The Info List - Beryllium Hydroxide

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Magnesium hydroxide

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

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Infobox references

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[edit] With alkalis it dissolves to form the tetrahydroxidoberyllate(2-) anion.[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

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[edit]

^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8 ^ Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN 0-618-94690-X.  ^ Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN 0-618-94690-X.  ^ 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 0-08-037941-9.  ^ a b c d Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5

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Be(BH4)2 BeBr2 BeCO3 BeCl2 BeF2 BeH BeH2 BeI2 Be(N3)2 Be(NO3)2 BeO Be(OH)2 BeS BeSO3 BeSO4 BeTe Be2C Be3N2

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LiOH Be(OH)2

B C NH3.H2O O F Ne

NaOH Mg(OH)2

Al(OH)3 Si P S Cl Ar

KOH Ca(OH)2 Sc(OH)3 Ti V Cr(OH)2 Cr(OH)3 Mn(OH)2 Fe(OH)2 Fe(OH)3 Co(OH)2 Ni(OH)2 CuOH Cu(OH)2 Zn(OH)2 Ga(OH)3 Ge(OH)2 As Se Br Kr

RbOH Sr(OH)2 Y(OH)3 Zr(OH)4 Nb Mo Tc Ru Rh Pd AgOH Cd(OH)2 In(OH)3 Sn(OH)2 Sn(OH)4 Sb(OH)3 Te I Xe

CsOH Ba(OH)2 * Hf Ta W Re Os Ir Pt Au(OH)3 Hg(OH)2 TlOH Tl(OH)3 Pb(OH)2 Pb(OH)4 Bi(OH)3 Po At Rn

Fr Ra ** Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og

* La(OH)3 Ce(OH)3 Pr(OH)3 Nd(OH)3 Pm(OH)3 Sm(OH)3 Eu(OH)3 Gd(OH)3 Tb(OH)3 Dy(OH)3 Ho(OH)3 Er(OH)3 Tm(OH)3 Yb(OH)3 Lu(OH)3

** Ac Th(OH)4 Pa UO2(OH)2 Np Pu Am Cm(OH)3 Bk Cf Es