Chemistry:Caesium monoxide

From HandWiki
Caesium oxide[1][2]
Caesium oxide
  Caesium cations, Cs+
  Oxide anions, O2−
Names
IUPAC name
Caesium oxide
Other names
Cesium oxide (United States )
Identifiers
3D model (JSmol)
ChemSpider
EC Number
  • 243-679-0
Properties
Cs2O
Molar mass 281.810 g·mol−1
Appearance Yellow-orange solid
Density 4.65 g/cm3, solid
Melting point 490 °C (914 °F; 763 K) (under N
2)
Reacts to form CsOH
1534.0·10−6 cm3/mol
Structure
anti-CdCl
2 (hexagonal)
Thermochemistry
76.0 J/(K·mol)
146.9 J/(K·mol)
−345.8 kJ/mol
Hazards
Main hazards Corrosive
GHS pictograms GHS05: CorrosiveGHS08: Health hazard
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acidNFPA 704 four-colored diamond
0
3
2
Flash point non-flammable
Related compounds
Other anions
Other cations
Related caesium oxides
Related compounds
 Caesium hydroxide
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

Caesium monoxide or caesium oxide is an chemical compound with the chemical formula Cs
2O. It is the simplest and most common oxide of the caesium. It 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[3] L. R. Koller described the first modern photoemissive surface in 1929–1930 as a layer of caesium on a layer of caesium oxide on a layer of silver.[4] It is a good electron emitter; however, its high vapor pressure limits its usefulness.[5]

Reactions

Elemental magnesium reduces caesium oxide to elemental caesium, forming magnesium oxide as a side-product:[6][7]

Cs
2O + Mg → 2 Cs + MgO

Cs
2O is hygroscopic, forming the corrosive CsOH on contact with water.

References

  1. ↑ 1.0 1.1 Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. pp. 451, 514. ISBN 0-8493-0487-3. .
  2. ↑ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 97–100. ISBN 978-0-08-022057-4. https://books.google.com/books?id=OezvAAAAMAAJ&q=0-08-022057-6&dq=0-08-022057-6&source=bl&ots=m4tIRxdwSk&sig=XQTTjw5EN9n5z62JB3d0vaUEn0Y&hl=en&sa=X&ei=UoAWUN7-EM6ziQfyxIDoCQ&ved=0CD8Q6AEwBA. .
  3. ↑ Capper, Peter; Elliott, C. T. (2000), Infrared Detectors and Emitters, Springer, p. 14, ISBN 978-0-7923-7206-6, https://books.google.com/books?id=HtgEcjQcgkkC&q=%22cesium+oxide%22+OR+%22caesium+oxide%22&pg=PA14 
  4. ↑ Busch, Kenneth W.; Busch, Marianna A. (1990), Multielement Detection Systems for Spectrochemical Analysis, Wiley-Interscience, p. 12, ISBN 978-0-471-81974-5, https://books.google.com/books?id=9H0W1J-Rku4C&q=%22cesium+oxide%22+OR+%22caesium+oxide%22&pg=PA12 
  5. ↑ Boolchand, Punit, ed. (2000), Insulating and Semiconducting Glasses, World Scientific, p. 855, ISBN 978-981-02-3673-1, Bibcode: 2000isg..book.....B, https://books.google.com/books?id=QK2f4eVh7qgC&q=%22cesium+oxide%22+OR+%22caesium+oxide%22&pg=PA855 
  6. ↑ Turner Jr., Francis M., ed. (1920), The Condensed Chemical Dictionary, New York: Chemical Catalog Co., p. 121, https://books.google.com/books?id=y8y0XE0nsYEC&q=%22cesium+oxide%22+OR+%22caesium+oxide%22&pg=PA121 
  7. ↑ Arora, M.G. (1997), S-Block Elements, New Delhi: Anmol Publications, p. 13, ISBN 978-81-7488-562-3, https://books.google.com/books?id=QR3TCaKaykEC&q=%22Bromine+dioxide%22&pg=PA256 



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