Thorium(IV) chloride
Identifiers | |
---|---|
3D model (
JSmol ) |
|
ChemSpider | |
ECHA InfoCard
|
100.030.039 |
EC Number |
|
PubChem CID
|
|
RTECS number
|
|
UNII | |
CompTox Dashboard (EPA)
|
|
| |
| |
Properties | |
ThCl4 | |
Molar mass | 373.849 g/mol |
Appearance | white needles hygroscopic
|
Density | 4.59 g/cm3, solid |
Melting point | 770 °C (1,420 °F; 1,040 K) |
Boiling point | 921 °C (1,690 °F; 1,194 K) |
Structure | |
tetragonal | |
Hazards | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
|
332 mg/kg intraperitoneal mouse |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
Thorium(IV) chloride describes a family of inorganic compounds with the formula ThCl4(H2O)n. Both the anhydrous and tetrahydrate (n = 4) forms are known. They are hygroscopic, water-soluble white salts.
Structures
The structure of thorium(IV) chloride features 8-coordinate Th centers with doubly bridging chloride ligands.[1]
Synthesis
ThCl4 was an intermediate in the original isolation of thorium metal by Jons Jacob Berzelius.[2]
Thorium(IV) chloride can be produced in a variety of ways. One method is a carbothermic reaction, 700 °C to 2600 °C, involving thorium oxides and carbon in a stream of chlorine gas:
- ThO2 + 2 C + 4 Cl2 → ThCl4 + 2 CO
The chlorination reaction can be effected with carbon tetrachloride:[3][4]
- Th(C2O4)2 + CCl4 → ThCl4 + 3 CO + 3 CO2
In another two-step method, thorium metal reacts with ammonium chloride:
- Th + 6 NH4Cl → (NH4)2ThCl6 + 4 NH3 + 2 H2
The hexachloride salt is then heated at 350 °C under a high vacuum to produce ThCl4.[5]
Reactions
- Lewis base adducts
ThCl4 reacts with
- Reduction to Th metal
Thorium(IV) chloride is an intermediate in the purification of thorium, which can be affected by:
- Reduction of ThCl4 with alkali metals.
- Electrolysis of anhydrous thorium(IV) chloride in fused mixture of NaCl and KCl.
- Ca reduction of a mixture of ThCl4 with anhydrous zinc chloride.[6]
References
- .
- ISSN 0021-9584.
- ^ Brauer, Georg (1963). Handbook Of Preparative Inorganic Chemistry. New York: Academic Press.
- doi:10.2172/5688597.
- ^ PMID 20107650.
- ^ "Periodic Table of Elements: Los Alamos National Laboratory". periodic.lanl.gov. Retrieved 2016-04-29.