Caesium oxide
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| Caesium oxide[1][2] | |
|---|---|
| |
| IUPAC name | Caesium oxide |
| Other names | Cesium oxide (US) |
| Identifiers | |
| InChI | InChI=1/2Cs.O/q2*+1;-2 |
| CAS number | [] |
| EC number | |
| ChemSpider | |
| Properties | |
| Chemical formula | Cs2O |
| Molar mass | 281.81 g/mol |
| Appearance | yellow-orange solid |
| Density | 4.65 g/cm3, solid |
| Melting point |
490 °C (under N2) |
| Solubility in water | very soluble in water |
| Structure | |
| Crystal structure | anti-CdCl2 (hexagonal) |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-345.8 kJ/mol |
| Standard molar entropy S |
146.9 J K-1 mol-1 |
| Specific heat capacity C | 76.0 J K-1 mol-1 |
| Hazards | |
| EU index number | not listed |
| Flash point | non-flammable |
| Related compounds | |
| Other anions | Caesium hydroxide |
| Other cations | Lithium oxide Sodium oxide Potassium oxide Rubidium oxide |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Caesium oxide (IUPAC name) or cesium oxide describes inorganic compounds composed of caesium and oxygen. The following binary (containing only Cs and O) oxides of caesium are known: Cs11O3, Cs4O, Cs7O, and Cs2O.[3]. Both the oxide and suboxides are brightly coloured. The species Cs2O forms yellow-orange hexagonal crystals.[1]
Uses
Caesium oxide is used in photocathodes to detect infrared signals in devices such as image intensifiers, vacuum photodiodes, photomultipliers, and TV camera tubes[4] L. R. Koller described the first modern photoemissive surface in 1929–30 as a layer of caesium on a layer of caesium oxide on a layer of silver.[5] It is a good electron emitter; however, its high vapor pressure limits its usefulness[6].
Reactions
Elemental magnesium reduces caesium oxide to elemental caesium:[7][8]
- Cs2O + Mg → Cs + MgO
References
- ↑ 1.0 1.1 CRC Handbook of Chemistry and Physics, 87th ed.; Lide, David R., Ed.; CRC Press: Boca Raton, FL, 2006; pp 451, 514. ISBN 0-8493-0487-3.
- ↑ Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 97–100. ISBN 0-08-022057-6.
- ↑ Simon, A. Group 1 and 2 Suboxides and Subnitrides — Metals with Atomic Size Holes and Tunnels. Coord. Chem. Rev. 1997, 163, 253–270. DOI: 10.1016/S0010-8545(97)00013-1.
- ↑ Capper, Peter; Elliott, C. T. Infrared Detectors and Emitters; Springer, 2000; p 14. ISBN 9780792372066, <http://books.google.com/books?id=HtgEcjQcgkkC&pg=PA14&dq=%22cesium+oxide%22+OR+%22caesium+oxide%22&lr=&as_drrb_is=b&as_minm_is=1&as_miny_is=2000&as_maxm_is=12&as_maxy_is=2009&as_brr=3&as_pt=ALLTYPES&ei=2nrASdqVM46syASCgN3SBA&client=firefox-a#PPA14,M1>
- ↑ Busch, Kenneth W.; Busch, Marianna A. Multielement Detection Systems for Spectrochemical Analysis; Wiley-Interscience, 1990; p 12. ISBN 9780471819745, <http://books.google.com/books?id=9H0W1J-Rku4C&pg=PA12&dq=%22cesium+oxide%22+OR+%22caesium+oxide%22&lr=&as_drrb_is=q&as_minm_is=1&as_miny_is=1776&as_maxm_is=12&as_maxy_is=2009&as_brr=3&as_pt=ALLTYPES&ei=wILASe63I5K8zATZtPHGBA&client=firefox-a>
- ↑ Insulating and Semiconducting Glasses; Boolchand, Punit, Ed.; World Scientific, 2000; p 855. ISBN 9789810236731, <http://books.google.com/books?id=QK2f4eVh7qgC&pg=PA855&dq=%22cesium+oxide%22+OR+%22caesium+oxide%22&lr=&as_drrb_is=b&as_minm_is=1&as_miny_is=2000&as_maxm_is=12&as_maxy_is=2009&as_brr=3&as_pt=ALLTYPES&ei=1HzASbD0BpX8ygTl4MTODQ&client=firefox-a>
- ↑ The Condensed Chemical Dictionary; Turner, Jr., Francis M., Ed.; Chemical Catalog Co.: New York, 1920; p 121, <http://books.google.com/books?id=y8y0XE0nsYEC&pg=PA121&dq=%22cesium+oxide%22+OR+%22caesium+oxide%22&lr=&as_drrb_is=q&as_minm_is=1&as_miny_is=1776&as_maxm_is=12&as_maxy_is=2009&as_brr=3&as_pt=ALLTYPES&ei=rIDAScrTMIPmzASo-si9Ag&client=firefox-a#PPA121,M1>
- ↑ Arora, M.G. S-Block Elements; Anmol Publications: New Delhi, 1997; p 13. ISBN 9788174885623, <http://books.google.com/books?id=XPuh2knuV6EC&pg=PA30&dq=%22cesium+oxide%22+OR+%22caesium+oxide%22+pollucite&lr=&as_brr=3&as_pt=ALLTYPES&ei=G4TASZWJIqSayASz6eGWAg&client=firefox-a#PPA30,M1>
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