Hydrides sodium hydride

Sodium Hydride. Sodium hydride [7646-69-7] decomposes to its elements without melting, starting at ca 300°C. Decomposition is rapid at 420°C. The dissociation pressure in kPa between 100 and 600°C for the decomposition range 15—90% NaH can be found from... [Pg.297]

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... [Pg.1848]

Metal hydrides Germane, lithium aluminum hydride, potassium hydride, sodium hydride... [Pg.55]

Hydride. Sodium hydride, [CAS 7646-69-7J, NaH. white solid, reactive with water yielding hydrogen gas and NaOH solution, formed by reaction of sodium and hydrogen at about 360°C. Used as a powerful reducing agent. [Pg.1491]

Metal hydrides. Lithium hydride, sodium hydride, potassium hydride and lithium aluminium hydride all react violently with water liberating hydrogen the heat of reaction may cause explosive ignition. Excess metal hydride from a reaction must be destroyed by the careful addition of ethyl acetate or acetone. [Pg.41]

All these are excellent solvents for organic compounds they are purified by initial storage over sodium hydroxide pellets and then heated under reflux with calcium hydride, lithium aluminium hydride, sodium hydride, or sodium, before being fractionally distilled (under reduced pressure if necessary) in an atmosphere of nitrogen. [Pg.406]

M-H (metal hydride) Sodium hydride Potassium hydride Strong, not nucleophilic base Deprotonation of weak organic acids with acidities as high as pKa 25... [Pg.144]

Ignition or explosive reaction with metals (e.g., aluminum, antimony powder, bismuth powder, brass, calcium powder, copper, germanium, iron, manganese, potassium, tin, vanadium powder). Reaction with some metals requires moist CI2 or heat. Ignites with diethyl zinc (on contact), polyisobutylene (at 130°), metal acetylides, metal carbides, metal hydrides (e.g., potassium hydride, sodium hydride, copper hydride), metal phosphides (e.g., copper(II) phosphide), methane + oxygen, hydrazine, hydroxylamine, calcium nitride, nonmetals (e.g., boron, active carbon, silicon, phosphoms), nonmetal hydrides (e.g., arsine, phosphine, silane), steel (above 200° or as low as 50° when impurities are present), sulfides (e.g., arsenic disulfide, boron trisulfide, mercuric sulfide), trialkyl boranes. [Pg.315]

ALKYLATION Benzyltiiethylammonium chloride. n-Butyl mercaptan. Dialkylcar-bonium fluoroborates. Diethoxycarboni-um fluoroborate. Dimethylcopperlithium. Ethyl vinyl ether. Dimethylformamidc dimethyl acetal. Dimethyl sulflde. Dimeth-ylsulfonium methylide. Ethyl chlorofor-mate. Hexamethylphosphoric tiiamide. Lithium diisopropylamide. Lithium N-iso-propylcyclohexylamide. O-Methyldiben-zofuranium fluoroborate. Methyl fluoro-sulfonatc. Naththalene-Sodium. Palladi-um(II) chloride. 1,2,2,6,6-PentamelhyI-pipetidine. Potassium hydroxide. Silver oxide. Sodium bis-2-mcthoxyethoxyaIu-minum hydride. Sodium hydride. Thai-lous ethoxide. [Pg.581]

Other bases may be employed, e.g. lithium hydride, sodium hydride, sodium amide or sodium in ethylene glycol with sodium in ethylene glycol, the reaction is called the Bamford-Stevens reaction. Aldehyde tosylhydrazones (200) do not form dianions with organolithiums, but the reagent adds to the carbon-nitrogen double bond to give the dilithium derivative (201) which decomposes to the organolithium compound (202). [Pg.218]

Besides the intramolecular cyclization of co-haloalkyl-substituted compounds, a variety of five- and six-membered 2-oxo-1,2-oxaphosphacyclanes can be obtained via thermal cyclization of co-hydroxyalkylphosphonates (preformed or obtained in situ) and related compounds [66-73], As the reaction proceeds through intramolecular transesterification requiring a prolonged heating, use of bases such as lithium hydride, sodium hydride, sodium alcoholate, etc. accelerates the reaction and increases the yield of heterocycles 62 (Scheme 35) [54],... [Pg.127]

INORGANIC PREPARATION OF OTHER HYDRIDES. Sodium hydride is one of the cheapest raw materials for the production of other hydrides. Sodium borohydride is prepared commercially by the reaction ... [Pg.111]

Hydrides commonly used in laboratories are lithium aluminum hydride, potassium hydride, sodium hydride, sodium borohydride, and calcium hydride. The following methods for their disposal demonstrate that the reactivity of metal hydrides varies considerably. Most hydrides can be decomposed safely by one of the four methods, but the properties of a given hydride must be well understood in order to select the most appropriate method. (CAUTION Most of the methods described below produce hydrogen gas, which can present an explosion hazard. The reaction shouid be carried out in a hood, behind a shield, and with proper safeguards to avoid exposure of the effluent gas to spark or flame. Any stirring device must be spark-proof.)... [Pg.165]

Substance Potassium hydride Sodium hydride CAS 7693-26-7 CAS 7646-69-7 (Commonly handled as dispersions in mineral oil)... [Pg.384]

Metal hydrides Sodium hydride, lithium tiluminum hydride... [Pg.259]

Platinum-carbon/sodium hydride Sodium hydride as hydrogen generator Reduction of active hydrogen compounds Sec. alcohols from ketones Replacement of chlorine by hydrogen... [Pg.337]

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