Perrhenic acid
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| Names | |
|---|---|
| IUPAC name
Perrhenic(VII) acid
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| Other names
Hydrated rhenium(VII) oxide
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.033.968 |
| RTECS number |
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CompTox Dashboard (EPA)
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| Properties | |
| H 4O 9Re 2 (solid) HReO 4 (gas) | |
| Molar mass | 251.2055 g/mol |
| Appearance | Pale yellow solid |
| Melting point | °C (? K) |
| Boiling point | sublimes |
| Soluble | |
| Acidity (pKa) | -1.25[1] |
| Structure | |
| octahedral-tetrahedral (solid) tetrahedral (gas) | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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Corrosive |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Related compounds | |
Related compounds
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Re 2O 7, Mn 2O 7 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Perrhenic acid is the chemical compound with the formula Re
2O
7(OH
2)
2. It is obtained by evaporating aqueous solutions of Re
2O
7. Conventionally, perrhenic acid is considered to have the formula HReO
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 Re
2O
7 is kept for a period of months, it breaks down and crystals of HReO
4·H
2O are formed, which contain tetrahedral ReO−
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.
Properties
The structure of solid perrhenic acid is [O
3Re-O-ReO
3(H
2O)
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:
- M(O)(H
2O) → M(OH)
2
Gaseous perrhenic acid is tetrahedral, as suggested by its formula {{H}}: No such template.
Reactions
Perrhenic acid or the related anhydrous oxide Re
2O
7 converts to dirhenium heptasulfide upon treatment with hydrogen sulfide:
- Re
2O
7 + 7 H
2S → Re
2S
7 + 7 H
2O
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. Re
2S
7 also catalyses the reduction of nitric oxide to N
2O.
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 ReOCl
3L
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] This catalyst is used in the dehydrogenation of alcohols and also promotes the decomposition of ammonia.
Catalysis
Perrhenic 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]
Other uses
Perrhenic acid is also used in the manufacture of x-ray targets.[10][11]
See also
References
- ^ http://www.iupac.org/publications/pac/1998/pdf/7002x0355.pdf
- ^ Glemser, O.; Müller, A.; Schwarzkopf, H. (1964). "Gasförmige Hydroxide. IX. Über ein Gasförmiges Hydroxid des Rheniums". Zeitschrift für anorganische und allgemeine Chemie (in German). 334: 21–26. doi:10.1002/zaac.19643340105.
{{cite journal}}: CS1 maint: multiple names: authors list (link). - ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Beyer, H.; Glemser, O.; Krebs, B. “Dirhenium Dihydratoheptoxide Re
2O
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. - ^ Schwarz, D. E.; Frenkel, A. I.; Nuzzo, R. G.; Rauchfuss, T. B.; Vairavamurthy, A. (2004). "Electrosynthesis of ReS
4. XAS Analysis of ReS
2, Re
2S
7, and ReS
4". Chemistry of Materials. 16: 151–158. doi:10.1021/cm034467v.{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ Parshall, G. W.; Shive, L. W.; Cotton, F. A. (1997). "Phosphine Complexes of Rhenium". Inorganic Syntheses. 17: 110–112. doi:10.1002/9780470132487.ch31.
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ van Vliet, M. C. A.; Arends, I. W. C. E.; Sheldon, R. A. (1999). "Rhenium Catalysed Epoxidations with Hydrogen Peroxide: Tertiary Arsines as Effective Cocatalysts". J. Chem. Soc., Perkin Trans. 1 (3): 377–80. doi:10.1039/a907975k.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ Ishihara, K.; Furuya, Y.; Yamamoto, H. (2002). "Rhenium(VII) Oxo Complexes as Extremely Active Catalysts in the Dehydration of Primary Amides and Aldoximes to Nitriles". Angewandte Chemie International Edition. 41 (16): 2983–2986. doi:10.1002/1521-3773(20020816)41:16<2983::AID-ANIE2983>3.0.CO;2-X.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ http://www.gehealthcare.com/usen/service/time_material_support/docs/Radplus2100.pdf
- ^ X-ray#Sources