Beryllium nitrate

Beryllium Nitrate. BeryUium nitrate tetrahydrate [13516-48-0], Be(N02)2 4H2O, is prepared by crystallization from a solution of beryUium hydroxide or beryllium oxide carbonate in a slight excess of dilute nitric acid. After dissolution is complete, the solution is poured into plastic bags and cooled to room temperature. The crystallization is started by seeding. Crystallization from more concentrated acids yields crystals with less water of hydration. On heating above 100°C, beryllium nitrate decomposes with simultaneous loss of water and oxides of nitrogen. Decomposition is complete above 250°C. 

Chemical Designations - Synonyms Beryllium Nitrate Trihydrate Chemical Formula Be(N03)j.3H20. 

Nickel, Copper and Beryllium nitrates Calcium, Magnesium, Strontium and Barium chlorides (5,7]... 

Beryllium iodide, 3 663 Beryllium nitrate, 3 664-665 Beryllium nitrate tetrahydrate, 3 664-665 Beryllium nitride, 3 665 Beryllium oxalate, 3 665 Beryllium oxalate trihydrate, 3 665 Beryllium oxide, 3 665-666 5 582 21 491 ceramic insulator, 5 593 energy gap at room temperature,... 

Synonyms/compounds Glucinium beryllium oxide beryllium chloride beryllium fluoride beryllium hydroxide beryllium phosphate beryllium nitrate beryllium sulfate beryllium carbonate... 

Beryllium oxide is obtained by thermal dissociation of beryllium nitrate or hydroxide ... 

PROP Pure beryllium is a hard, brittle, silvery metal. Mp 1278°, bp 2970°, d 1.85. Beryllium oxide white powder. Mp 2530°, d 3.0. Beryllium chloride white to faintly yellow powder, deliquescent. Mp 399°, bp 482°. Beryllium fluoride glassy, hygroscopic solid. Mp 545°, d 2.0. Beryllium nitrate white to slightly yellow crystals. Mp 60°). Beryllium sulfate Mp 550°. 

Pure beryllium hydroxide, freshly prepared from 12 g. (0.06 mol) of beryllium nitrate 4-hydrate, is dissolved by... 

The paper discusses two types of reaction involving metal complexes, and it is postulated that each proceeds by an initial free-radical step. In reactions between metal carbonyls and N2O4—NO2 mixtures, the nature of the product depends upon the phase in which the reaction is carried out. In the liquid phase, where the predominant equilibrium is N204 N0+ + NO3-, metal nitrates or carbonyl nitrates are formed in the gas phase, where the equilibrium is N2O4 2NO2/ nitrites or their derivatives are produced. Reactions of Mn2(CO) o Fe(CO)5, Co2(CO)3, and Ni(CO)4 are discussed. Anhydrous metal nitrates in which the nitrate group is covalently bonded to the metal have enhanced reactivity. This is believed to result from the dissociation M—O—N02 M—O + NO2 This can explain the solution properties of beryllium nitrates, and the vigorous (even explosive) reaction of anhydrous copper nitrate with diethyl ether. 

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