Rhenium pentachloride

Rhenium pentachloride
Names
IUPAC name
Rhenium pentachloride
Other names
Rhenium(V) chloride, Rhenium chloride, pentachlororhenium
Identifiers
13596-35-5 YesY
ChemSpider 75428
EC Number 237-042-6
Jmol 3D model Interactive image
PubChem 83602
Properties
ReCl5
Molar mass 363.471 g/mol
Appearance red-brown
Density 4.9 g/cm3, solid
Melting point 220 °C (428 °F; 493 K)
Boiling point N/A
Will react to decompose and release HCl (g)
Structure
Monoclinic, mP48; a = 0.924 nm, b = 1.154 nm, c = 1.203 nm, α = 90°, β = 109.1°, γ = 90° [1]
P21/c, No. 14
Octahedral
Hazards
Main hazards releases HCl upon hydrolysis
Safety data sheet MSDS
R/S statement R: 36, 37, 38
NFPA 704
Flammability (red): no hazard code Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
1
0
Related compounds
Other anions
Rhenium hexafluoride
Related compounds
Trirhenium nonachloride, rhenium tetrachloride, rhenium hexachloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Rhenium pentachloride is an inorganic compound of chlorine and rhenium. The compound has the formula Re2Cl10 but it is usually referred to as the pentachloride. It is a red-brown solid. It is the highest chloride of rhenium.

Structure and preparation

Rhenium pentachloride has a bioctahedral structure and can be formulated as Cl4Re(μ-Cl)2ReCl4. The Re-Re distance is 3.74 Å.[1] The motif is similar to that seen for tantalum pentachloride.

This compound was first prepared in 1933,[2] a few years after the discovery of rhenium. The preparation involves chlorination of rhenium at temperatures up to 900 °C.[3] The material can be purified by sublimation.

ReCl5 is one of the most oxidized binary chlorides of Re. With a d2 configuration, it could conceivably be further chlorinated, and indeed ReCl6 has been prepared, albeit indirectly from rhenium hexafluoride.[4] Rhenium heptafluoride is known but not the heptachloride.[5]

Uses and reactions

It degrades in air to a brown liquid.[6]

Although rhenium pentachloride has no commercial applications, it is of historic significance as one of the early catalysts for olefin metathesis.[7] Reduction gives Trirhenium nonachloride.

Oxygenation affords the Re(VII) oxychloride:[8]

ReCl5 + 3 Cl2O → ReO3Cl + 5 Cl2

References

  1. 1 2 Mucker, K. F.; Smith, G. S.; Johnson, Q. (1968). "The crystal structure of ReCl5". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 24 (6): 874. doi:10.1107/S0567740868003316.
  2. Geilmann, Wilhelm; Wrigge, Friedrich W.; Biltz, Wilhelm. (1933). "Rheniumpentachlorid". Z. anorg. allgem. Chem. (in German) 214 (3): 244. doi:10.1002/zaac.19332140304.
  3. Roger Lincoln, Geoffrey Wilkinson "Rhenium Pentachloride and Volatile Metal Chlorides by Direct Chlorination Using a Vertical-Tube Reactor" Inorganic Syntheses, 1980, Volume 20, Pages 41–43. doi:10.1002/9780470132517.ch11.
  4. Tamadon, Farhad; Seppelt, Konrad (2013). "The Elusive Halides VCl5, MoCl6, and ReCl6". Angew. Chem. Int. Ed. 52: 767–769. doi:10.1002/anie.201207552.
  5. Stuart A. Macgregor and Klaus H. Moock "Stabilization of High Oxidation States in Transition Metals. 2.1 WCl6 Oxidizes [WF6]-, but Would PtCl6 Oxidize [PtF6]-? An Electrochemical and Computational Study of 5d Transition Metal Halides: [MF6]z versus [MCl6]z (M = Ta to Pt; z = 0, 1−, 2−)" pp 3284–3292. doi:10.1021/ic9605736
  6. Edwards, D. A.; Ward, R. T. (1970). "Some reactions of rhenium(V) chloride". Journal of the Chemical Society a Inorganic Physical Theoretical: 1617. doi:10.1039/J19700001617.
  7. Ring-opening polymerization of endo and exo-dicyclopentadiene and their 7,8-dihydro derivatives, Hamilton, J.G.; Ivin, K.J.; Rooney, J.J. Journal of Molecular Catalysis 1986 , 36, 115.
  8. Housecroft, C. E.; Sharpe, A. G. (2004). Inorganic Chemistry (2nd ed.). Prentice Hall. ISBN 978-0130399137.

External links

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