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Rhenium trichloride

Rhenium Trichloride
Systematic name Rhenium(III) chloride
Other names Rhenium trichloride
Molecular formula ReCl3
Molar mass 292.57 g/mol
Appearance red, crystalline, nonvolatile solid
CAS number [13569-63-6]
Density and phase 4800 kg/m³
Solubility in water hydrolyzes to form Re2O3.xH2O.
In acetone
In methanol
In acetic acid
Melting point N/A
Boiling point 500 °C (decomposes)
Molecular shape (trimeric solid and in solution)
(dimeric in acetic acid)
Crystal structure Double Layered Rhombohedral
Dipole moment  ? D
MSDS External MSDS
Main hazards Corrosive (C)
NFPA 704
Flash point N/A
R/S statement R: R20 R21 R22 R23 R36 R37 R38
S: S3 S7 S8 S22 S24 S25 S26 S27 S28 S30 S41 S63
RTECS number  ?
Supplementary data
Structure and
n, εr, etc.
Phase behaviour
Solid, liquid, gas
Spectral data UV, IR, NMR, MS
Related compounds
Other anions Rhenium tribromide
Rhenium triiodide
Other cations Rhenium pentachloride
Technetium trichloride
Related compounds
Except where noted otherwise, data are given for
materials in their standard state (at 25 °C, 100 kPa)
Infobox disclaimer and references

Rhenium trichloride (ReCl3) is a compound of rhenium and chlorine.



Rhenium trichloride was first discovered in 1932 by Geilnann, Wriuce, and Biltz. [2]

Structure and physical properties

The crystal structure of rhenium trichloride consists of well-defined Re3Cl9 units that are connected by chlorine atom bridges. The Re3Cl9 unit structure also applies to rhenium trichloride dissolved in a variety of solvents, with the only possible exception being the dimer structure when dissolved in acetic acid. The Re3Cl9 crystal structure has C3v symmetry.[1]

Rhenium trichloride is comparatively non-volatile but produces a green vapour during strong heating. It may have a very small temperature-independent paramagnetism, but the susceptibility is ambiguous. [3]

Chemical properties

Rhenium trichloride prepared from rhenium pentachloride without further treatment is chemically reactive, but if it is vacuum sublimed at 500 oC, then it becomes comparatively unreactive. However, x-ray diffraction tests show no observable difference in structure between the untreated and vacuum sublimed material.[3]

The heat of oxidation according to the equation,
ReCl3(s) + 4OH- + 2OCl- --> ReO4- + 2H2O + 5Cl-
is 190.7 ± 0.2 kcal/mol.[3]


Rhenium trichloride is most efficiently prepared by the thermal decomposition of rhenium pentachloride in nitrogen. Other methods include reacting sulphuryl chloride with rhenium powder with or without the addition of aluminum chloride, the thermal decomposition of salts of hexachlororhenic(IV) acid,[3] or the heating of Re2(O2CCH3)4Cl2 under HCl gas.[4]


Rhenium trichloride is used as a starting material for synthesis of rhenium complexes. ReCl3 can react with peralkylated benzene-metal complexes that act as electron reservoirs.[5]


  1. ^ a b Cotton, F. A.; Mague J. T. Inorg. Chem. 1964, 233
  2. ^ Geilnann, W.; Wriuce, F. W.; Biltz. W.: Nachr. Ges. Wiss. Gottingen 1932, 579.
  3. ^ a b c d Colton, R. Chemistry of rhenium and technetium. London: Interscience Publishers. 1965.
  4. ^ Lincoln R.; Wilkinson, G.: Inorg. Synth. 1980, 20, 44
  5. ^ Hamon, J-R, Astruc, D., Organomet., 1989, 8(9), 2243-2247.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Rhenium_trichloride". A list of authors is available in Wikipedia.
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