| 词条 | Perrhenic acid |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 476992919 | ImageFile = ChemicalStructureOfPerrhenicAcid.png | ImageSize = 150px | ImageName = Perrhenic acid | ImageFile1 = Perrhenic-acid-3D-balls.png | ImageSize1 = 150px | ImageName1 = Ball-and-stick model of the perrhenic acid molecule | IUPACName = Tetraoxorhenic(VII) acid | OtherNames = Hydrated rhenium(VII) oxide |Section1={{Chembox Identifiers | InChI = 1/2H2O.7O.2Re/h2*1H2;;;;;;;;;/rH4O9Re2/c1-10(2,3)9-11(4,5,6,7)8/h4-5H2 | InChIKey = JOTGKJVGIIKFIQ-SEUCOXMMAB | SMILES = [OH2][Re](=O)(=O)(=O)([OH2])O[Re](=O)(=O)=O | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/2H2O.7O.2Re/h2*1H2;;;;;;;;; | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = JOTGKJVGIIKFIQ-UHFFFAOYSA-N | CASNo_Ref = {{cascite|changed|??}} | CASNo = 13768-11-1 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID=21106462 | RTECS = TT4550000 |Section2={{Chembox Properties | Formula = {{chem|H|4|O|9|Re|2}} (solid) {{chem|H|Re|O|4}} (gas) | MolarMass = 251.2055 g/mol | Appearance = Pale yellow solid | Density = | Solubility = Soluble | MeltingPt = | BoilingPt = sublimes | ConjugateBase = Perrhenate | pKa = -1.25[1] |Section3={{Chembox Structure | Coordination = octahedral-tetrahedral (solid) tetrahedral (gas) |Section7={{Chembox Hazards | ExternalSDS = | MainHazards = Corrosive | NFPA-H = 3 | NFPA-F = | NFPA-R = | FlashPt = Non-flammable | RPhrases = {{R34}} | SPhrases = {{S26}}, {{S36/37}}, {{S39}}, {{S45}} |Section8={{Chembox Related | OtherCompounds = {{chem|link=Rhenium(VII) oxide| Re|2|O|7}}, {{chem|link = Manganese(VII) oxide|Mn|2|O|7}} }} Perrhenic acid is the chemical compound with the formula {{chem|Re|2|O|7|(O|H|2|)|2|}}. It is obtained by evaporating aqueous solutions of {{chem|Re|2|O|7}}. Conventionally, perrhenic acid is considered to have the formula {{chem|H|Re|O|4}}, and a species of this formula forms when rhenium(VII) oxide sublimes in the presence of water or steam.[2] When a solution of {{chem|Re|2|O|7}} is kept for a period of months, it breaks down and crystals of {{chem|H|Re|O|4|·H|2|O}} are formed, which contain tetrahedral {{chem|Re|O|4|-}}[3] For most purposes, perrhenic acid and rhenium(VII) oxide are used interchangeably. Rhenium can be dissolved in nitric or concentrated sulfuric acid to produce perrhenic acid. PropertiesThe structure of solid perrhenic acid is [{{chem|O|3|Re-O-Re|O|3|(H|2|O)|2|}}].[4] This species is a rare example of a metal oxide coordinated to water—most often metal-oxo-aquo species are unstable with respect to the corresponding hydroxides: {{chem|M|(O)|(H|2|O)}} → {{chem|M|(O|H)|2}} The two rhenium atoms have different bonding geometries, with one being tetrahedral and the other octahedral, and with the water ligands coordinated to the latter. Gaseous perrhenic acid is tetrahedral, as suggested by its formula {{chem|H|Re|O|4}}. ReactionsPerrhenic acid or the related anhydrous oxide {{chem|Re|2|O|7}} converts to dirhenium heptasulfide upon treatment with hydrogen sulfide: {{chem|Re|2|O|7}} + 7 {{chem|H|2|S}} → {{chem|Re|2|S|7}} + 7 {{chem|H|2|O}} The heptasulfide, which has a complex structure,[5] catalyses the hydrogenation of double bonds and is useful because it tolerates sulfur compounds, which poison noble metal catalysts. {{chem|Re|2|S|7}} also catalyses the reduction of nitric oxide to {{chem|N|2|O}}. Perrhenic acid in the presence of HCl undergoes reduction in the presence of thioethers and tertiary phosphines to give Re(V) complexes with the formula {{chem|Re|O|Cl|3|L|2|}}.[6] Perrhenic acid combined with platinum on a support gives rise to a useful hydrogenation and hydrocracking catalyst for the petroleum industry.[7] For example, silica impregnated with a solution of perrhenic acid is reduced with hydrogen at 500 °C.{{Citation needed|date=April 2011}} This catalyst is used in the dehydrogenation of alcohols and also promotes the decomposition of ammonia. CatalysisPerrhenic acid is a precursor to a variety of homogeneous catalysts, some of which are promising in niche applications that can justify the high cost of rhenium. In combination with tertiary arsines, perrhenic acid gives a catalyst for the epoxidation of alkenes with hydrogen peroxide.[8] Perrhenic acid catalyses the dehydration of oximes to nitriles.[9] {{clear|left}}Other usesPerrhenic acid is also used in the manufacture of x-ray targets.[10][11] See also
References1. ^http://www.iupac.org/publications/pac/1998/pdf/7002x0355.pdf {{Rhenium compounds}}2. ^{{cite journal |author1=Glemser, O. |author2=Müller, A. |author3=Schwarzkopf, H. | title = Gasförmige Hydroxide. IX. Über ein Gasförmiges Hydroxid des Rheniums | journal = Zeitschrift für anorganische und allgemeine Chemie | year = 1964 | volume = 334 | pages = 21–26| language = German | doi = 10.1002/zaac.19643340105}}. 3. ^{{Greenwood&Earnshaw}} 4. ^Beyer, H.; Glemser, O.; Krebs, B. “Dirhenium Dihydratoheptoxide {{chem|Re|2|O|7|(OH|2|)|2}} - New Type of Water Bonding in an Aquoxide” Angewandte Chemie, International Edition English 1968, Volume 7, Pages 295 - 296. {{doi|10.1002/anie.196802951}}. 5. ^{{cite journal |author1=Schwarz, D. E. |author2=Frenkel, A. I. |author3=Nuzzo, R. G. |author4=Rauchfuss, T. B. |author5=Vairavamurthy, A. | title = Electrosynthesis of {{chem|Re|S|4}}. XAS Analysis of {{chem|Re|S|2}}, {{chem|Re|2|S|7}}, and {{chem|Re|S|4}} | journal = Chemistry of Materials | year = 2004 | volume = 16 | pages = 151–158 | doi = 10.1021/cm034467v}} 6. ^{{cite journal | title = Phosphine Complexes of Rhenium | author = Parshall, G. W. |journal = Inorganic Syntheses | year = 1997 | volume = 17 | pages = 110–112| doi = 10.1002/9780470132487.ch31 | last2 = Shive | first2 = L. W. | last3 = Cotton | first3 = F. A.}} 7. ^Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}. 8. ^{{cite journal|author=van Vliet, M. C. A.; Arends, I. W. C. E.; Sheldon, R. A.|year=1999|title=Rhenium Catalysed Epoxidations with Hydrogen Peroxide: Tertiary Arsines as Effective Cocatalysts|journal=J. Chem. Soc., Perkin Trans. 1|pages=377–80 | doi = 10.1039/a907975k|issue=3 }} 9. ^{{cite journal |author1=Ishihara, K. |author2=Furuya, Y. |author3=Yamamoto, H. | title = Rhenium(VII) Oxo Complexes as Extremely Active Catalysts in the Dehydration of Primary Amides and Aldoximes to Nitriles | journal = Angewandte Chemie International Edition | volume = 41 | pages = 2983–2986 | year = 2002 | doi = 10.1002/1521-3773(20020816)41:16<2983::AID-ANIE2983>3.0.CO;2-X | issue = 16 }} 10. ^http://www.gehealthcare.com/usen/service/time_material_support/docs/Radplus2100.pdf{{dead link|date=March 2018 |bot=InternetArchiveBot |fix-attempted=yes }} 11. ^X-ray#Sources 3 : Mineral acids|Perrhenates|Transition metal oxoacids |
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