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Caesium perchlorate or cesium perchlorate (CsClO4), is a perchlorate of caesium. It forms white crystals, which are sparingly soluble in cold water and ethanol. It dissolves more easily in hot water.

Caesium perchlorate[1][2]
Cesium perchlorate.png
Cesium perchlorate 25g.jpg
Names
IUPAC name
Caesium perchlorate
Other names
Cesium perchlorate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.298
EC Number
  • 236-643-0
Properties
CsClO4
Molar mass 232.36 g/mol
Appearance Colorless crystals
Density 3.327 g/cm3
Melting point 250 °C (482 °F; 523 K) (decomposes)
1.974 g/100 ml (25 °C)
1.4887
Structure
orthorhombic (<219 °C)
cubic (>219 °C, a = 798 pm)
Pnma (<219 °C)
F43m (>219 °C)
a = 982 pm, b = 600 pm, c = 779 pm (orthorhombic, <219 °C)
Hazards
Safety data sheet External MSDS
Flash point Non-flammable
Related compounds
Other anions
Caesium chloride
Caesium chlorate
Other cations
Lithium perchlorate
Sodium perchlorate
Potassium perchlorate
Rubidium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

CsClO4 is the least soluble of the alkali metal perchlorates (followed by Rb, K, Li, and Na), a property which may be used for separatory purposes and even for gravimetric analysis. [3] This low solubility played an important role in the characterization of francium as an alkali metal, as francium perchlorate coprecipitates with caesium perchlorate.[4]

Table of solubility in water[1][2]
Temperature (°C) 0 8.5 14 25 40 50 60 70 99
Solubility (g / 100 ml) 0.8 0.91 1.91 1.974 3.694 5.47 7.30 9.79 28.57

When heated, CsClO4 decomposes to caesium chloride above 250 °C. Like all perchlorates, it is a strong oxidant and may react violently with reducing agents and organic materials, especially at elevated temperatures.

ReferencesEdit

  1. ^ a b Perry, Dale L.; Phillips, Sidney L. (1995), Handbook of Inorganic Compounds, CRC Press.
  2. ^ a b Brezina, F.; Mollin, J.; Pastorek, R.; Sindelar, Z. (1986), Chemicke tabulky anorganickych sloucenin, SNTL.
  3. ^ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 1017. ISBN 978-0-08-022057-4..
  4. ^ Hyde, E. K. (1952), "Radiochemical Methods for the Isolation of Element 87 (Francium)", J. Am. Chem. Soc., 74 (16): 4181–84, doi:10.1021/ja01136a066

External linksEdit