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Lithium bromide was used as a sedative beginning in the early 1900s, but it fell into disfavor in the 1940s as newer sedatives became available and when some heart patients died after using the salt substitute lithium chloride. [11] Like lithium carbonate and lithium chloride, it was used as treatment for bipolar disorder.
The Gmelin rare earths handbook lists 1522 °C and 1550 °C as two melting points given in the literature, the most recent reference [Handbook on the chemistry and physics of rare earths, vol.12 (1989)] is given with 1529 °C.
The melting point of a substance is the point where it changes state from solid to liquid while the boiling point of a substance (in liquid state) is the point where the vapour pressure of the liquid equals the environmental pressure surrounding the liquid [102] [103] and all the liquid changes state to gas.
Melting point: 849 °C (1,560 °F; 1,122 K) ... Lithium metaborate is a chemical compound of lithium, ... with a small amount of lithium bromide.
Melting point: 469 °C (876 °F; 742 K) Boiling point: 1,171 °C (2,140 °F; 1,444 K) ... Lithium chloride Lithium bromide Lithium astatide: Other cations. Sodium iodide
Lithium forms salt-like derivatives with all halides and pseudohalides. Some examples include the halides LiF, LiCl, LiBr, LiI, as well as the pseudohalides and related anions. Lithium carbonate has been described as the most important compound of lithium. [100] This white solid is the principal product of beneficiation of lithium ores.
Melting point: 718 °C (1,324 °F; 991 K) ... Rubidium bromide ... Other cations. Lithium chloride Sodium chloride Potassium chloride Caesium chloride
Lithium borohydride (LiBH 4) is a borohydride and known in organic synthesis as a reducing agent for esters. Although less common than the related sodium borohydride , the lithium salt offers some advantages, being a stronger reducing agent and highly soluble in ethers, whilst remaining safer to handle than lithium aluminium hydride .