|Jmol-3D images||Image 1|
|Molar mass||149.912 g/mol|
|Appearance||Whitish-yellow deliquescent crystals|
|Melting point||272 °C (522 °F; 545 K)|
|Solubility in water||300 g/100 mL at 30 °C|
|Solubility||Soluble in ethanol|
heat capacity C
|Std enthalpy of
|EU Index||Not listed|
|Flash point||Not flammable|
|LD50||570 mg/kg (oral, rat)|
|Other anions||Caesium oxide
|Other cations||Lithium hydroxide
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Cesium hydroxide (CsOH) is a chemical compound consisting of an ion of cesium and a hydroxide ion. It is a strong base (pKb=-1.76), much like other alkali metal hydroxides such as sodium hydroxide and potassium hydroxide. In fact, caesium hydroxide is powerful enough to quickly corrode through glass.
It is an anisotropic etchant of silicon, exposing octahedral planes. This technique can form pyramids and regularly shaped etch pits for uses such as Microelectromechanical systems. It is known to have a higher selectivity to etch highly p-doped silicon than the more commonly used potassium hydroxide.
However, this compound is not usually used in experiments as the extraction of cesium is very expensive and the fact that it behaves very much like rubidium hydroxide and potassium hydroxide although it is more reactive than they are.
Cesium hydroxide can be obtained by the following chemical reaction:
- 2 Cs + 2 H2O → 2 CsOH + H2
The above reaction occurs explosively with enough force to shatter a Pyrex beaker. Cesium metal will react with ice above −116 °C.
- Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–51, ISBN 0-8493-0594-2
- Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 5–14, ISBN 0-8493-0594-2