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Caesium hydroxide is a strong base (pK a = 15.76) containing the highly reactive alkali metal caesium, much like the other alkali metal hydroxides such as sodium hydroxide and potassium hydroxide.
Water-reactive substances [1] are those that spontaneously undergo a chemical reaction with water, often noted as generating flammable gas. [2] Some are highly reducing in nature. [ 3 ] Notable examples include alkali metals , lithium through caesium , and alkaline earth metals , magnesium through barium .
A water molecule in the first solvation shell of an aqua ion may exchange places with a water molecule in the bulk solvent. It is usually assumed that the rate-determining step is a dissociation reaction. [M(H 2 O) n] z+ → [M(H 2 O) n-1] z+ * + H 2 O. The * symbol signifies that this is the transition state in a chemical reaction. The rate of ...
Caesium oxalate (standard IUPAC spelling), or dicesium oxalate, or cesium oxalate (American spelling) is a chemical compound with the chemical formula Cs 2 C 2 O 4. It is a caesium salt of oxalic acid .
Caesium (IUPAC spelling; [9] also spelled cesium in American English) is a chemical element; it has symbol Cs and atomic number 55. It is a soft, silvery-golden alkali metal with a melting point of 28.5 °C (83.3 °F; 301.6 K), which makes it one of only five elemental metals that are liquid at or near room temperature .
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]
Caesium ozonide is an oxygen-rich chemical compound of caesium, with the chemical formula Cs O 3. It consists of caesium cations Cs + and ozonide anions O − 3. It can be formed by reacting ozone with caesium superoxide: [2] [3] CsO 2 + O 3 → CsO 3 + O 2. The compound reacts strongly with any water in the air forming caesium hydroxide. [3] 4 ...
It reacts with water to form hydrogen peroxide and caesium hydroxide. [2] 2 CsO 2 + 2 H 2 O → O 2 ↑ + H 2 O 2 + 2 CsOH. Heating to approximately 400 °C induces thermal decomposition to caesium peroxide. [3] The standard enthalpy of formation ΔH f 0 of caesium superoxide is −295 kJ/mol. [4] Caesium superoxide reacts with ozone to form ...