Beryllium complexes hydrates

Beryllium complexes, 3 amines, 7 anionic, 10 hydrates, 6 phthalocyanine, 59 poly carboxylic acid, 33 Schiff bases, 28 Beryllium dichloride ether complexes, 8 Beryllium difluoride ammine complexes, 7 Beryllium dihalides sulfide complexes, 10 Beryllium halides amine complexes, 8 ammonia complexes, 7 carbonyl complexes, 9 Beryllium nitrate basic, 32... 

The study of coordination compounds of the lanthanides dates in any practical sense from around 1950, the period when ion-exchange methods were successfully applied to the problem of the separation of the individual lanthanides,131-133 a problem which had existed since 1794 when J. Gadolin prepared mixed rare earths from gadolinite, a lanthanide iron beryllium silicate. Until 1950, separation of the pure lanthanides had depended on tedious and inefficient multiple crystallizations or precipitations, which effectively prevented research on the chemical properties of the individual elements through lack of availability. However, well before 1950, many principal features of lanthanide chemistry were clearly recognized, such as the predominant trivalent state with some examples of divalency and tetravalency, ready formation of hydrated ions and their oxy salts, formation of complex halides,134 and the line-like nature of lanthanide spectra.135... 

Beryllium cliloride has a hydrate BeCl2.4H20 and an unusually stable tetra-ammine Be (N 113)4012. The formation of 4-co-ordinate complexes by Be is very common nearly all its inorganic salts have tetrahydrates containing... 

The structure of bis(salicylaldoxime)beryllium has been proposed as being trans octahedral by comparison of the space group and unit cell volume with those of related transition metal complexes it is presumably a (hydrate if it is indeed octahedral in geometry. Stability constants have been reported for a range of beryllium j3-ketoamines derived from both salicylaldehyde and acetylacetone precursors. They show strong complexes which are stable to hydrolysis under the conditions used. ... 

If it is necessary to extract the rare metal from an acid or alkaline leach liquor, or similar solution, a resin should be selected which is known to be stable in the leaching reagent. For extraction of the rare metal ion itself, the resin would normally be of the cation-exchange type, unless the rare metal ion could be converted to an anionic complex. However, the possibility of designing a process in which the impurities are absorbed by the resin and the rare metal remains unextracted, should not be neglected. An example of this type has been developed by Ayres,i > in which iron, titanium, lanthanum and beryllium impurities are extracted from a zirconium nitrate solution by operation at a pH where the zirconium is converted to a non-ionic hydrated oxide sol. 

---