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Lithium nitrate is an inorganic compound with the formula LiNO 3. It is the lithium salt of nitric acid (an alkali metal nitrate ). The salt is deliquescent , absorbing water to form the hydrated form, lithium nitrate trihydrate.
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.
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:
The reaction first forms nitryl fluoride FNO 2 that reacts further with the lithium nitrate: [8] BrF 5 + 3 LiNO 3 → 3 LiF + BrONO 2 + O 2 + 2 FNO 2 FNO 2 + LiNO 3 → LiF + N 2 O 5. The compound can also be created in the gas phase by reacting nitrogen dioxide NO 2 or N 2 O 4 with ozone: [13] 2 NO 2 + O 3 → N 2 O 5 + O 2
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.
The reaction forms hydrogen gas and lithium hydroxide. [10] When placed over a flame, lithium compounds give off a striking crimson color, but when the metal burns strongly, the flame becomes a brilliant silver. Lithium will ignite and burn in oxygen when exposed to water or water vapor.