Caesium chromate
| Identifiers | |
|---|---|
| 13454-78-9 | |
| 3D model (Jmol) | Interactive image |
| ChemSpider | 55521 |
| ECHA InfoCard | 100.033.296 |
| EC Number | 236-640-4 |
| PubChem | 61613 |
| |
| |
| Properties[1] | |
| Cs2CrO4 | |
| Appearance | Yellow crystalline solid |
| Density | 4.237 g/cm3 |
| 71.4 g/100 ml (13 °C) | |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions |
Caesium sulfate |
| Other cations |
Sodium chromate Potassium chromate Ammonium chromate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Caesium chromate, the caesium salt of chromic acid, is used to produce caesium vapour by reaction with silicon, boron, or titanium,[2] which is used to in the final stages of creating vacuum tubes; the caesium vapour reacts with the remaining gases, including nitrogen and oxygen.[3]
References
- ↑ Weast, Robert C., ed. (1981). CRC Handbook of Chemistry and Physics (62nd ed.). Boca Raton, FL: CRC Press. p. B-91. ISBN 0-8493-0462-8..
- ↑ Liebhafsky, H. A.; Winslow, A. F. (1947), "Cesium Chromate Photo‐Tube Pellets", Journal of Applied Physics, Journal of Applied Physics, Vol. 18, No. 12, 18 (12): 1128, doi:10.1063/1.1697594
- ↑ Emsley, John (2001), Nature's Building Blocks: An A-Z Guide to the Elements, Oxford University Press, p. 81, ISBN 0-19-850340-7.
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