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Beryllium hydroxide






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From Wikipedia, the free encyclopedia
  

Beryllium hydroxide
Names
IUPAC name

Beryllium hydroxide

Other names
  • Beryllic acid
  • Hydrated beryllia
    • Identifiers

    CAS Number

    3D model (JSmol)
    ChEBI
    ChemSpider
    ECHA InfoCard 100.033.048 Edit this at Wikidata
    EC Number
    • 236-368-6

    Gmelin Reference

    		 1024
    MeSH Beryllium+hydroxide

    PubChem CID
    RTECS number
    • DS3150000
    UNII

    CompTox Dashboard (EPA)

    • InChI=1S/Be.2H2O/h;2*1H2/q+2;;/p-2 checkY

      Key: WPJWIROQQFWMMK-UHFFFAOYSA-L checkY

    • InChI=1/Be.2H2O/h;2*1H2/q+2;;/p-2

      Key: WPJWIROQQFWMMK-NUQVWONBAB

    • O[Be]O

    Properties

    Chemical formula

    		 BeH2O2
    Molar mass 43.026 g·mol−1
    Appearance Vivid white, opaque crystals
    Density 1.92 g cm−3[1]
    Melting point (decomposes)

    Solubility in water

    		 0.0000023965 g/L

    Solubility product (Ksp)

    		6.92×10−22[2]
    Acidity (pKa) 3.7[3]
    Structure

    Molecular shape

    		 Linear
    Thermochemistry

    Heat capacity (C)

    		 1.443 J K−1

    Std molar
    entropy     (S⦵298)

    		 47 J·mol−1·K−1[4]

    Std enthalpy of
    formation     (ΔfH⦵298)

    		 -904 kJ mol−1[4]

    Gibbs free energy (ΔfG⦵)

    		 -818 kJ/mol
    Hazards
    Occupational safety and health (OHS/OSH):

    Main hazards

    		 Carcinogenic
    GHS labelling:

    Pictograms

    		 GHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard[5]

    Signal word

    		 Danger
    NFPA 704 (fire diamond)
    NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
    4
    0
    0
    Lethal dose or concentration (LD, LC):

    LD50 (median dose)

    		 4 mg kg−1 (intravenous, rat)
    NIOSH (US health exposure limits):

    PEL (Permissible)

    		 TWA 0.002 mg/m3
    C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)[6]

    REL (Recommended)

    		 Ca C 0.0005 mg/m3 (as Be)[6]

    IDLH (Immediate danger)

    		 Ca [4 mg/m3 (as Be)][6]
    Related compounds

    Related compounds

    		 Aluminium oxide

    Magnesium hydroxide

    Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

    ☒N verify (what is checkY☒N ?)

    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.[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[edit]

    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[edit]

    1. ^ 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 978-1138561632.
  • ^ Handbook of Chemistry and Physics. Cleveland, Ohio: Chemical Rubber Publishing Company. 1951. pp. 1636–1637.
  • ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN 978-0-618-94690-7.
  • ^ "Beryllium Hydroxide". American Elements. Retrieved 5 July 2023.
  • ^ 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

    • Retrieved from "https://en.wikipedia.org/w/index.php?title=Beryllium_hydroxide&oldid=1226643225"
    Categories: 
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     ●Beryllium compounds
     ●Hydroxides
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