Beryllium hydroxide
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Template:Chembox image cellTemplate:Chembox AllOtherNamesTemplate:Chembox headerbarTemplate:Chembox IndexlistTemplate:Chembox JmolTemplate:Chembox ChEMBLTemplate:Chembox ECHATemplate:Chembox E numberTemplate:Chembox IUPHAR ligandTemplate:Chembox UNIITemplate:Chembox CompToxTemplate:Chembox headerbarTemplate:Chembox SolubilityInWaterTemplate:Chembox headerbarTemplate:Chembox headerbarTemplate:Chembox DeltaGfreeTemplate:Chembox headerbarTemplate:Chembox OHS (set)Template:Chembox GHS (set)Template:Chembox Lethal amounts (set)Template:Chembox setHeaderTemplate:Chembox setDatarowTemplate:Chembox setDatarowTemplate:Chembox setDatarowTemplate:Chembox headerbarTemplate:Chembox Datapage checkTemplate:Chembox Footer| Template:Longitem | Template:Unbulleted list |
| ChEBI | Template:Unbulleted list |
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| EC Number | Template:Unbulleted list |
| Template:Longitem | 1024 |
| KEGG | Template:Unbulleted list |
| MeSH | Beryllium+hydroxide |
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| Template:Longitem | Template:Chembox Elements/molecular formula |
| Molar mass | Template:Chem molar mass |
| Appearance | Vivid white, opaque crystals |
| Density | 1.92 g cm−3[1] |
| Melting point | Template:Chembox CalcTemperatures |
| Template:Longitem | 6.92Template:E[2] |
| Acidity (pKa) | 3.7[3] |
| Template:Longitem | Linear |
| Template:Longitem | 1.443 J K−1 |
| Template:Longitem | 47 J·mol−1·K−1[4] |
| Template:Longitem | −904 kJ mol−1[4] |
| NFPA 704 (fire diamond) | Template:NFPA 704 diamond |
| Template:Longitem | Aluminium oxide |
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Beryllium hydroxide, Be(OH)2, is an amphoteric hydroxide, dissolving in both acids and alkalis. Industrially, it is produced as a by-product in the extraction of beryllium metal from the ores beryl and bertrandite.[7] The natural pure beryllium hydroxide is rare (in form of the mineral behoite, orthorhombic) or very rare (clinobehoite, monoclinic).[8][9] When alkali is added to beryllium salt solutions the α-form (a gel) is formed. If this left to stand or boiled, the rhombic β-form precipitates.[10] This has the same structure as zinc hydroxide, Zn(OH)2, with tetrahedral beryllium centers.[11]
Reactions
Beryllium hydroxide is difficult to dissolve in water. With alkalis it dissolves to form the tetrahydroxoberyllate (also known as tetrahydroxidoberyllate) anion, [Be(OH)4]2−.[12] With sodium hydroxide solution:
- 2 NaOH(aq) + Be(OH)2(s) → Na2[Be(OH)4](aq)
With acids, beryllium salts are formed.[12] For example, with sulfuric acid, H2SO4, beryllium sulfate is formed:
- Be(OH)2 + H2SO4 → BeSO4 + 2 H2O
Beryllium hydroxide dehydrates at 400 °C to form the soluble white powder, beryllium oxide:[12]
- Be(OH)2 → BeO + H2O
Further heating at higher temperature produces acid insoluble BeO.[12]
References
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- ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, Template:ISBN
- ↑ Script error: No such module "citation/CS1".
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- ↑ a b Script error: No such module "citation/CS1".
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- ↑ a b c Script error: No such module "citation/CS1".
- ↑ Jessica Elzea Kogel, Nikhil C. Trivedi, James M. Barker and Stanley T. Krukowski, 2006, Industrial Minerals & Rocks: Commodities, Markets, and Uses, 7th edition, SME, Template:ISBN
- ↑ Mindat, http://www.mindat.org/min-603.html
- ↑ Mindat, http://www.mindat.org/min-1066.html
- ↑ Mary Eagleson, 1994, Concise encyclopedia chemistry, Walter de Gruyter, Template:ISBN
- ↑ Script error: No such module "citation/CS1".
- ↑ a b c d Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier Template:ISBN
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