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| verifiedrevid = 399730099 |
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| verifiedrevid = 416167690 |
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| Name = Copper (II) bromide |
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| ImageFile = Copper(II)_bromide.jpg |
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| Name = Copper (II) bromide |
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| ImageFile = CuBr2-1000x1000.jpg |
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<!-- | ImageSize = 200px --> |
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| ImageCaption = Anhydrous |
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| ImageName = Copper (II) bromide |
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| ImageFile1 = Bromid měďnatý.PNG |
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| OtherNames = Cupric bromide |
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| ImageCaption1 = Tetrahydrate |
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| Section1 = {{Chembox Identifiers |
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| OtherNames = Cupric bromide<br>Copper dibromide |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| Section1 = {{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 8395631 |
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| ChemSpiderID = 8395631 |
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| EC_number = 232-167-2 |
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| InChI = 1/2BrH.Cu/h2*1H;/q;;+2/p-2 |
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| InChI = 1/2BrH.Cu/h2*1H;/q;;+2/p-2 |
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| SMILES = .. |
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| SMILES = .. |
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| StdInChIKey = QTMDXZNDVAMKGV-UHFFFAOYSA-L |
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| StdInChIKey = QTMDXZNDVAMKGV-UHFFFAOYSA-L |
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| CASNo = 7789-45-9 |
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| CASNo = 7789-45-9 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| PubChem = 10220139 |
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| UNII = 1KC430K0ZN |
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| PubChem = 24611 |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = CuBr<sub>2</sub> |
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| Formula = CuBr<sub>2</sub> |
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| MolarMass = 223.37 g/mol |
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| MolarMass = 223.37 g/mol |
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| Appearance = grayish black crystals |
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| Appearance = grayish black crystals <br> ] |
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| Density = 4.71 g/cm<sup>3</sup>, solid |
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| Density = 4.710 g/cm<sup>3</sup>, solid |
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| Solubility = 55.7 g/100mL (20 °C) |
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| Solubility = 55.7 g/100 mL (20 °C) |
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| Solubleother = soluble in ], ], ]; insoluble in ] |
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| SolubleOther = Soluble in ], ], ], insoluble in ], ], ], ] |
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| MeltingPt = 498 °C (771 K) |
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| MeltingPtC = 498 |
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| BoilingPtC = 900 |
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| BoilingPt = 900 °C (1173 K) <ref>http://www.mallbaker.com/americas/msds/english/C5841_msds_us_Default.pdf</ref> |
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| MagSus = +685.5·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section7 = {{Chembox Hazards |
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| Section3 = {{Chembox Structure |
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| CrystalStruct = monoclinic |
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| EUIndex = Not listed |
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| NFPA-H = 2 |
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| NFPA-R = 0 |
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| NFPA-F = 0 |
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| Section8 = {{Chembox Related |
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| Section7 = {{Chembox Hazards |
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| NFPA-H = 2 |
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| OtherAnions = ]<br />] |
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| NFPA-R = 0 |
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| OtherCations = ]<br />]<br/>] |
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| NFPA-F = 0 |
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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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| OtherAnions = ]<br/>] |
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| OtherCations = ]<br/>]<br/>]<br/>]<br/>]}} |
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'''Copper(II) bromide''' (]]) is a ]. It is used in ] as an intensifier and as a ] agent in ].<ref>''A cycloaddition route to novel triazole boronic esters'' Jianhui Huang, Simon J. F. Macdonald and Joseph P. A. Harrity, ], '''2009''', 436–438, {{DOI: 10.1039/b817052e}}</ref> |
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'''Copper(II) bromide''' (]]) is a ] that forms an unstable tetrahydrate CuBr<sub>2</sub>·4H<sub>2</sub>O. It is used in ] as an ] and as a ] agent in ].<ref>{{cite journal |title=A cycloaddition route to novel triazole boronic esters |first1=Jianhui |last1=Huang |first2=Simon J. F. |last2=Macdonald |first3=Joseph P. A. |last3=Harrity |journal=] |year=2009 |pages=436–438 |doi=10.1039/b817052e |issue=4|pmid=19137177 }}</ref> |
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It is also used in the ], a class of laser where the medium is copper bromide vapour formed in situ from hydrogen bromide in reaction with the enclosing copper discharge tube.<ref> |
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It is also used in the ], a class of laser where the medium is copper bromide vapour formed in-situ from ] reacting with the copper discharge tube.<ref>{{cite journal |last1=Livingstone |first1=E. S. |last2=Maitland |first2=A. |title=A high power, segmented metal, copper bromide laser |journal=Measurement Science and Technology |year=1991 |volume=2 |number=11 |page=1119 |doi=10.1088/0957-0233/2/11/022 |bibcode=1991MeScT...2.1119L |s2cid=250801465 |issn=0957-0233}}</ref> Producing yellow or green light, it is used in ] applications. |
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==Synthesis== |
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Copper(II) bromide can be obtained by combining copper oxide and hydrobromic acid:<ref>{{cite book |title=Synthetic methods of Organometallic and Inorganic Chemistry |editor1-first=D. K. |editor1-last=Breitinger |editor2-first=W. A. |editor2-last=Herrmann |publisher=Thieme Medical Publishers |location=New York |year=1999 |isbn=0-86577-662-8}}</ref> |
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:CuO + 2HBr → CuBr<sub>2</sub> + H<sub>2</sub>O. |
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The tetrahydrate can be produced by recrystallization of solutions of copper(II) bromide at 0 °C. If heated above 18 °C, it releases water to produce the anhydrous form.<ref name="hydrate">{{cite journal |author1=Kenji Waizumi |author2=Hideki Masuda |author3=Hitoshi Ohtaki |title=X-ray structural studies of FeBr2·4H2O, CoBr2·4H2O, NiCl2·4H2O and CuBr2·4H2O. cis/trans selectivity in transition metal(II) dihalide tetrahydrate |journal=Inorganica Chimica Acta |date=1992 |volume=192 |issue=2 |pages=173–181 |doi=10.1016/S0020-1693(00)80756-2 |language=en}}</ref> |
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==Purification== |
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Copper(II) bromide is purified by crystallization twice from water, filtration to remove any CuBr and concentration under vacuum. This product is dehydrated using ].<ref><!--unclear ref, please clarify and convert to cite book or cite journal-->Hope et al. J Chem Soc 5226 1960, Glemser & Sauer in Handbook of Preparative Inorganic Chemistry (Ed.Brauer) Academic Press Vol II p 1009 1965.</ref> |
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==Molecular and crystal structure== |
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] |
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In the solid state CuBr<sub>2</sub> has a polymeric structure, with CuBr<sub>4</sub> planar units connected on opposite sides to form chains. The crystal structure is ], ] C2/m, with ] a = 714 ], b = 346 pm, c = 718 pm, e ß = 121° 15'.<ref>{{cite journal |last=Helmholz |first=Lindsay |title=The Crystal Structure of Anhydrous Cupric Bromide |journal=] |year=1947 |volume=69 |number=4 |pages=886–889 |doi=10.1021/ja01196a046}}</ref> CuBr<sub>2</sub> monomeric units are present in the gas phase at high temperature.<ref>{{cite encyclopedia |last=Conry |first=Rebecca R. |article=Copper: Inorganic & Coordination Chemistry |title=Encyclopedia of Inorganic Chemistry |edition=2nd |publisher=John Wiley & Sons |year=2006 |doi=10.1002/0470862106.ia052 |isbn=978-0-470-86210-0}}</ref> |
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The tetrahydrate, structurally formulated as ·2H<sub>2</sub>O, has a monoclinic crystal structure and consists of distorted square planar''trans''- centres as well as two molecules of ].<ref name="hydrate" /> |
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==Reactions== |
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Copper(II) bromide in chloroform-ethyl acetate reacts with ketones resulting in the formation of alpha-bromo ketones. The resulting product can be directly used for the preparation of derivatives. This heterogeneous method is reported to be the most selective and direct method of formation of α-bromo ketones.<ref>{{cite journal |last1=King |first1= L. Carroll |last2=Ostrum |first2=G. Kenneth |title=Selective Bromination with Copper(II) Bromide |journal=] |year=1964 |volume=29 |number=12 |pages=3459–3461 |doi=10.1021/jo01035a003}}</ref> |
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Dibromination of NPGs, n-pentenyl glycosides, using CuBr<sub>2</sub>/LiBr reagent combination was performed in order for an NPG to serve as a glycosyl acceptor during halonium-promoted couplings. |
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Such reaction gives high yield of the dibromides from alkenyl sugars that are resistant to a direct reaction with molecular bromine.<ref>{{cite journal |last1=Rodebaugh |first1=Robert |last2=Debenham |first2=John S. |last3=Fraser-Reid |first3=Burt J. |last4=Snyder |first4=James P. |journal=] |year=1999 |volume=64 |number=5 |pages=1758–1761 |title=Bromination of Alkenyl Glycosides with Copper(II) Bromide and Lithium Bromide: Synthesis, Mechanism, and DFT Calculations |doi= 10.1021/jo9718509|pmid=11674253 }}</ref> |
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==Usage== |
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Copper(II) bromide lasers produce pulsed yellow and green light and have been studied as a possible treatment for cutaneous lesions.<ref>{{cite journal |last1=McCoy |first1=S. |last2=Hanna |first2=M. |last3=Anderson |first3=P. |last4=McLennan |first4=G. |last5=Repacholi |first5=M. |journal=Dermatol. Surg. |date=June 1996 |volume=22 |number=6 |pages=551–7 |title=An evaluation of the copper-bromide laser for treating telangiectasia |doi=10.1111/j.1524-4725.1996.tb00373.x |pmid=8646471 |s2cid=22626280 |issn=1076-0512}}</ref> Experiments have also shown copper bromide treatment to be beneficial for skin rejuvenation.<ref>Davis P., Town G., Haywards H. ''A practical comparison of IPLs and the Copper Bromide Laser for photorejuvenation, acne and the treatment of vascular&pigmented lesions.''</ref> |
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It has been widely used in photography as its solution was used as the bleaching step for intensifying collodion and gelatin negatives.<ref>Diane Heppner ''The Focal Encyclopedia of Photography'', Inc. Elsevier '''2007'''4th edition</ref> |
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Copper(II)bromide has also been proposed as a possible material in humidity indicator cards.<ref>George McKedy US Patent Application Publication, Pub.No.: US2010/0252779 A1</ref> |
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==Safety== |
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==Safety== |
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Copper(II) bromide is harmful if swallowed. It affects the central nervous system, brain, eyes, liver, and kidneys. It causes irritation to skin, eyes, and respiratory tract. |
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Copper(II) bromide is harmful if swallowed. It affects the central nervous system, brain, eyes, liver, and kidneys. It causes irritation to skin, eyes, and respiratory tract. |
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==Natural occurrence== |
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Pure copper(II) bromide is as yet (2020) unknown among minerals. However, barlowite, Cu<sub>4</sub>BrF(OH)<sub>6</sub>, contains both copper and bromide.<ref>{{Cite web|url=https://www.mindat.org/min-40276.html|title = Verification}}</ref><ref>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> |
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==See also== |
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==See also== |
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*] (]]) |
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==References== |
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==References== |
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<references/> |
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<references/> |
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http://msds.chem.ox.ac.uk/CO/copper_II_bromide.html |
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{{Copper compounds}} |
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{{Copper compounds}} |
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{{Bromides}} |
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{{inorganic-compound-stub}} |
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