Beryllium formate, basic

Beryllium diacetate tetraisobuty-rate, basic, properties of, 3 7 Beryllium formate, basic, properties and structure of, 3 7, 8 Beryllium isobutyrate, basic, properties and structure of, 3 7, 8 Beryllium isovalerate, basic, properties of, 3 7... 

For the preparation of basic beryllium formate and basic beryllium propionate, see the literature cited under II also H, Hendus and H. D. Hardt, Z. anorg. allg. Chem. 277, 127 (1954). 

Basic Beryllium Formate, Be40(CH0,)e-— This compound was first prepared by Lacombe (1902 3) by the action of anhydrous formic acid in excess on the carbonate and sublimation of the product under diminished pressure Parsons (,1904 5) attempted to use it for atomic weight determination, but found its sublimation and purification too difficult, as even under much diminished pressure it was partly decomposed. 

Even when modifiers are not necessary for cement formation, they can lead to improved cement properties. Kingery (1950b) also examined this effect. He found that optimum bonding was achieved with cations that had small ionic radii and were amphoteric or weakly basic, such as beryllium, aluminium, magnesium and iron. By contrast, cations that were highly basic and had large ionic radii, for example calcium, thorium and barium, had a detrimental effect on bonding. 

The addition of soluble carbonates to beryllium salt solutions gives only basic carbonates. Beryllium salt solutions also have the property of dissolving additional amounts of the oxide or hydroxide. This behavior is attributable to the formation of complex species with Be—OH—Be or Be—O—Be bridges. The rapidly established equilibria involved in the hydrolysis of the [Be(H20)4]2+ ion are very complicated and depend on the anion, the concentration, the temperature, and the pH. The main species, which will achieve four-coordination by additional water molecules, are considered to be Be2(OH)3+ and Be3(OH)3+ (probably cyclic). 

Beryllium Chromate, BeCrO4.H20, and the basic eonqrouud, EeCr04.6Ee(0TI).2, have been described by Glassmaun, whose results, however, have not been confirmed by subsequent workers. It appears to be established that a solution of chromic acid absoi bs beryllium hydroxide in the exact ratio of iBe(OH)., K rOj, w hich points to the formation of the neutral chromate. When solutions of beryllium salts are treated with equivalent quantities of chromates, the prccij titates at first formed redissolve but if the chromate is added in excess, yellow precipitates of strongly basic beryllium chromates of uncertain composition are obtained. 

Action of Organic Acid on Beryllium Carbonate or Basic Carbonate. This method is similar in all respects to the above procedure. While it has been used most extensively for only the simpler members of the series, there is no apparent reason why it should not be equally effective for the preparation of other members as well. The procedure is one of the few claimed to give the basic formate. Directions given for the preparation of the basic acetate (synthesis 3) and basic propionate (synthesis 3) represent modifications of this general procedure. 

During the processes of weathering and formation of sediments, beryllium closely follows the course of aluminum, being enriched, along with aluminum, in clays, bauxites, recent deep sea deposits, and other hydrolyzate sediments. This is due to the similarity of the basic properties and solubilities of these metals. Though radii and charges of the Be and ions differ, their ionic potentials are rather simi-... 

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