Thorium(IV) chloride
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3D model (JSmol)
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| ECHA InfoCard | 100.030.039 |
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PubChem CID
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| 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 | |
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EU classification (DSD) (outdated)
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not listed |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 (what is   ?) |
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| Infobox references | |
Thorium(IV) chloride (ThCl4) is an inorganic chemical compound. In addition to the anhydrous ThCl4, two hydrates have been reported: ThCl4(H2O)4 and ThCl4(H2O)8. These hydroscopic salts are water-soluble and white, at room temperature. Similar to other thorium complexes thorium(IV) chloride has a high melting point 770 °C (1,418 °F) and a boiling point of 921 °C (1,690 °F). Like all the other actinides, thorium is radioactive and has sometimes been used in the production of nuclear energy. Thorium(IV) chloride does not appear naturally but instead is derived from Thorite, Thorianite, or Monazite which are naturally occurring formations.
Thorium was first discovered by Jons Jacob Berzelius in 1828. After receiving a sample of minerals from his colleague Jens Esmarck, Berzelius was able to isolate thorium using a method that had been used for other metals like cerium, zirconium, and titanium. This process involved using alkali metals to disassociate the thorium from its prior ligand form ThSiO4 (further described in synthesis). An intermediate in the isolation process was thorium(IV) chloride and thus the compound was discovered.
The structure of thorium(IV) chloride is square planar with a symmetry of D4h. In this coordinate compound the bond length between the Th-Cl bond is 2.690 Å. The structure has been reported as hydrous or anhydrous. Due to the compound’s hydroscopic nature in the presence of water it can form either ThCl4(H2O)4 and ThCl4(H2O)8.
Thorium(IV) Chloride can be produced in a variety of ways but the most common starting reactant is either thorium dioxide or Thorium (IV) orthosilicate.
One way thorium(IV) chloride is synthesized is through a carbothermic reaction. The carbothermic reaction require very high temperature ranging from 700 °C to 2600 °C. What necessitates these extreme environments are thorium dioxides melting temperature of 3,390 °C. The reaction between graphite and thorium dioxide usually takes place in a stream of chlorine gas forming the thorium(IV) chloride. However the chlorination reaction can be done by another compound Cl2-CCl4 which is a more stable reactant than pure Chlorine gas. Cl2-CCl4 is formed by passing a gas mixture of Cl2 through a wash bottle filled with CCl4.
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