Back Sesiumchloried Afrikaans كلوريد السيزيوم Arabic سزیوم کولورید AZB সিজিয়াম ক্লোরাইড Bengali/Bangla Chlorid cesný Czech Caesiumchlorid German Χλωριούχο καίσιο Greek Cezia klorido Esperanto Cloruro de cesio Spanish سزیم کلرید Persian

Caesium chloride

"CsCl" redirects here. For other uses, see CSCL.
Caesium chloride
Names
IUPAC name
Caesium chloride
Other names
Cesium chloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.728 Edit this at Wikidata
EC Number
  • 231-600-2
UNII
  • InChI=1S/ClH.Cs/h1H;/q;+1/p-1 checkY
    Key: AIYUHDOJVYHVIT-UHFFFAOYSA-M checkY
  • InChI=1/ClH.Cs/h1H;/q;+1/p-1
    Key: AIYUHDOJVYHWHXWOFAO
  • [Cs+].[Cl-]
Properties
CsCl
Molar mass 168.36 g/mol
Appearance white solid
hygroscopic
Density 3.988 g/cm3[1]
Melting point 646 °C (1,195 °F; 919 K)[1]
Boiling point 1,297 °C (2,367 °F; 1,570 K)[1]
1910 g/L (25 °C)[1]
Solubility soluble in ethanol[1]
Band gap 8.35 eV (80 K)[2]
-56.7·10−6 cm3/mol[3]
1.712 (0.3 μm)
1.640 (0.59 μm)
1.631 (0.75 μm)
1.626 (1 μm)
1.616 (5 μm)
1.563 (20 μm)[4]
Structure
CsCl, cP2
Pm3m, No. 221[5]
a = 0.4119 nm
0.0699 nm3
1
Cubic (Cs+)
Cubic (Cl−)
Hazards
GHS labelling:
GHS07: Exclamation markGHS08: Health hazard
Warning
H302, H341, H361, H373
P201, P202, P260, P264, P270, P281, P301+P312, P308+P313, P314, P330, P405, P501
Lethal dose or concentration (LD, LC):
2600 mg/kg (oral, rat)[6]
Related compounds
Other anions
 Caesium fluoride
Caesium bromide
Caesium iodide
Caesium astatide
Other cations
 Lithium chloride
Sodium chloride
Potassium chloride
Rubidium chloride
Francium chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Caesium chloride or cesium chloride is the inorganic compound with the formula CsCl. This colorless salt is an important source of caesium ions in a variety of niche applications. Its crystal structure forms a major structural type where each caesium ion is coordinated by 8 chloride ions. Caesium chloride dissolves in water. CsCl changes to NaCl structure on heating. Caesium chloride occurs naturally as impurities in carnallite (up to 0.002%), sylvite and kainite. Less than 20 tonnes of CsCl is produced annually worldwide, mostly from a caesium-bearing mineral pollucite.[7]

Caesium chloride is widely used in isopycnic centrifugation for separating various types of DNA. It is a reagent in analytical chemistry, where it is used to identify ions by the color and morphology of the precipitate. When enriched in radioisotopes, such as 137CsCl or 131CsCl, caesium chloride is used in nuclear medicine applications such as treatment of cancer and diagnosis of myocardial infarction. Another form of cancer treatment was studied using conventional non-radioactive CsCl. Whereas conventional caesium chloride has a rather low toxicity to humans and animals, the radioactive form easily contaminates the environment due to the high solubility of CsCl in water. Spread of 137CsCl powder from a 93-gram container in 1987 in Goiânia, Brazil, resulted in one of the worst-ever radiation spill accidents killing four and directly affecting 249 people.

  1. ^ a b c d e Haynes, p. 4.57
  2. ^ Lushchik, A; Feldbach, E; Frorip, A; Ibragimov, K; Kuusmann, I; Lushchik, C (1994). "Relaxation of excitons in wide-gap CsCl crystals". Journal of Physics: Condensed Matter. 6 (12): 2357–2366. Bibcode:1994JPCM....6.2357L. doi:10.1088/0953-8984/6/12/009. S2CID 250824677.
  3. ^ Haynes, p. 4.132
  4. ^ Haynes, p. 10.240
  5. ^ Watanabe, M.; Tokonami, M.; Morimoto, N. (1977). "The transition mechanism between the CsCl-type and NaCl-type structures in CsCl". Acta Crystallographica Section A. 33 (2): 294. Bibcode:1977AcCrA..33..294W. doi:10.1107/S0567739477000722.
  6. ^ Cesium chloride. nlm.nih.gov
  7. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

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