Caesium hydride

Sodium hydride ignites in oxygen at 230°C, and finely divided uranium hydride ignites on contact. Lithium hydride, sodium hydride and potassium hydride react slowly in dry air, while rubidium and caesium hydrides ignite. Reaction is accelerated in moist air, and even finely divided lithium hydride ignites then [1], Finely divided magnesium hydride, prepared by pyrolysis, ignites immediately in air [2], See also COMPLEX HYDRIDES... 

Bromogermane, 0246 Cadmium hydride, 3953 Caesium hydride, 4258 Calcium hydride, 3927 Cerium dihydride, 3962 Cerium trihydride, 3963... 

Caesium dodeca(trifluoromethyl)carbadodecaborane(14)[l-], see Caesium dodecakistrifluoromethylcarba-cfoso-dodecaborate, 3589b Caesium fluoride, 4249 Caesium fluoroxysulfate, 4250 Caesium graphite, 2877 Caesium hexafluorobromate, 0236 Caesium hexahydroaluminate(3—), 0067 Caesium hydride, 4252 Caesium hydrogen xenate, 4253 Caesium lithium tridecahydrononaborate, 0194 Caesium nitrate, 4255 Caesium nitride, 4260 Caesium oxide, 4258... 

Bromogermane, 0246 Cadmium hydride, 3947 Caesium hydride, 4252 Calcium hydride, 3921 Cerium dihydride, 3956 Cerium trihydride, 3957... 

The density of the hydride is 0-92,8 and the vapour-tension for each interval of 10° between 300° C. and 410° C. is 15, 17, 21, 27, 38, 55, 87, 186, 201, 285, 396, and 540 mm. respectively.7 Sodium hydride is the most stable of the alkali-metal hydrides, and caesium hydride the least. The sodium derivative is unaffected by dry air, but decomposes in presence of traces of moisture. Although insoluble in organic solvents such as carbon disulphide, carbon tetrachloride, benzene, and turpentine, it dissolves in the alkali-metals and their amalgams. 

Potassium hydride, KH.—Moissan5 prepared the hydride by a method analogous to that employed by him for the corresponding sodium derivative, the excess of potassium being dissolved by liquid ammonia. Ephraim and Michel6 passed hydrogen into potassium at 350° C., and found the reaction to be promoted by the presence of calcium. The hydride forms white crystals of density 0-80. The vapour-tension for each temperature-interval of 10° between 350° and 410° C. corresponds with the values 56, 83, 120, 168, 228, 308, and 430 mm. respectively.7 In chemical properties potassium hydride resembles the sodium compound, but is less stable. Its stability is greater than that of rubidium hydride or caesium hydride. Carbon dioxide converts it into potassium formate. 

For lithium hydride an early (1981) lattice dynamics simulation [70] was in better agreement with the spectrum recorded on the TOSCA spectrometer than an older (1965) INS spectrum [71]. The INS spectra of the sodium, potassium, rubidium and caesium hydrides were accurately... 

All form the hydride MIT by direct, union of the elements nt sotuo-what elevated temperatures the hydrides with witter give MOJI Ifj, the rubidium and caesium hydrides are unstable at orilinary temperatures. 

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