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Caesium chloride Other names Cesium chloride Identifiers CAS number 7647-17-8 Y ChemSpider 22713 Y UNII GNR9HML8BA Y EC number 231-600-2 Jmol-3D images Image 1 SMILES [Cs+].[Cl-] InChI InChI=1S/ClH.Cs/h1H;/q;+1/p-1 Y Key: AIYUHDOJVYHVIT-UHFFFAOYSA-M Y InChI=1/ClH.Cs/h1H;/q;+1/p-1 Key: AIYUHDOJVYHVIT-REWHXWOFAO Properties Molecular formula CsCl Molar mass 168.36 g/mol Appearance white solid hygroscopic Density 3.99 g/cm3 Melting point 645 °C Boiling point 1297 °C (vaporizes) Solubility in water 1620 g/L (1 °C) Solubility soluble in ethanol[1] Structure Crystal structure Caesium chloride (see text) Coordination geometry simple cubic (interpenetrating) Related compounds Other anions Caesium fluoride Caesium bromide Caesium iodide Other cations Lithium chloride Sodium chloride Potassium chloride Rubidium chloride  Y(what is this?)  (verify) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references Caesium chloride is the inorganic 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 1 Preparation 2 Crystal structure 3 Uses 3.1 Miscellaneous applications 4 References 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 Main article: Cubic crystal system The caesium chloride structure adopts a primitive cubic lattice with a two atom basis, where both atoms have eightfold 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 alkaline 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+ ionic radius 102 pm, Cl− 181 pm) the sodium chloride structure is adopted. Ball-and-stick model of the unit cell of the CsCl structure Ball-and-stick model of the cubic coordination of Cs and Cl in CsCl Uses Caesium chloride is widely used in centrifugation in a technique known as isopycnic centrifugation. Centripetal 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 (Ci 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 ruptured, leading to several deaths. Miscellaneous applications Caesium chloride (non-radioactive) has also promoted as an alternative cancer therapy[4], but has been linked to the deaths of over 50 patients, when it was used as part of a scientifically unvalidated cancer treatment.[5] Caesium chloride is used in the preparation of electrically conducting glasses.[6] References ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–67; 1363, ISBN 0849305942  ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6 ^ Manfred Bick and Horst Prinz "Cesium and Cesium Compounds” in Ullmann’s Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim.doi:10.1002/14356007.a06_153. ^ Sartori H. E. "Cesium therapy in cancer patients." Pharmacol Biochem Behav. 1984;21 Suppl 1:11-3.PMID: 6522427. ^ Wood, Leonie. "'Cured' cancer patients died, court told". The Sydney Morning Herald. 20 November 2010.  ^ Tver'yanovich, Y. S. et al. (1998). Glass Phys. Chem., 24, 446. v · d · e  Caesium compounds CsBr · CsCl · CsClO4 · Cs2CrO4 · CsF · CsH · CsI · CsNO3 · CsOH · Cs2CO3 · Cs2SO4 · CsC2H3O2 · Cs2O · Cs2TiO2