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The hydrated form, lithium nitrate trihydrate, has an extremely high specific heat of fusion, 287 ± 7 J/g, [3] and hence can be used for thermal energy storage at its melt temperature of 303.3 K. [4] Lithium nitrate has been proposed as a medium to store heat collected from the sun for cooking.
Lithium nitrite is the lithium salt of nitrous acid, with formula LiNO 2. This compound is hygroscopic and very soluble in water. It is used as a corrosion inhibitor in mortar. [4] It is also used in the production of explosives, due to its ability to nitrosate ketones under certain conditions. [5]
The presence of alkoxyl or related chelating groups accelerates lithium–halogen exchange. [3] Lithium halogen exchange is typically a fast reaction. It is usually faster than nucleophilic addition and can sometimes exceed the rate of proton transfer. [4] Exchange rates usually follow the trend I > Br > Cl.
A recommended laboratory synthesis entails dehydrating nitric acid (HNO 3) with phosphorus(V) oxide: [11] P 4 O 10 + 12 HNO 3 → 4 H 3 PO 4 + 6 N 2 O 5. Another laboratory process is the reaction of lithium nitrate LiNO 3 and bromine pentafluoride BrF 5, in the ratio exceeding 3:1.
The nitrate ion. Alkali metal nitrates are chemical compounds consisting of an alkali metal (lithium, sodium, potassium, rubidium and caesium) and the nitrate ion. Only two are of major commercial value, the sodium and potassium salts. [1] They are white, water-soluble salts with melting points ranging from 255 °C (LiNO 3) to 414 °C (CsNO
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 nitride is prepared by direct reaction of elemental lithium with nitrogen gas: [2] 6 Li + N 2 → 2 Li 3 N. Instead of burning lithium metal in an atmosphere of nitrogen, a solution of lithium in liquid sodium metal can be treated with N 2. Lithium nitride must be protected from moisture as it reacts violently with water to produce ammonia:
In organometallic chemistry, organolithium reagents are chemical compounds that contain carbon–lithium (C–Li) bonds.These reagents are important in organic synthesis, and are frequently used to transfer the organic group or the lithium atom to the substrates in synthetic steps, through nucleophilic addition or simple deprotonation. [1]