Caesium perchlorate
From Wikipedia, the free encyclopedia
| Caesium perchlorate | |
|---|---|
 |
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| IUPAC name | Caesium perchlorate |
| Other names | Cesium perchlorate |
| Identifiers | |
| CAS number | [13454-84-7] |
| PubChem | |
| EINECS number | |
| SMILES | [O-]Cl(=O)(=O)=O.[Cs+] |
| Properties | |
| Molecular formula | CsClO4 |
| Molar mass | 232.355 g.mol-1 |
| Appearance | Colorless crystalls |
| Density | 3.327 g.cm-3[1] |
| Melting point |
250 °C[1] |
| Solubility in water | 1.974 g / 100 ml |
| Hazards | |
| R-phrases | R8 |
| S-phrases | S17 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Caesium perchlorate, CsClO4 (also known as cesium perchlorate), is a perchlorate of caesium. It forms white hygroscopic crystals in the solid state soluble in water and alcohol.
Under temperature 219 °C it has orthorhombic structure Pnma with lattice constants a = 9.82, b = 6.00, c = 7.79 (.10-1 nm). Above 219 °C it crystallizes in cubic crystallic structure F43m with lattice constant a = 7.98 . 10-1 nm.[2]
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 is attributed to the formation of aggregates between the metal atom and the perchlorate anion.
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 CsCl at 575 °C. Like all perchlorates, it is a strong oxidant and may react violently with reducing agents and organic materials, especially at elevated temperatures.
Caesium perchlorate helped in discovering francium and identifying it as an alkali metal because francium-223 coprecipitated with cesium perchlorate.[4][5]
[edit] See also
[edit] References
- ^ a b c Dale L. Perry, Sidney L. Phillips. Handbook of Inorganic Compounds. CRC Press, 1995
- ^ a b F. Brezina, J. Mollin, R. Pastorek, Z. Sindelar. Chemicke tabulky anorganickych sloucenin (Chemical tables of inorganic compounds). SNTL, 1986.
- ^ A. Earnshaw, Norman Greenwood. Chemistry of the Elements, Second Edition. Butterworth-Heinemann, 1997
- ^ Martin Ambrose Paul, Edward Jasper King, Larkin Hundley Farinholt. General Chemistry. Harcourt, Brace & World, 1967. D. E. Barnes. Newnes Concise Encyclopaedia of Nuclear Energy. G. Newnes, 1962.
- ^ E. K. Hyde (1952). "Radiochemical Methods for the Isolation of Element 87 (Francium)". J. Am. Chem. Soc. 74 (16): 4181–4184. doi:.
