Beryllium hydroxide

Beryllium hydroxide
IUPAC name

Beryllium hydroxide
Other names

Hydrated beryllia
Identifiers
CAS number 13327-32-7 N
PubChem 25879
ChemSpider 24727701 N
EC number 236-368-6
MeSH Beryllium+hydroxide
ChEBI CHEBI:35102 Y
RTECS number DS3150000
Gmelin Reference 1024
Jmol-3D images Image 1
Properties
Molecular formula H2BeO2
Molar mass 43.03 g mol−1
Exact mass 43.017661443 g mol-1
Appearance Vivid white, opaque crystals
Density 1.92 g cm-3[1]
Melting point

1000 °C, 1273 K, 1832 °F
Structure
Molecular shape Linear
Thermochemistry
Std enthalpy of
formation ΔfHo298		 -902.5 kJ mol-1
Specific heat capacity, C 1.443 J K-1
Hazards
Main hazards Carcinogenic
LD50 4 mg kg-1 (intravenous, rat)
Related compounds
Related compounds Aluminium oxide

Magnesium hydroxide
 N (verify) (what is: Y/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
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.[2] 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.[3] This has the zinc hydroxide, Zn(OH)2 structure with tetrahedral beryllium centers.[4]

Reactions

With alkalis it dissolves to form the tetrahydroxidoberyllate(2-) anion.[5] With sodium hydroxide solution:

2NaOH(aq) + Be(OH)2(s) → Na2Be(OH)4(aq)

With acids, beryllium salts are formed.[5] 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:[5]

Be(OH)2 → BeO + H2O

Further heating at higher temperature produces acid insoluble BeO.[5]

References

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
  2. ^ 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 0873352335
  3. ^ Mary Eagleson, 1994, Concise encyclopedia chemistry, Walter de Gruyter, ISBN 3110114518
  4. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 0080379419. 
  5. ^ a b c d Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0123526515