| Names | |
|---|---|
| IUPAC name Rhenium(III) chloride | |
| Other names Rhenium trichloride | |
| Identifiers | |
3D model (JSmol) |
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| ChemSpider | |
| ECHA InfoCard | 100.033.610 |
| EC Number |
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| |
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| Properties | |
| ReCl3 | |
| Molar mass | 292.57 g/mol |
| Appearance | red, crystalline, nonvolatile solid |
| Density | 4800 kg/m3 |
| Melting point | N/A |
| Boiling point | 500 °C (932 °F; 773 K) (decomposes) |
| hydrolyzes to form Re2O3.xH2O. | |
| Structure | |
| Rhombohedral,hR72 | |
| R-3m, No. 166 | |
| (trimeric solid and in solution) (dimeric in acetic acid) | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | Corrosive (C) |
| Safety data sheet (SDS) | External MSDS |
| Related compounds | |
Otheranions | Rhenium tribromide Rhenium triiodide |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Trirhenium nonachloride is acompound with the formula ReCl3, sometimes also written Re3Cl9. It is a dark red hygroscopic solid that is insoluble in ordinary solvents. The compound is important in the history ofinorganic chemistry as an early example of a cluster compound with metal-metal bonds.[1] It is used as a starting material for synthesis of other rhenium complexes.
As shown byX-ray crystallography trirhenium nonachloride consists of Re3Cl12 subunits that share three chloridebridges with adjacent clusters. The interconnected network of clusters forms sheets. Around each Re center are seven ligands, four bridging chlorides, one terminal chloride, and two Re-Re bonds.[2]
Thehydrate is molecular with the formula Re3Cl9(H2O)3.[3]
Theheat of oxidation is evaluated according to the equation:
The enthalpy for this process is 190.7 ± 0.2 kcal/mol.[2]
The compound was discovered in 1932.[4] Trirhenium nonachloride is efficiently prepared by thermal decomposition ofrhenium pentachloride or hexachlororhenic(IV) acid:[5]
If the sample is vacuumsublimed at 500 °C, the resulting material is comparatively unreactive. The partially hydrated material such asRe3Cl9(H2O)4[6] can be more useful synthetically. Other synthetic methods include treatingrhenium withsulfuryl chloride. This process is sometimes conducted with the addition ofaluminium chloride.[2] It is also obtained by heating Re2(O2CCH3)4Cl2 under HCl:
Reaction of the tri- and pentachlorides givesrhenium tetrachloride:
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