| Revision as of 12:40, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 476064991 of page Copper(II)_chloride for the Chem/Drugbox validation project (updated: 'ChEMBL'). |
Latest revision as of 17:00, 25 October 2024 edit 42.110.173.174 (talk) →Co-catalyst in Wacker processTags: Mobile edit Mobile web edit |
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{{good article}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{chembox |
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{{chembox |
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| Watchedfields = changed |
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| Watchedfields = changed |
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| verifiedrevid = 460120755 |
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| verifiedrevid = 476995602 |
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| ImageFile = Tolbachite-3D-balls.png |
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| ImageFile = Tolbachite-3D-balls.png |
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| ImageCaption = Anhydrous |
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| ImageCaption = Anhydrous{{legend|rgb(256, 128, 80)|], Cu}}{{legend|lime|], Cl}} |
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| ImageFile1 = Copper(II) chloride.jpg |
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| ImageFile1 = Copper(II) chloride.jpg |
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| ImageCaption1 = Anhydrous |
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| ImageCaption1 = Anhydrous |
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| ImageFile2 = Cupric chloride.jpg |
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| ImageFile2 = Cupric chloride.jpg |
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| ImageCaption2 = Dihydrate |
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| ImageCaption2 = Dihydrate |
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| IUPACName = Copper(II) chloride<br />Copper dichloride |
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| IUPACName = Copper(II) chloride |
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| OtherNames = Cupric chloride |
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| OtherNames = Cupric chloride |
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| Section1 = {{Chembox Identifiers |
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| Section1 = {{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 148374 |
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| ChemSpiderID = 148374 |
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| ChEMBL_Ref = {{ebicite|changed|EBI}} |
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| ChEMBL_Ref = {{ebicite|correct|EBI}} |
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| ChEMBL = <!-- blanked - oldvalue: 1200553 --> |
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| ChEMBL = 1200553 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = P484053J2Y |
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| InChI = 1/2ClH.Cu/h2*1H;/q;;+2/p-2/rCl2Cu/c1-3-2 |
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| InChI = 1/2ClH.Cu/h2*1H;/q;;+2/p-2/rCl2Cu/c1-3-2 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 49553 |
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| ChEBI = 49553 |
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| SMILES = ClCl |
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| SMILES = .. |
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| SMILES_Comment = anhydrous |
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| SMILES1 = Cl(Cl)() |
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| SMILES1_Comment = dihydrate |
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| InChIKey = ORTQZVOHEJQUHG-LRIOHBSEAE |
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| InChIKey = ORTQZVOHEJQUHG-LRIOHBSEAE |
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| InChI1 = 1/2ClH.Cu/h2*1H;/q;;+2/p-2 |
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| InChI1 = 1/2ClH.Cu/h2*1H;/q;;+2/p-2 |
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| InChIKey1 = ORTQZVOHEJQUHG-NUQVWONBAE |
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| InChIKey1 = ORTQZVOHEJQUHG-NUQVWONBAE |
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| SMILES1 = .. |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/2ClH.Cu/h2*1H;/q;;+2/p-2 |
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| StdInChI = 1S/2ClH.Cu/h2*1H;/q;;+2/p-2 |
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| CASNo = 7447-39-4 |
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| CASNo = 7447-39-4 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo2_Ref = {{cascite|correct|CAS}} |
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| CASOther = <br/>10125-13-0 (dihydrate) |
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| CASNo2 = 10125-13-0 |
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| CASNo2_Comment= (dihydrate) |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = P484053J2Y |
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| UNII2_Ref = {{fdacite|correct|FDA}} |
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| UNII2 = S2QG84156O |
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| UNII2_Comment = (dihydrate) |
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| PubChem = 24014 |
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| PubChem = 24014 |
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| RTECS = GL7000000 |
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| RTECS = GL7000000 |
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| Gmelin = 9300 |
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| Beilstein = 8128168 |
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| DrugBank = DB09131 |
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| UNNumber = 2802 |
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| EC_number = 231-210-2 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = CuCl<sub>2</sub> |
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| Formula = {{chem2|CuCl2 |
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}} |
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| MolarMass = 134.45 g/mol (anhydrous)<br/>170.48 g/mol (dihydrate) |
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| Appearance = yellow-brown solid (anhydrous)<br/>blue-green solid (dihydrate) |
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| MolarMass = 134.45 g/mol (anhydrous)<br />170.48 g/mol (dihydrate) |
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| Appearance = dark brown solid (anhydrous)<br />light blue solid (dihydrate) |
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| Odor = odorless |
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| Odor = odorless |
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| Density = 3.386 g/cm<sup>3</sup> (anhydrous) <br /> 2.51 g/cm<sup>3</sup> (dihydrate) |
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| Density = 3.386 g/cm<sup>3</sup> (anhydrous) <br /> 2.51 g/cm<sup>3</sup> (dihydrate) |
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| Solubility = 70.6 g/100 mL (0 °C) <br> 75.7 g/100 mL (25 °C) <br> 107.9 g/100 mL (100 °C) |
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| Solubility = 70.6 g/(100 mL) (0 °C) <br> 75.7 g/(100 mL) (25 °C) <br> 107.9 g/(100 mL) (100 °C) |
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| SolubleOther = ''methanol:'' <br> 68 g/ 100 mL (15 °C) <hr> ''ethanol:'' <br> 53 g/100 mL (15 °C) <br> soluble in ] |
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| SolubleOther = ''methanol:''<br>68 g/(100 mL) (15 °C) |
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<br/>''ethanol:''<br>53 g/(100 mL) (15 °C) <br> soluble in ] |
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| MeltingPtC = 630 |
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| MeltingPt = 498 °C (anhydrous) <br /> 100 °C (dehydration of dihydrate) |
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| MeltingPt_notes = (extrapolated)<br /> 100 °C (dehydration of dihydrate) |
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| BoilingPt = 993 °C (anhydrous, decomp) |
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| BoilingPtC = 993 |
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| BoilingPt_notes = (anhydrous, decomposes) |
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| MagSus = +1080·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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| Section3 = {{Chembox Structure |
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| Section3 = {{Chembox Structure |
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| Structure_ref = <ref>{{cite journal |author1=A. F. Wells |title=The crystal structure of anhydrous cupric chloride, and the stereochemistry of the cupric atom |journal=Journal of the Chemical Society |date=1947 |pages=1670–1675 |doi=10.1039/JR9470001670 |language=en}}</ref><ref>{{cite journal |author1=Sydney Brownstein |author2=Nam Fong Han |author3=Eric Gabe |author4=Yvon LePage |title=A redetermination of the crystal structure of cupric chloride dihydrate |journal=Zeitschrift für Kristallographie |date=1989 |volume=189 |issue=1 |pages=13–15 |doi=10.1524/zkri.1989.189.1-2.13 |bibcode=1989ZK....189...13B |language=en}}</ref> |
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| CrystalStruct = ] (β = 121°) (anhydrous) <br> ] (dihydrate) |
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| SpaceGroup = C2/m (anhydrous) <br> ''Pbmn'' (dihydrate) |
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| PointGroup = |
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| LattConst_a = 6.85 Å (anhydrous) <br> 7.41 Å (dihydrate) |
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| LattConst_b = 3.30 Å (anhydrous) <br> 8.09 Å (dihydrate) |
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| LattConst_c = 6.70 Å (anhydrous) <br> 3.75 Å (dihydrate) |
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| UnitCellVolume = |
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| Coordination = ] |
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| Coordination = ] |
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| MolShape = |
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| CrystalStruct = distorted ] |
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| OrbitalHybridisation = |
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| Dipole = |
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| Section7 = {{Chembox Hazards |
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}} |
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| ExternalMSDS = |
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| Section7 = {{Chembox Hazards |
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| ExternalSDS = |
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| NFPA-H = 2 |
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| NFPA-H = 2 |
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| NFPA-F = 0 |
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| NFPA-F = 0 |
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| NFPA-R = 1 |
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| NFPA-R = 1 |
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| GHSPictograms = {{GHS05}}{{GHS06}}{{GHS07}}{{GHS09}} |
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| EUClass = Not listed |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|301|302|312|315|318|319|335|410|411}} |
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| PPhrases = {{P-phrases|261|264|270|271|273|280|301+310|301+312|302+352|304+340|305+351+338|310|312|321|322|330|332+313|337+313|362|363|391|403+233|405|501}} |
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| FlashPt = Non-flammable |
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| FlashPt = Non-flammable |
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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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| Section8 = {{Chembox Related |
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| Section8 = {{Chembox Related |
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| OtherAnions = ]<br/>] |
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| OtherAnions = ]<br />] |
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| OtherCations = ]<br/>]<br/>] |
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| OtherCations = ]<br />]<br />] |
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'''Copper(II) chloride''', also known as '''cupric chloride''', is an ] with the ] {{chem2|CuCl2|auto=1}}. The ] yellowish-brown ] form slowly absorbs moisture to form the orthorhombic blue-green ] {{chem2|CuCl2*2H2O}}, with two ]. It is industrially produced for use as a ] in the ]. |
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Both the anhydrous and the dihydrate forms occur naturally as the rare minerals '''tolbachite''' and '''eriochalcite''', respectively. |
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==Structure== |
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], Cu}}{{legend|red|], O}}{{legend|lime|], Cl}}{{legend|white|], H}}]] |
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Anhydrous copper(II) chloride adopts a distorted ] structure. In this structure, the ] centers are ]. Most copper(II) compounds exhibit distortions from idealized ] due to the ], which in this case describes the localization of one ] into a ] that is strongly ] with respect to a pair of chloride ligands. In {{chem2|CuCl2*2H2O}}, the copper again adopts a highly distorted octahedral geometry, the Cu(II) centers being surrounded by two water ligands and four chloride ligands, which ] asymmetrically to other Cu centers.<ref>{{Cite book |last=Wells |first=A.F. |title=Structural Inorganic Chemistry |publisher=Clarendon Press |year=1984 |isbn=0-19-855370-6 |location=Oxford |page=253}}</ref><ref name="greenwood" /> |
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Copper(II) chloride is ]. Of historical interest, {{chem2|CuCl2*2H2O}} was used in the first ] measurements by ] in 1944.<ref>{{cite book|url=https://books.google.com/books?id=FldqbSffUMgC&pg=PA167|page=167|title=Mechanochemistry in Nanoscience and Minerals Engineering|author=Peter Baláž|publisher=Springer|year=2008|isbn=978-3-540-74854-0}}</ref><ref>{{cite book|url=https://books.google.com/books?id=l3F9yUSk-rgC&pg=PA3|page=3|title=Electron paramagnetic resonance: a practitioner's toolkit|author=Carlo Corvaja|publisher=John Wiley and Sons|year=2009|isbn=978-0-470-25882-8}}</ref> |
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==Properties and reactions== |
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] |
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Aqueous solutions prepared from copper(II) chloride contain a range of copper(II) ] depending on ], temperature, and the presence of additional ]. These species include the blue color of {{chem2|(2+)}} and the yellow or red color of the halide complexes of the formula {{chem2|^{''x''−}|}}.<ref name="greenwood">Greenwood, N. N. and Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. p. 1183–1185 {{ISBN|0-7506-3365-4}}.</ref> |
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===Hydrolysis=== |
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When copper(II) chloride solutions are treated with a ], a ] of ] occurs:<ref name="Ullmann" /> |
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:{{chem2|CuCl2 + 2 NaOH → Cu(OH)2 + 2 NaCl}} |
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Partial hydrolysis gives ], {{chem2|Cu2(OH)3Cl}}, a popular fungicide.<ref name="Ullmann" /> When an aqueous solution of copper(II) chloride is left in the air and isn't stabilized by a small amount of acid, it is prone to undergo slight hydrolysis.<ref name="greenwood" /> |
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===Redox and decomposition=== |
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Copper(II) chloride is a mild ]. It starts to decompose to ] and ] around {{convert|400|C}} and is completely decomposed near {{convert|1000|C}}:<ref name="Ullmann">{{Cite book|title=Ullmann's Encyclopedia of Industrial Chemistry|author1=Zhang, J. |author2=Richardson, H. W.|year=2016|isbn=978-3-527-30673-2|chapter=Copper Compounds|pages=1–31 |doi=10.1002/14356007.a07_567.pub2}}</ref><ref name="tgdta">{{cite journal |author1=Shuiliang Zhou |author2=Shaobo Shen |author3=Dalong Zhao |author4=Zhitao Zhang |author5=Shiyu Yan |title=Evaporation and decomposition of eutectics of cupric chloride and sodium chloride |journal=Journal of Thermal Analysis and Calorimetry |date=2017 |volume=129 |issue=3 |pages=1445–1452 |doi=10.1007/s10973-017-6360-y |s2cid=99924382 |language=en}}</ref><ref name="Kirk">{{Cite book|title=Kirk-Othmer Encyclopedia of Chemical Technology|last=Richardson|first=H. W.|year=2003|isbn=0471238961|chapter=Copper Compounds|doi=10.1002/0471238961.0315161618090308.a01.pub2}}</ref><ref name="cucl">{{cite journal |author1=Z. Wang |author2=G. Marin |author3=G. F. Naterer |author4=K. S. Gabriel |title=Thermodynamics and kinetics of the thermal decomposition of cupric chloride in its hydrolysis reaction |journal=Journal of Thermal Analysis and Calorimetry |date=2015 |volume=119 |issue=2 |pages=815–823 |doi=10.1007/s10973-014-3929-6 |s2cid=93668361 |url=https://research.library.mun.ca/13446/1/2015-JTAC.pdf |language=en}}</ref> |
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:{{chem2|2 CuCl2 → 2 CuCl + Cl2}} |
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The reported ] of copper(II) chloride of {{convert|498|C}} is a melt of a mixture of copper(I) chloride and copper(II) chloride. The true melting point of {{convert|630|C}} can be extrapolated by using the melting points of the mixtures of CuCl and {{chem2|CuCl2}}.<ref>{{cite journal |author1=Wilhelm Biltz |author2=Werner Fischer |title=Beiträge zur systematischen Verwandtschaftslehre. XLIII. Über das System Cupro-/Cuprichlorid |journal=Zeitschrift für anorganische und allgemeine Chemie |date=1927 |volume=166 |issue=1 |pages=290–298 |doi=10.1002/zaac.19271660126 |language=de}}</ref><ref name="group">{{cite book |author1=A. G. Massey |author2=N. R. Thompson |author3=B. F. G. Johnson |title=The Chemistry of Copper, Silver and Gold |date=1973 |publisher=Elsevier Science |isbn=9780080188607 |language=en |page=42}}</ref> Copper(II) chloride reacts with several metals to produce copper metal or copper(I) chloride (CuCl) with oxidation of the other metal. To convert copper(II) chloride to copper(I) chloride, it can be convenient to reduce an aqueous solution with ] as the ]:<ref name="Ullmann" /> |
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:{{chem2|2 CuCl2 + SO2 + 2 H2O → 2 CuCl + 2 HCl + H2SO4}} |
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===Coordination complexes=== |
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{{chem2|CuCl2}} reacts with HCl or other ] sources to form complex ions: the red {{chem2|−}} (found in ] {{chem2|K}}) (it is a ] in reality, {{chem2|(2−)}}, a couple of tetrahedrons that share an edge), and the green or yellow {{chem2|(2−)}} (found in ] {{chem2|K2}}).<ref name="greenwood" /><ref name="tetra">{{cite book|author=Naida S. Gill |author2=F. B. Taylor |series=Inorganic Syntheses |year=1967 |volume=9 |pages=136–142 |doi=10.1002/9780470132401.ch37 |title=Tetrahalo Complexes of Dipositive Metals in the First Transition Series |isbn=978-0-470-13240-1}}</ref><ref name="handbook" /> |
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:{{chem2|CuCl2 + Cl- ⇌ -}} |
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:{{chem2|CuCl2 + 2 Cl- ⇌ (2-)}} |
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Some of these complexes can be crystallized from aqueous solution, and they adopt a wide variety of structures.<ref name="tetra" /> |
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Copper(II) chloride also forms a variety of ] with ]s such as ], ] and ]:<ref name="Ullmann" /><ref name="greenwood" /><ref>{{cite journal |author1=W. Libus |author2=S. K. Hoffmann |author3=M. Kluczkowski |author4=H. Twardowska |title=Solution equilibriums of copper(II) chloride in pyridine and pyridine-diluent mixtures |journal=Inorganic Chemistry |date=1980 |volume=19 |issue=6 |pages=1625–1632 |doi=10.1021/ic50208a039 |language=en}}</ref> |
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:{{chem2|CuCl2 + 2 C5H5N → }} (tetragonal) |
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:{{chem2|CuCl2 + 2 (C6H5)3P\dO → }} (tetrahedral) |
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However "soft" ligands such as ]s (e.g., ]), iodide, and ] as well as some tertiary ]s induce ] to give copper(I) complexes.<ref name="greenwood" /> |
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==Preparation== |
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Copper(II) chloride is prepared commercially by the action of ] of copper. Copper at red heat (300-400°C) combines directly with chlorine gas, giving (molten) copper(II) chloride. The reaction is very ].<ref name="Ullmann" /><ref name="handbook">{{cite book |author1=H. Wayne Richardson |title=Handbook of Copper Compounds and Applications |date=1997 |publisher=CRC Press |isbn=9781482277463 |language=en |pages=24–68}}</ref> |
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:{{chem2|Cu(s) + Cl2(g) → CuCl2(l)}} |
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A solution of copper(II) chloride is commercially produced by adding chlorine gas to a circulating mixture of ] and copper. From this solution, the dihydrate can be produced by evaporation.<ref name="Ullmann" /><ref name="Kirk" /> |
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Although copper metal itself cannot be oxidized by hydrochloric acid, copper-containing bases such as the hydroxide, ], or ] can react to form {{chem2|CuCl2}} in an ] which can subsequently be heated above {{convert|100|C}} to produce the anhydrous derivative.<ref name="Ullmann" /><ref name="Kirk" /> |
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Once prepared, a solution of {{chem2|CuCl2}} may be purified by ]. A standard method takes the solution mixed in hot dilute hydrochloric acid, and causes the crystals to form by cooling in a ] ({{chem2|CaCl2}}) ice bath.<ref name = bertz>S. H. Bertz, E. H. Fairchild, in ''Handbook of Reagents for Organic Synthesis, Volume 1: Reagents, Auxiliaries and Catalysts for C-C Bond Formation'', (R. M. Coates, S. E. Denmark, eds.), pp. 220–223, Wiley, New York, 1738.</ref><ref>{{cite book|title = Purification of Laboratory Chemicals|author1=W. L. F. Armarego |author2=Christina Li Lin Chai |pages = 461|url = https://books.google.com/books?id=PTXyS7Yj6zUC&pg=PA461|format = ] excerpt|edition = 6th|isbn = 978-1-85617-567-8|publisher = Butterworth-Heinemann|date = 2009-05-22}}</ref> |
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There are indirect and rarely used means of using copper ions in solution to form copper(II) chloride. ] of aqueous sodium chloride with copper ] produces (among other things) a blue-green ] that can be collected and converted to the hydrate. While this is not usually done due to the emission of toxic chlorine gas, and the prevalence of the more general ], the electrolysis will convert the copper metal to copper ions in solution forming the compound. Indeed, any solution of copper ions can be mixed with hydrochloric acid and made into a copper chloride by removing any other ions.<ref>{{cite journal |author1=J. Ji |author2=W. C. Cooper |title=Electrochemical preparation of cuprous oxide powder: Part I. Basic electrochemistry |journal=Journal of Applied Electrochemistry |date=1990 |volume=20 |issue=5 |pages=818–825 |doi=10.1007/BF01094312 |s2cid=95677720 |language=en}}</ref> |
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==Uses== |
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=== Co-catalyst in Wacker process === |
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A major industrial application for copper(II) chloride is as a co-catalyst with ] in the ]. In this process, ] (ethylene) is converted to ] (acetaldehyde) using water and air. During the reaction, ] ] to ], and the {{chem2|CuCl2}} serves to re-oxidize this back to {{chem2|PdCl2}}. Air can then oxidize the resultant ] back to {{chem2|CuCl2}}, completing the cycle.<ref name="org">{{cite journal |author1=Nicholas D. P. Cosford |author2=Pauline Pei Li |author3=Thierry Ollevier |title=Copper(II) Chloride |journal=Encyclopedia of Reagents for Organic Synthesis |date=2015 |pages=1–8 |doi=10.1002/047084289X.rc214.pub3 |isbn=9780470842898 |language=en}}</ref> |
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# {{chem2|C2H4 + PdCl2 + H2O → CH3CHO + Pd + 2 HCl}} |
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# {{chem2|Pd + 2 CuCl2 → 2 CuCl + PdCl2}} |
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# {{chem2|4 CuCl + 4 HCl + O2 → 4 CuCl2 + 2 H2O}} |
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The overall process is:<ref name="org" /> |
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:{{chem2|2 C2H4 + O2 → 2 CH3CHO}} |
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=== In organic synthesis === |
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Copper(II) chloride has some highly specialized applications in the ].<ref name="bertz" /> It affects the ] of ]—this is often performed in the presence of ]. It is able to chlorinate the ] of ] compounds:<ref name="org" /><ref>{{cite journal |author1=C. E. Castro |author2=E. J. Gaughan |author3=D. C. Owsley |year=1965 |title=Cupric Halide Halogenations |journal=] |volume=30 |issue=2 |pages=587 |doi=10.1021/jo01013a069}}</ref> |
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:] |
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This reaction is performed in a polar solvent such as ], often in the presence of ], which accelerates the reaction.<ref name="org" /> |
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{{chem2|CuCl2}}, in the presence of ], can also oxidize ]. The major product can be directed to give either a ] or a coupled product from oxidative dimerization. The latter process provides a high-yield route to ]:<ref>{{cite journal |author1=J. Brussee |author2=J. L. G. Groenendijk |author3=J. M. Koppele |author4=A. C. A. Jansen |year=1985 |title=On the mechanism of the formation of s(−)-(1, 1'-binaphthalene)-2,2'-diol via copper(II)amine complexes |journal=] |volume=41 |issue=16 |pages=3313 |doi=10.1016/S0040-4020(01)96682-7}}</ref><!--this methodology is obsolete and the citations are too specialized for wikipedia--> |
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:] |
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Such compounds are intermediates in the synthesis of ] and its derivatives.<ref name="org" /> |
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Copper(II) chloride dihydrate promotes the hydrolysis of ], i.e., for deprotection to regenerate diols<ref name="Chandrasekhar2003">{{cite journal |last=Chandrasekhar |first=M. |author2=Kusum L. Chandra |author3=Vinod K. Singh |year=2003 |title=Total Synthesis of (+)-Boronolide, (+)-Deacetylboronolide, and (+)-Dideacetylboronolide |journal=] |volume=68 |issue=10 |pages=4039–4045 |doi=10.1021/jo0269058 |pmid=12737588}}</ref> or ], as in this example (where TBDPS = ]):<ref name="Krishna2007">{{cite journal |last=Krishna |first=Palakodety Radha |author2=G. Dayaker |year=2007 |title=A stereoselective total synthesis of (−)-andrachcinidine via an olefin cross-metathesis protocol |journal=] |publisher=Elsevier |volume=48 |issue=41 |pages=7279–7282 |doi=10.1016/j.tetlet.2007.08.053}}</ref> |
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:] |
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{{chem2|CuCl2}} also catalyses the ] addition of ]s to ]s; the alpha-chlorosulfone may then undergo ] with a base to give a vinyl ] product.<ref name="org" /> |
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=== Catalyst in production of chlorine === |
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Copper(II) chloride is used as a ] in a variety of processes that produce chlorine by ]. The ] takes place at about 400 to 450 °C in the presence of a copper chloride:<ref name="Ullmann" /> |
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:{{chem2|4 HCl + O2 → 2 Cl2 + 2 H2O}} |
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Copper(II) chloride catalyzes the chlorination in the production of ] and ].<ref name="Ullmann" /> |
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Copper(II) chloride is used in the ] where it reacts with steam into copper(II) oxide dichloride and hydrogen chloride and is later recovered in the cycle from the ] of copper(I) chloride.<ref name="cucl" /> |
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===Niche uses=== |
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Copper(II) chloride is used in ] as a blue/green coloring agent. In a ], copper chlorides, like all copper compounds, emit green-blue light.<ref>{{cite web | title = Flame Tests | url = http://www.chemguide.co.uk/inorganic/group1/flametests.html | first = Jim | last = Clark | date = August 2018 | website = chemguide.co.uk | archive-url = https://web.archive.org/web/20201127013520/http://www.chemguide.co.uk/inorganic/group1/flametests.html | url-status = live | archive-date = November 27, 2020 | access-date = January 10, 2021}}</ref> |
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In ]s (HICs), cobalt-free brown to azure (copper(II) chloride base) HICs can be found on the market.<ref>{{cite patent| number =US 20150300958 A1| title =Adjustable colorimetric moisture indicators | pubdate=2015| inventor =Evan Koon Lun Yuuji Hajime| url =https://www.google.com/patents/US20150300958?cl=en}}</ref> In 1998, the ] classified items containing cobalt(II) chloride of 0.01 to 1% ] as T (Toxic), with the corresponding ] of R49 (may cause cancer if inhaled). Consequently, new cobalt-free humidity indicator cards containing copper have been developed.<ref>{{cite web |title=Cobalt dichloride |url=https://echa.europa.eu/substance-information/-/substanceinfo/100.028.718 |website=European Chemicals Agency |publisher=ECHA |access-date=30 May 2023}}</ref> |
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Copper(II) chloride is used as a ] in the textile industry, ] ], ], and ].<ref name="Ullmann" /><ref>{{cite book |author1=B.H. Patel |editor1-last=Clark |editor1-first=M. |title=Handbook of Textile and Industrial Dyeing |date=2011 |publisher=Woodhead Publishing |isbn=9781845696955 |pages=412–413 |url=https://www.sciencedirect.com/book/9781845696955/handbook-of-textile-and-industrial-dyeing |access-date=2 June 2023 |language=en |chapter=11 - Natural dyes}}</ref> |
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==Natural occurrence== |
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] |
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Copper(II) chloride occurs naturally as the very rare anhydrous mineral tolbachite and the dihydrate eriochalcite.<ref name="xray18">Marlene C. Morris, Howard F. McMurdie, Eloise H. Evans, Boris Paretzkin, Harry S. Parker, and Nicolas C. Panagiotopoulos (1981) ''Copper chloride hydrate (eriochalcite)'', in '' National Bureau of Standards, Monograph 25, Section 18; page 33.</ref> Both are found near ]s and in some copper mines.<ref>{{cite web |title=Tolbachite |url=https://www.mindat.org/min-3990.html |website=mindat.org |access-date=24 August 2023 |language=en}}</ref><ref>{{cite web |title=Eriochalcite |url=https://www.mindat.org/min-1398.html |website=mindat.org |access-date=24 August 2023}}</ref><ref>{{cite web |title=The New IMA List of Minerals |url=http://cnmnc.units.it/imalist.htm |website=Università degli studi di Trieste |publisher=International Mineralogical Association |access-date=24 August 2023 |language=en}}</ref> Mixed oxyhydroxide-chlorides like ] ({{chem2|Cu2(OH)3Cl}}) are more common, arising among Cu ore beds oxidation zones in arid climates.<ref>{{cite web |title=Atacamite |url=https://www.mindat.org/min-406.html |website=mindat.org |access-date=30 May 2023}}</ref> |
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==Safety and biological impact== |
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Copper(II) chloride can be toxic. Only concentrations below 1.3 ] of aqueous copper ions are allowed in drinking water by the ].<ref>{{cite web |title=National Primary Drinking Water Regulations |url=https://www.epa.gov/ground-water-and-drinking-water/national-primary-drinking-water-regulations#Inorganic |website=EPA |date=30 November 2015 |access-date=29 May 2023}}</ref> If copper chloride is absorbed, it results in headache, diarrhea, a drop in ], and fever. Ingestion of large amounts may induce ], ], and ].<ref name="CopperHealth">{{cite web |title=Copper: Health Information Summary |work=Environmental Fact Sheet |publisher=New Hampshire Department of Environmental Services |id=ARD-EHP-9 |year=2005 |url=http://des.nh.gov/organization/commissioner/pip/factsheets/ard/documents/ard-ehp-9.pdf |archiveurl=https://web.archive.org/web/20170120014307/http://www.des.nh.gov/organization/commissioner/pip/factsheets/ard/documents/ard-ehp-9.pdf |archivedate=20 January 2017}}</ref><ref>{{cite web |title=Safety Data Sheet |url=https://www.sigmaaldrich.com/US/en/sds/aldrich/203149 |website=Sigma Aldrich |access-date=30 June 2023}}</ref> |
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Copper(II) chloride has been demonstrated to cause ] and ] cycle disturbances within ] (onion) cells.<ref>{{cite journal | last1=Macar | first1=Tuğçe Kalefetoğlu | title=Resveratrol ameliorates the physiological, biochemical, cytogenetic, and anatomical toxicities induced by copper (II) chloride exposure in Allium cepa L. | url=https://link.springer.com/article/10.1007/s11356-019-06920-2 | journal=Environmental Science and Pollution Research | year=2020 | volume=27 | issue=1 | pages=657–667 | doi=10.1007/s11356-019-06920-2 | pmid=31808086 | s2cid=208649491}}</ref> Such cellular disturbances lead to ]. Copper(II) chloride has also been studied as a harmful environmental pollutant. Often present in irrigation-grade water, it can negatively affect water and soil microbes.<ref>{{cite journal | last1=Shiyab | first1=Safwan | title=Phytoaccumulation of copper from irrigation water and its effect on the internal structure of lettuce. | journal=Agriculture | year=2018 | volume=8 | issue=2 | pages=29 | doi=10.3390/agriculture8020029 | doi-access=free}}</ref> Specifically, ] were found to be very sensitive to the presence of copper(II) chloride. At a concentration of 0.95 mg/L, copper(II) chloride was found to cause a 50% inhibition (IC50) of the metabolic activity of denitrifying microbes.<ref>{{cite journal | last1=Ochoa-Herrera | first1=Valeria | title=Toxicity of copper (II) ions to microorganisms in biological wastewater treatment systems. | url=https://www.sciencedirect.com/science/article/pii/S0048969711011065 | journal=Science of the Total Environment | year=2011 | volume=412 | issue=1 | pages=380–385 | doi=10.1016/j.scitotenv.2011.09.072 | pmid=22030247 | bibcode=2011ScTEn.412..380O}}</ref> |
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==See also== |
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* ] |
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==References== |
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{{Reflist}} |
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==Further reading== |
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* {{Greenwood&Earnshaw|ref=none}} |
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* {{cite book |author=Lide, David R. |title=CRC handbook of chemistry and physics: a ready-reference book of chemical and physical data |url=https://archive.org/details/handbookofchemis00crcp |url-access=registration |publisher=CRC Press |location=Boca Raton |year=1990 |isbn=0-8493-0471-7|ref=none}} |
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* ''The Merck Index'', 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960. |
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* D. Nicholls, ''Complexes and First-Row Transition Elements'', Macmillan Press, London, 1973. |
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* A. F. Wells, '''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984. |
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* J. March, ''Advanced Organic Chemistry'', 4th ed., p. 723, Wiley, New York, 1992. |
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* ''Fieser & Fieser Reagents for Organic Synthesis'' Volume 5, p158, Wiley, New York, 1975. |
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* {{cite journal |
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| title = Chlorocuprates(II) |
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| author = D. W. Smith |
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| journal = Coordination Chemistry Reviews |
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| year = 1976 |
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| volume = 21 |
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| issue = 2–3 |
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| pages = 93–158 |
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| doi = 10.1016/S0010-8545(00)80445-2 |
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|ref=none}} |
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==External links== |
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{{Commons category|Copper(II) chloride}} |
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* at '']'' (University of Nottingham) |
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* |
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* |
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{{Copper compounds}} |
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{{Chlorides}} |
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] |
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] |
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] |
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] |
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] |
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] |