Caesium chloride
| Caesium chloride | |
|---|---|
| |
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| IUPAC name | Caesium chloride |
| Other names | Cesium chloride |
| Identifiers | |
| InChI | InChI=1/ClH.Cs/h1H;/q;+1/p-1 |
| InChIKey | AIYUHDOJVYHVIT-REWHXWOFAO |
| Standard InChI | InChI=1S/ClH.Cs/h1H;/q;+1/p-1 |
| Standard InChIKey | AIYUHDOJVYHVIT-UHFFFAOYSA-M |
| CAS number | [] |
| EC number | |
| ChemSpider | |
| Properties[1] | |
| Chemical formula | CsCl |
| Molar mass | 168.36 g/mol |
| Appearance | white solid, hygroscopic |
| Density | 3.988 g/cm3 |
| Melting point |
645 °C |
| Boiling point |
1290 °C |
| Solubility in water | 162.22 g/100 ml (0.7 °C) 259.56 g7100 ml (89.5 ºC) |
| Solubility in methanol | 33.7 g/100 ml (25 ºC) |
| Solubility in ethanol | very soluble |
| Solubility in acetone | insoluble |
| Refractive index (nD) | 1.6418 |
| Structure | |
| Crystal structure | Caesium chloride (see text) |
| Space group | Pm3m, No. 221 |
| Coordination geometry | Cubic (Cs+) Cubic (Cl−) |
| Hazards | |
| Material safety data sheet (MSDS) | External MSDS |
| EU index number | not listed |
| Flash point | non-flammable |
| Related compounds | |
| Other anions | Caesium fluoride Caesium bromide Caesium iodide |
| Other cations | Lithium chloride Sodium chloride Potassium chloride Rubidium chloride |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Caesium chloride is the chemical compound with the formula CsCl. This colorless solid is an important source of caesium ions in a variety of applications. CsCl is also well known as a structural type.
Contents
Preparation
Caesium chloride can be prepared by the reaction of caesium hydroxide or caesium carbonate with hydrochloric acid: the resulting salt is purified by recrystallization.
Crystal structure
The caesium chloride structure is composed of a primitive cubic lattice with a two atom basis, where both atoms have eight-fold coordination. The chloride atoms lie upon the lattice points at the edges of the cube, while the caesium atoms lie in the holes in the center of the cubes. This structure is shared with CsBr and CsI and many intermetallic compounds. In contrast, the other alkal metal halides have the sodium chloride structure.[2] When both ions are similar in size (Cs+ ionic radius 174 pm for this coordination number, Cl− 181 pm) the CsCl structure is adopted, when they are different (Na+, 102 pm; Cl−, 181 pm) the sodium chloride structure is adopted.
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unit cell of the CsCl structure |
coordination of Cs and Cl in CsCl |
Uses
Caesium chloride is also widely used in the centrifugation in a technique known as isopycnic centrifugation. Centrifugal and diffusive forces establish a density gradient which allows separation of mixtures on the basis of their molecular density. This technique allows separation of DNA of different densities (e.g. DNA fragments with differing A-T or G-C content).[3]
Radioisotopes of caesium chloride are used in nuclear medicine, including treatment of cancer. In the production of radioactive sources, it is normal to choose a chemical form of the radioisotope which would not be readily dispersed in the environment in the event of an accident. For instance, radiothermal generators (RTGs) often use strontium titanate, which is insoluble in water. For teletherapy sources, however, the radioactive density (activity in a given volume) needs to be very high, which is not possible with known insoluble caesium compounds. A thimble-shaped container of radioactive caesium chloride provides the active source. In the Goiânia accident, such a source was reptured, leading to several deaths.
Miscellaneous applications
Caesium chloride (non-radioactive) is also promoted as an alternative cancer therapy.[4] Caesium chloride is used in the preparation of electrically conducting glasses.[5]
References
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-91. ISBN 0-8493-0462-8.
- ↑ Wells, A. F. Structural Inorganic Chemistry, 5th ed.; Clarendon Press: Oxford, 1984. ISBN 0-19-855370-6
- ↑ Bick, Manfred; Prinz, Horst Cesium and Cesium Compounds. In Ullmann’s Encyclopedia of Industrial Chemistry, 5th ed.; Wiley-VCH: Weinheim, 2005. DOI: 10.1002/14356007.a06_153.
- ↑ Sartori, H. E. Cesium therapy in cancer patients. Pharmacol. Biochem. Behav. 1984, 21 (Suppl 1), 11. PMID 6522427.
- ↑ Tver'yanovich, Y. S.; et al. Glass Phys. Chem. 1998, 24, 446.
External links
- Biodegradation and Bioconcentration of caesium chloride from the National Institute of Technology and Evaluation (Japan)
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