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Lithium iodide, or LiI, is a compound of lithium and iodine. When exposed to air , it becomes yellow in color, due to the oxidation of iodide to iodine. [ 2 ] It crystallizes in the NaCl motif . [ 3 ]
Lithium hydroxide – LiOH; Lithium iodide – LiI; Lithium iron phosphate – FeLiO 4 P; Lithium nitrate – LiNO 3; Lithium sulfide – Li 2 S; Lithium sulfite – Li 2 SO 3; Lithium sulfate – Li 2 SO 4; Lithium superoxide – LiO 2; Lithium hexafluorophosphate – LiPF 6
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Lithium enolate formation can be generalized as an acid–base reaction, in which the relatively acidic proton α to the carbonyl group (pK =20-28 in DMSO) reacts with organolithium base. Generally, strong, non-nucleophilic bases, especially lithium amides such LDA, LiHMDS and LiTMP are used.
Hydroiodic acid (or hydriodic acid) is a colorless liquid. It is an aqueous solution of hydrogen iodide with the chemical formula H I. It is a strong acid, in which hydrogen iodide is ionized completely in an aqueous solution. Concentrated aqueous solutions of hydrogen iodide are usually 48% to 57% HI by mass. [2] An oxidized solution of ...
Typically lithium fluoride is mixed with beryllium fluoride to form a base solvent , into which fluorides of uranium and thorium are introduced. Lithium fluoride is exceptionally chemically stable and LiF/ BeF 2 mixtures ( FLiBe ) have low melting points (360 to 459 °C or 680 to 858 °F) and the best neutronic properties of fluoride salt ...
Lithium chloride is a chemical compound with the formula Li Cl.The salt is a typical ionic compound (with certain covalent characteristics), although the small size of the Li + ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.
A Lewis base is also a Brønsted–Lowry base, but a Lewis acid does not need to be a Brønsted–Lowry acid. The classification into hard and soft acids and bases ( HSAB theory ) followed in 1963. The strength of Lewis acid-base interactions, as measured by the standard enthalpy of formation of an adduct can be predicted by the Drago–Wayland ...