Rhenium pentachloride
From Wikipedia, the free encyclopedia
| Rhenium pentachloride | |
|---|---|
| IUPAC name | Rhenium pentachloride |
| Other names | Rhenium(V) chloride, Rhenium chloride, pentachlororhenium |
| Identifiers | |
| CAS number | [13596-35-5] |
| Properties | |
| Molecular formula | ReCl5 |
| Molar mass | 363.471 g/mol |
| Appearance | red-brown |
| Density | 4.9 g/cm3, solid |
| Melting point |
220 °C |
| Boiling point |
N/A |
| Solubility in water | Will react to decompose and release HCl (g) |
| Structure | |
| Crystal structure | double hexagonally closed packed |
| Molecular shape | Octahedral |
| Hazards | |
| MSDS | MSDS |
| Main hazards | Highly Air Sensitive, will decompose to form HCl(g) |
| NFPA 704 |
 1
0
|
| R/S statement | R: 36, 37, 38 |
| Related compounds | |
| Other anions | Rhenium hexathiocyanate, Rhenium tetraiodate, Rhenium hexafluoride |
| Related compounds | Rhenium trichloride, Rhenium tetrachloride, Rhenium hexachloride |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
|
Rhenium pentachloride is a compound of rhenium and chlorine. It is a red-brown solid that is very air sensitive and reacts with water to give hydrogen chloride. This compound was first discovered by Geilmann, Wrigge, and Biltz in 1933.[1]
Contents |
[edit] Structure and physical properties
Rhenium pentachloride was found to exist as a solid in the form of Re2Cl10, which has a bridged structure with octahedrally coordinated rhenium atoms and can be formulated Cl4Re(μ-Cl)2ReCl4.[2] It has a melting point of 220 °C and is a paramagnetic molecule.[3] There has been no report of a boiling point for this compound. Rhenium pentachloride is a double hexagonally closed packed structure.[2]
[edit] Preparation
The preparation of this can be found by the chlorination of rhenium at 500 °C.[1] The purification of this material is done through multiple sublimations. The reaction leads to only one side product ReCl3. Synthesis of ReCl4 and ReCl6 must be done by other means.
[edit] Uses
Due to its reactivity ReCl5 is not biologically active. However it can be used to make compounds such as Cp2ReH, which similar to nickelocene can act as a catalyst to react with olefins.[2] An example of this catalytic activity is in the formation of polymers using ReCl5.[4]
This compound is highly reactive and as mentioned previously can react to form lower oxidation states such as rhenium trichloride, which has catalytic activity for a wide variety of applications. An example is the following reaction:[5]
- ReCl5 + 3 Cl2O → ReO3Cl + 5 Cl2
[edit] Reactions
Rhenium pentachloride is very air sensitive. Leaving it out overnight in atmosphere will lead to a brown liquid.[6]
It can react to form lower oxidation state chlorides such as rhenium trichloride.
- ReCl5 → ReCl3
It can also react with neutral and anionic donors to form complexed species.
- ReCl5 + 6CNS- → [Re(CNS)6]-
It is also reactive enough to react with solvents such as ammonia:
- ReCl5 + NH3 (excess) → ReCl3(NH2)2
[edit] References
- ^ a b Geilmann, Wilhelm; Wrigge, Friedrich W.; Biltz, Wilhelm. (1933). "Rheniumpentachlorid" (in German). Z. anorg. allgem. Chem. 214: 244. doi:.
- ^ a b c Mucker, K. F. (1968). "The crystal structure of ReCl5". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 24: 874. doi:.
- ^ CRC Handbook Online Edition
- ^ 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
- ^ Housecroft, C.E., Sharpe, A.G., Inorganic Chemistry, 2nd ed., Pearson Education Limited: Essex, England
- ^ Edwards, D. A. (1970). "Some reactions of rhenium(V) chloride". Journal of the Chemical Society A Inorganic Physical Theoretical: 1617. doi:.
