| Revision as of 12:44, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 474102625 of page Cobalt(II)_fluoride for the Chem/Drugbox validation project (updated: 'CASNo'). |
Latest revision as of 20:54, 3 January 2024 edit Keresluna (talk | contribs)Autopatrolled, Extended confirmed users4,071 edits →External links: replace template |
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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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| Verifiedfields = changed |
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| verifiedrevid = 441576054 |
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| verifiedrevid = 476995955 |
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| ImageFile = Fluorid kobaltnatý.PNG |
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| ImageFile = Fluorid kobaltnatý.PNG |
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| ImageSize = |
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| IUPACName = Cobalt(II) fluoride |
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| IUPACName = Cobalt(II) fluoride |
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| OtherNames = cobalt difluoride |
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| OtherNames = cobalt difluoride |
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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 = 23205 |
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| ChemSpiderID = 23205 |
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| InChI = 1/Co.2FH/h;2*1H/q+2;;/p-2 |
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| InChI = 1/Co.2FH/h;2*1H/q+2;;/p-2 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = YCYBZKSMUPTWEE-UHFFFAOYSA-L |
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| StdInChIKey = YCYBZKSMUPTWEE-UHFFFAOYSA-L |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo_Ref = {{cascite|changed|??}} |
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| CASNo = <!-- blanked - oldvalue: 10026-17-2 --> |
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| CASNo = 10026-17-2 |
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| UNII_Ref = {{fdacite|changed|FDA}} |
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| UNII =9KI67810UR |
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| PubChem = 24820 |
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| PubChem = 24820 |
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| RTECS = GG0770000 |
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| RTECS = GG0770000 |
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| EINECS = 233-061-9 |
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| EINECS = 233-061-9 |
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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 = ]] |
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| Formula = ]] |
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| MolarMass = 96.93 g/mol |
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| MolarMass = 96.93 g/mol |
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| Appearance = Red crystalline solid |
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| Appearance = Red crystalline solid |
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| Density = 4.46 g/cm<sup>3</sup> (anhydrous) <br> 2.22 g/cm<sup>3</sup> (tetrahydrate) |
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| Density = 4.46 g/cm<sup>3</sup> (anhydrous) <br> 2.22 g/cm<sup>3</sup> (tetrahydrate) |
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| MeltingPtC = 1217 |
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| MeltingPtC = 1217 |
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| BoilingPtC = 1400 |
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| BoilingPtC = 1400 |
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| Solubility = 1.4 g/100 mL (25 °C) |
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| Solubility = 1.4 g/100 mL (25 °C) |
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| SolubleOther = soluble in ] <br> insoluble in ], ], ] |
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| SolubleOther = soluble in ] <br> insoluble in ], ], ] |
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| MagSus = +9490.0·10<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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| CrystalStruct = tetragonal (a,hydrous) <br> orthorhombic (tetrahydrate) |
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| CrystalStruct = tetragonal (anhydrous) <br> orthorhombic (tetrahydrate) |
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| Section4 = {{Chembox Hazards |
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|Section4={{Chembox Hazards |
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| MainHazards = |
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| MainHazards = |
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| LD50 = oral (rat): 150 mg/kg |
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| LD50 = oral (rat): 150 mg/kg |
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| NFPA-H = 3 |
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| NFPA-H = 3 |
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| NFPA-F = 0 |
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| NFPA-F = 0 |
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| NFPA-R = 2 |
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| NFPA-R = 0 |
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| NFPA-O = |
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| NFPA-S = |
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| FlashPt = |
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| FlashPt = |
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| Autoignition = |
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| AutoignitionPt = |
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}} |
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}} |
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| Section5 = {{Chembox Related |
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|Section5={{Chembox Related |
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| OtherAnions = ], ] |
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| OtherAnions = ], ] |
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| OtherCations = ], ] |
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| OtherCations = ], ] |
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| OtherCpds = ] }} |
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| OtherCompounds = ] }} |
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}} |
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] |
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'''Cobalt(II) fluoride''' is a ] with the formula (CoF<sub>2</sub>). It is a pink crystalline solid compound<ref>{{citation|title=Handbook of Inorganic Chemicals |author= Pradyot Patnaik|year= 2002|publisher=McGraw-Hill Professional|url= https://books.google.com/books?id=Xqj-TTzkvTEC&q=%22Cobalt(II)+fluoride%22&pg=PA241|isbn=978-0-07-049439-8}}</ref><ref>{{citation |title=Article title Heat Exchange between Cobalt(II) Fluoride Powder and the Wall of Rotating Cylinder |author1=Pashkevich, D. S. |author2=Radchenko S. M. |author3=Mukhortov, D. A. |journal=Russian Journal of Applied Chemistry |publisher=Consultants Bureau |url=http://www.maik.rssi.ru/abstract/rjapchem/97/rjapchem1447_abstract.pdf |issn=1070-4272 |access-date=2007-03-07 |archive-url=https://web.archive.org/web/20040929065300/http://www.maik.rssi.ru/abstract/rjapchem/97/rjapchem1447_abstract.pdf |archive-date=2004-09-29 |url-status=dead }}</ref> which is ] at low temperatures (T<sub>N</sub>=37.7 K)<ref>Ashcroft/Mermin: Solid State Physics (Tab. 33.2)</ref> The formula is given for both the red tetragonal crystal, (CoF<sub>2</sub>), and the tetrahydrate red orthogonal crystal, (CoF<sub>2</sub>·4H<sub>2</sub>O). CoF<sub>2</sub> is used in oxygen-sensitive fields, namely metal production. In low concentrations, it has public health uses. |
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CoF<sub>2</sub> is sparingly soluble in water. The compound can be dissolved in warm ], and will decompose in boiling water. Yet the hydrate is water-soluble, especially the di-hydrate CoF<sub>2</sub>·2H<sub>2</sub>O and tri-hydrate CoF<sub>2</sub>·3H<sub>2</sub>O forms of the compound. The hydrate will also decompose with heat. |
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Like some other metal difluorides, CoF<sub>2</sub> crystallizes in the ] structure, which features octahedral Co centers and planar fluorides.<ref>{{cite journal |doi=10.1021/ja01650a005|title=The Crystal Structure of MnF<sub>2</sub>, FeF<sub>2</sub>, CoF<sub>2</sub>, NiF<sub>2</sub> and ZnF<sub>2</sub>|first1=J. W.|last1=Stout|first2=Stanley A.|last2=Reed|journal= J. Am. Chem. Soc.|year=1954|volume=76|issue=21|pages=5279–5281}}</ref> |
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==Preparation== |
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Cobalt(II) fluoride can be prepared from anhydrous cobalt(II) chloride or cobalt(II) oxide in a stream of ]: |
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:CoCl<sub>2</sub> + 2HF → CoF<sub>2</sub> + 2HCl |
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:CoO + 2HF → CoF<sub>2</sub> + H<sub>2</sub>O |
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It is produced in the reaction of cobalt (III) fluoride with water. |
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The ] cobalt(II) fluoride is formed by dissolving cobalt(II) in hydrofluoric acid. The anhydrous fluoride can be extracted from this by ]. Other synthesis can occur at higher temperatures. It has been shown that at 500 °C ] will combine with cobalt producing a mixture of CoF<sub>2</sub> and CoF<sub>3</sub>.<ref>{{citation|title= Comprehensive Inorganic Chemistry |author= J.C. Bailar |year= 1973|publisher=Pergoamon}}</ref> |
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==Uses== |
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Cobalt(II) fluoride can be used as a catalyst to alloy metals. It is also used for optical deposition, of which it tremendously improves optical quality. Cobalt(II) fluoride is available in most volumes in an ultra high purity composition. High purity compositions improve optical qualities and its usefulness as a standard. |
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==Analysis== |
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To analyze this compound, Cobalt (II) fluoride can be dissolved in nitric acid. The solution is then diluted with water until appropriate concentration for AA or ICP ] for the cobalt. A small amount of salt can be dissolved in cold water and analyzed for fluoride ion by a fluoride ion-selective electrode or ion ]. |
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==Chemical properties== |
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CoF<sub>2</sub> is a weak ]. Cobalt(II) complexes are usually octahedral or tetrahedral. As a 19-electron species it is a good reducing agent, fairly oxidizable into an 18-electron compound. Cobalt(II) fluoride can be reduced by hydrogen at a 300 °C. |
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==References== |
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<references/> |
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==External links== |
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{{Commons category|Cobalt(II) fluoride}} |
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{{Cobalt compounds}} |
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{{fluorides}} |
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] |
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] |
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