air. It was synthesized only in 1973 by high temperature and very high pressures.<ref name="SeidelEhrhardt1974">{{cite journal|last1=Seidel|first1=H.|last2=Ehrhardt|first2=H.|last3=Viswanathan|first3=K.|last4=Johannes|first4=W.|title=Darstellung, Struktur und Eigenschaften von Kupfer(II)-Carbonat|journal=Zeitschrift für anorganische und allgemeine Chemie|volume=410|issue=2|year=1974|pages=138–148|issn=0044-2313|doi=10.1002/zaac.19744100207}}</ref> |
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:2 Cu (s) + H<sub>2</sub>O (g) + CO<sub>2</sub> + O<sub>2</sub> → Cu(OH)<sub>2</sub> + CuCO<sub>3</sub> (s) |
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Copper carbonate decomposes at 290 °C, giving off ] and leaving ]: |
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:CuCO<sub>3</sub> (s) → CuO (s) + CO<sub>2</sub> (g) |
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'''Basic copper(II) carbonate''' occurs naturally as ] (Cu<sub>2</sub>(OH)<sub>2</sub>CO<sub>3</sub>) and ] (Cu<sub>3</sub>(OH)<sub>2</sub>(CO<sub>3</sub>)<sub>2</sub>). |
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==Preparation== |
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==Preparation== |
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] on roofs of ].]] |
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Copper carbonate is prepared by combining aqueous solutions of copper sulfate and ]. Copper basic carbonate precipitates from the solution: |
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Basic copper carbonate is prepared by combining aqueous solutions of ] and ]. Basic copper carbonate precipitates from the solution, with release of ] {{chem|C|O|2}}:<ref name="hep">Jack Reginald Irons Hepburn (1927): "The chemical nature of precipitated basic cupric carbonate". Article CCCLXXXVI, ''Journal of the Chemical Society'' (Resumed), volume 1927, pp. 2883–2896. {{doi|10.1039/JR9270002883}}</ref> |
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:{{chem2|2CuSO4 + 2Na2CO3 + H2O -> Cu2(OH)2CO3 + 2Na2SO4 + CO2}} |
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Basic copper carbonate can also be prepared by treating aqueous solutions of ] with ]. |
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: 2 CuSO<sub>4</sub> + 2 Na<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O → Cu<sub>2</sub>(OH)<sub>2</sub>CO<sub>3</sub> + 2 Na<sub>2</sub>SO<sub>4</sub> + CO<sub>2</sub> |
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] may also be substituted with ]. |
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The formation of copper carbonate can be verified in the following steps: |
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a) Centrifuge the above mentioned solution, 1 minute at 6000 g is sufficient |
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b) Wash the precipitate with distilled water and centrifuge again |
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c) The colour of the precipitate is blue, like that of several copper salts but none of the sodium salts |
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d) If dilute (1M) hydrochloric acid is added, then bubbles of CO<sub>2</sub> will emerge and the precipitate will be fully solubilised. These would not be formed if dilute hydrochloric acid was added to solid Na<sub>2</sub>SO<sub>4</sub>. |
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== Reactions == |
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Pure copper carbonate is obtained from basic copper carbonate in the presence of carbon dioxide at 180 °C and 4.6 MPa (46 atm) pressure. {{Citation Needed|Please give a reliable resource.|date=February 2011}} |
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Basic copper carbonate is decomposed by acids, such as solutions of ] {{chem|H|Cl}}, into the copper(II) salt and carbon dioxide. |
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In 1794 the French chemist ] (1754–1826) thermally decomposed copper carbonate to CO<sub>2</sub> and CuO, ].<ref>{{Cite journal |last=Kapoor |first=Satish C. |date=1965 |title=Berthollet, Proust, and Proportions |url=https://www.jstor.org/stable/27757247 |journal=Chymia |volume=10 |pages=53–110 |doi=10.2307/27757247 |issn=0095-9367}}</ref> |
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==Reactions== |
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The basic copper carbonates, malachite and azurite, both decompose forming H<sub>2</sub>O, CO<sub>2</sub>, and CuO, ].<ref name="BrownMackenzie1984">{{cite journal|last1=Brown|first1=I.W.M.|last2=Mackenzie|first2=K.J.D.|last3=Gainsford|first3=G.J.|title=Thermal decomposition of the basic copper carbonates malachite and azurite|journal=Thermochimica Acta|volume=75|issue=1–2|year=1984|pages=23–32|issn=0040-6031|doi=10.1016/0040-6031(84)85003-0}}</ref> |
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<big>1) Reaction with acids:</big> |
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==Uses== |
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copper carbonate reacts with acids and gives carbon dioxide and corresponding copper(II) salts of that acid: |
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Basic copper carbonate is used to remove thiols and hydrogen sulfide from some gas streams, a process called "sweetening". Like many other copper compounds, it also has been used as an ], ] and similar applications. It is a precursor to various catalysts and copper soaps.<ref name=Ullmann/> |
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Both malachite and azurite, as well as synthetic basic copper carbonate have been used as ]s.<ref>Valentine Walsh, Tracey Chaplin, ''Pigment Compendium: A Dictionary and Optical Microscopy of Historical Pigments'', 2008, Routledge, {{ISBN|978-0-7506-8980-9}}</ref> One example of the use of both ] and its artificial form blue verditer<ref>, ColourLex</ref> is the portrait of the family of ] by ].<ref>Robert L. Feller, Rubens’s: The Gerbier Family: Technical Examination of the Pigments and Paint Layers, ''Studies in the History of Art'', Vol. 5 (1973), pp. 54–74.</ref> The green skirt of Deborah Kip is painted in ], ], blue verditer (artificial form of azurite), ], ] and yellow lake. The green color is achieved by mixing blue and yellow pigments.<ref>, ColourLex</ref> |
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*copper carbonate + hydrochloric acid → copper chloride + water + carbon dioxide: |
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:CuCO<sub>3</sub> + 2HCl → CuCl<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub> |
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*copper carbonate + sulfuric acid → copper sulfate + water + carbon dioxide: |
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:CuCO<sub>3</sub> + H<sub>2</sub>SO<sub>4</sub> → CuSO<sub>4</sub> + H<sub>2</sub>O + CO<sub>2</sub> |
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*copper carbonate + nitric acid → copper nitrate + water + carbon dioxide: |
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:CuCO<sub>3</sub> + 2HNO<sub>3</sub> → Cu(NO<sub>3</sub>)<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub> |
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*copper carbonate + acetic acid → copper acetate + water + carbon dioxide: |
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:CuCO<sub>3</sub> + 2CH<sub>3</sub>COOH → Cu(CH<sub>3</sub>COO)<sub>2</sub> + H<sub>2</sub>O +CO<sub>2</sub> |
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<big>2) Decomposition:</big> |
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*copper carbonate decomposes at 290°C and forms copper(II) oxide: |
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CuCO<sub>3</sub> → CuO + CO<sub>2</sub> |
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==References== |
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==References== |
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==External links== |
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==External links== |
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{{Commons cat|Copper(II) carbonate}} |
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{{Commons category|Basic copper carbonate}} |
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* at ColourLex |
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* at ColourLex |
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{{Clear}} |
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{{carbonates}} |
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{{Copper compounds}} |
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{{Copper compounds}} |
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{{DEFAULTSORT:Copper(Ii) Carbonate}} |
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{{DEFAULTSORT:Copper(Ii) Carbonate}} |
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