| |
| Names | |
|---|---|
|
IUPAC name
Caesium peroxide
| |
| Identifiers | |
| Properties | |
| Cs2O2 | |
| Molar mass | 297.809 g·mol−1 |
| Appearance | Yellowish [1] |
| Structure | |
| Orthorhombic [2] | |
| Related compounds | |
Other
cations
|
|
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
| |
Caesium peroxide or cesium peroxide is an inorganic compound of caesium and oxygen with the chemical formula Cs2 O2. It can be formed from caesium metal by adding a stoichiometric amount in ammonia solution, or oxidizing the solid metal directly. [1]
- 2 Cs + O2 → Cs2O2
It can also be formed by the thermal decomposition of caesium superoxide: [3]
- 2 CsO2 → Cs2O2 + O2
Upon heating until 650 °C, the compound will decompose to caesium monoxide and atomic oxygen: [4]
- Cs2O2 → Cs2O + [O]
Caesium peroxide shows a Raman vibration at 743 cm−1, due to the presence of the peroxide ions. [5] The compound is often used as a coating for photocathodes, due to its low work function. [6]
- ^ a b I. I. Volnov (2012). Peroxides, Superoxides, and Ozonides of Alkali and Alkaline Earth Metals. Springer. p. 45. ISBN 9781468482522.
- ^ Band, A.; Albu-Yaron, A.; Livneh, T.; Cohen, H.; Feldman, Y.; Shimon, L.; Popovitz-Biro, R.; Lyahovitskaya, V.; Tenne, R. (2004-07-27). "Characterization of Oxides of Cesium". The Journal of Physical Chemistry B. 108 (33). American Chemical Society (ACS): 12360–12367. doi: 10.1021/jp036432o. ISSN 1520-6106.
- ^ Berardinelli, S. P.; Kraus, D. L. (1974-01-01). "Thermal decomposition of the higher oxides of cesium in the temperature range 320-500.deg". Inorganic Chemistry. 13 (1). American Chemical Society (ACS): 189–191. doi: 10.1021/ic50131a037. ISSN 0020-1669.
- ^ Zefirov, Nikolaj (1995). Chimičeskaja ėnciklopedija : v pjati tomach (in Bosnian). Moskva: Izdat. p. 658. ISBN 5-85270-092-4. OCLC 258155382.
- ^ Livneh, Tsachi; Band, Alisa; Tenne, Reshef (2002). "Raman scattering from the peroxide ion in Cs2O2". Journal of Raman Spectroscopy. 33 (8). Wiley: 675–676. Bibcode: 2002JRSp...33..675L. doi: 10.1002/jrs.900. ISSN 0377-0486.
- ^ Sun, Yun; Liu, Zhi; Pianetta, Piero; Lee, Dong-Ick (2007). "Formation of cesium peroxide and cesium superoxide on InP photocathodes activated by cesium and oxygen". Journal of Applied Physics. 102 (7). AIP Publishing: 074908–074908–6. Bibcode: 2007JAP...102g4908S. doi: 10.1063/1.2786882. ISSN 0021-8979.
 | This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |
|
| |
| Names | |
|---|---|
|
IUPAC name
Caesium peroxide
| |
| Identifiers | |
| Properties | |
| Cs2O2 | |
| Molar mass | 297.809 g·mol−1 |
| Appearance | Yellowish [1] |
| Structure | |
| Orthorhombic [2] | |
| Related compounds | |
Other
cations
|
|
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
| |
Caesium peroxide or cesium peroxide is an inorganic compound of caesium and oxygen with the chemical formula Cs2 O2. It can be formed from caesium metal by adding a stoichiometric amount in ammonia solution, or oxidizing the solid metal directly. [1]
- 2 Cs + O2 → Cs2O2
It can also be formed by the thermal decomposition of caesium superoxide: [3]
- 2 CsO2 → Cs2O2 + O2
Upon heating until 650 °C, the compound will decompose to caesium monoxide and atomic oxygen: [4]
- Cs2O2 → Cs2O + [O]
Caesium peroxide shows a Raman vibration at 743 cm−1, due to the presence of the peroxide ions. [5] The compound is often used as a coating for photocathodes, due to its low work function. [6]
- ^ a b I. I. Volnov (2012). Peroxides, Superoxides, and Ozonides of Alkali and Alkaline Earth Metals. Springer. p. 45. ISBN 9781468482522.
- ^ Band, A.; Albu-Yaron, A.; Livneh, T.; Cohen, H.; Feldman, Y.; Shimon, L.; Popovitz-Biro, R.; Lyahovitskaya, V.; Tenne, R. (2004-07-27). "Characterization of Oxides of Cesium". The Journal of Physical Chemistry B. 108 (33). American Chemical Society (ACS): 12360–12367. doi: 10.1021/jp036432o. ISSN 1520-6106.
- ^ Berardinelli, S. P.; Kraus, D. L. (1974-01-01). "Thermal decomposition of the higher oxides of cesium in the temperature range 320-500.deg". Inorganic Chemistry. 13 (1). American Chemical Society (ACS): 189–191. doi: 10.1021/ic50131a037. ISSN 0020-1669.
- ^ Zefirov, Nikolaj (1995). Chimičeskaja ėnciklopedija : v pjati tomach (in Bosnian). Moskva: Izdat. p. 658. ISBN 5-85270-092-4. OCLC 258155382.
- ^ Livneh, Tsachi; Band, Alisa; Tenne, Reshef (2002). "Raman scattering from the peroxide ion in Cs2O2". Journal of Raman Spectroscopy. 33 (8). Wiley: 675–676. Bibcode: 2002JRSp...33..675L. doi: 10.1002/jrs.900. ISSN 0377-0486.
- ^ Sun, Yun; Liu, Zhi; Pianetta, Piero; Lee, Dong-Ick (2007). "Formation of cesium peroxide and cesium superoxide on InP photocathodes activated by cesium and oxygen". Journal of Applied Physics. 102 (7). AIP Publishing: 074908–074908–6. Bibcode: 2007JAP...102g4908S. doi: 10.1063/1.2786882. ISSN 0021-8979.
|
| This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |