Beryllium hydroxide
Names | |
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IUPAC name
Beryllium hydroxide
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Other names
Hydrated beryllia
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Identifiers | |
3D model (JSmol)
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ChEBI | |
ChemSpider | |
ECHA InfoCard | 100.033.048 |
EC Number |
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1024 | |
MeSH | Beryllium+hydroxide |
PubChem CID
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RTECS number |
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
BeH2O2 | |
Molar mass | 43.026 g·mol−1 |
Appearance | Vivid white, opaque crystals |
Density | 1.92 g cm−3[1] |
Melting point | (decomposes) |
0.0000023965 g/L | |
Solubility product (Ksp)
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6.92×10−22[2] |
Structure | |
Linear | |
Thermochemistry | |
Heat capacity (C)
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1.443 J K−1 |
Std molar
entropy (S |
47 J·mol−1·K−1[3] |
Std enthalpy of
formation (ΔfH⦵298) |
-904 kJ mol−1[3] |
Gibbs free energy (ΔfG˚)
|
-818 kJ/mol |
Hazards | |
Main hazards | Carcinogenic |
GHS labelling: | |
Signal word
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Danger |
NFPA 704 (fire diamond) |
4
0
0 |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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4 mg kg−1 (intravenous, rat) |
NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 0.002 mg/m3 C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)[4] |
REL (Recommended)
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Ca C 0.0005 mg/m3 (as Be)[4] |
IDLH (Immediate danger)
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Ca [4 mg/m3 (as Be)][4] |
Related compounds | |
Related compounds
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Aluminium oxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
what is ?) | (|
Infobox references | |
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.[5] The natural pure beryllium hydroxide is rare (in form of the mineral behoite, orthorhombic) or very rare (clinobehoite, monoclinic).[6][7] 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.[8] This has the same structure as zinc hydroxide, Zn(OH)2, with tetrahedral beryllium centers.[9]
Reactions[]
Beryllium hydroxide is difficult to dissolve in water. With alkalis it dissolves to form the tetrahydroxoberyllate/tetrahydroxidoberyllate anion, [Be(OH)4]2−.[10] With sodium hydroxide solution:
- 2NaOH(aq) + Be(OH)2(s) → Na2Be(OH)4(aq)
With acids, beryllium salts are formed.[10] For example, with sulfuric acid, H2SO4, beryllium sulfate is formed:
- Be(OH)2 + H2SO4 → BeSO4 + 2H2O
Beryllium hydroxide dehydrates at 400 °C to form the soluble white powder, beryllium oxide:[10]
- Be(OH)2 → BeO + H2O
Further heating at higher temperature produces acid insoluble BeO.[10]
References[]
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 4–47. ISBN 1138561630.
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN 978-0-618-94690-7.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0054". National Institute for Occupational Safety and Health (NIOSH).
- ^ Jessica Elzea Kogel, Nikhil C. Trivedi, James M. Barker and Stanley T. Krukowski, 2006, Industrial Minerals & Rocks: Commodities, Markets, and Uses, 7th edition, SME, ISBN 0-87335-233-5
- ^ 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, ISBN 3-11-011451-8
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ a b c d Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
- Amphoteric compounds
- Beryllium compounds
- Hydroxides