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| Verifiedfields = changed
| Verifiedfields = changed
| Watchedfields = changed
| Watchedfields = changed
| verifiedrevid = 399538974
| verifiedrevid =
| ImageFile1 = BeOH.png
| IUPACName = Beryllium hydroxide
| IUPACName = Beryllium hydroxide
| OtherNames = Hydrated beryllia
| OtherNames = Hydrated beryllia
| Section1 = {{Chembox Identifiers
|Section1={{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|??}}
| CASNo_Ref = {{cascite|correct|}}
| CASNo = <!-- blanked - oldvalue: 13327-32-7 -->
| CASNo = 13327-32-7
| UNII_Ref = {{fdacite|correct|FDA}}
| PubChem = 25879
| UNII = 2X0LRF1T6Q
| PubChem_Ref = {{Pubchemcite|correct|pubchem}}
| ChemSpiderID = 24110
| =
| ChemSpiderID = 24110
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| EINECS = 236-368-6
| MeSHName = Beryllium+hydroxide
|
MeSHName = Beryllium+hydroxide
| ChEBI_Ref = {{ebicite|changed|EBI}}
| ChEBI_Ref = {{ebicite||EBI}}
| ChEBI = 35102
| ChEBI = 35102
| RTECS = DS3150000
| RTECS = DS3150000
| Gmelin = 1024
| Gmelin = 1024
| SMILES = O[Be]O
| SMILES = O[Be]O
| StdInChI = 1S/Be.2H2O/h;2*1H2/q+2;;/p-2
| StdInChI = 1S/Be.2H2O/h;2*1H2/q+2;;/p-2
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| InChI = 1/Be.2H2O/h;2*1H2/q+2;;/p-2
| InChI = 1/Be.2H2O/h;2*1H2/q+2;;/p-2
| StdInChIKey = WPJWIROQQFWMMK-UHFFFAOYSA-L
| StdInChIKey = WPJWIROQQFWMMK-UHFFFAOYSA-L
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| InChIKey = WPJWIROQQFWMMK-NUQVWONBAB
| InChIKey = WPJWIROQQFWMMK-NUQVWONBAB
}}
}}
| Section2 = {{Chembox Properties
|Section2={{Chembox Properties
| H = 2
| H = 2
⚫
| Appearance = Vivid white, opaque crystals
⚫
| Be = 1
⚫
| Density = 1.92 g cm<sup></sup><ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN</ref>
⚫
| O = 2
⚫
| MeltingPtC =
| ExactMass = 43.017661443 g mol<sup>-1</sup>
| MeltingPt_notes = (decomposes)
⚫
| Appearance = Vivid white, opaque crystals
| pKa = 3.7<ref>{{cite book |title=Handbook of Chemistry and Physics |date=1951 |publisher=Chemical Rubber Publishing Company |location=Cleveland, Ohio |pages=1636–1637}}</ref>
⚫
| Density = 1.92 g cm<sup>-3</sup><ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref>
| Solubility = 0.0000023965 g/L
⚫
| MeltingPtC = 1000
| SolubilityProduct = 6.92{{e|&minus;22}}<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=4–47|edition=99 |language=English}}</ref>
| Melting_notes decomposes
}}
}}
| Section3 = {{Chembox Structure
|Section3={{Chembox Structure
| MolShape = Linear
| MolShape = Linear
}}
}}
| Section4 = {{Chembox Thermochemistry
|Section4={{Chembox Thermochemistry
| DeltaHf = -904 kJ mol<sup>−1</sup><ref name=CP6>{{cite book |author= Zumdahl, Steven S.|title= Chemical Principles 6th Ed. |publisher= Houghton Mifflin Company |year= 2009 |isbn= 978-0-618-94690-7}}</ref>
⚫
| DeltaHf = -902.5 kJ mol<sup>-1</sup>
| DeltaGf = -818 kJ/mol
| HeatCapacity = 1.443 J K<sup>-1</sup>
| Entropy = 47 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=CP6/>
⚫
}}
⚫
| = . <sup></sup>
| Section5 = {{Chembox Hazards
⚫
| MainHazards = Carcinogenic
⚫
| LD50 = 4 mg kg<sup>-1</sup> (intravenous, rat)
}}
}}
| Section6 = {{Chembox Related
|={{Chembox
⚫
| MainHazards = Carcinogenic
⚫
| OtherCpds = [[Aluminium oxide]]<br />
⚫
| =
⚫
| =
| NFPA-R = 0
| GHSPictograms = {{GHS06}}{{GHS08}}{{GHS09}}<ref>{{cite web |title=Beryllium Hydroxide |url=https://www.americanelements.com/beryllium-hydroxide-13327-32-7 |website=American Elements |access-date=5 July 2023}}</ref>
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|}}
| PPhrases = {{P-phrases|}}
⚫
| LD50 = 4 mg kg<sup></sup> (intravenous, rat)
| REL = Ca C 0.0005 mg/m<sup>3</sup> (as Be)<ref name=PGCH>{{PGCH|0054}}</ref>
| PEL = TWA 0.002 mg/m<sup>3</sup><br>C 0.005 mg/m<sup>3</sup> (30 minutes), with a maximum peak of 0.025 mg/m<sup>3</sup> (as Be)<ref name=PGCH/>
| IDLH = Ca [4 mg/m<sup>3</sup> (as Be)]<ref name=PGCH/>
⚫
}}
|Section6={{Chembox Related
⚫
| = [[Aluminium oxide]]<br>
[[Magnesium hydroxide]]
[[Magnesium hydroxide]]
}}
}}
}}
}}


'''Beryllium hydroxide''', Be(OH)<sub>2</sub> is an [[amphoteric]] [[hydroxide]], dissolving in both [[acids]] and [[alkali]]s. Industrially it is produced as a by-product in the extraction of beryllium metal from the ores, [[beryl]] and [[bertrandite]].<ref>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</ref> 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.<ref name = "Eagleson">Mary Eagleson, 1994, Concise encyclopedia chemistry, Walter de Gruyter, ISBN 3110114518</ref> This has the [[zinc hydroxide]], Zn(OH)<sub>2</sub> structure with tetrahedral beryllium centers.<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref>
'''Beryllium hydroxide''', Be(OH)<sub>2</sub> is an [[amphoteric]] [[hydroxide]], dissolving in both [[]] and [[alkali]]s. Industrially it is produced as a by-product in the extraction of beryllium metal from the ores [[beryl]] and [[bertrandite]].<ref>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 </ref> 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.<ref name="Eagleson">Mary Eagleson, 1994, Concise encyclopedia chemistry, Walter de Gruyter, ISBN</ref> This has the [[zinc hydroxide]], Zn(OH)<sub>2</sub> with tetrahedral beryllium centers.<ref name="Greenwood">{{Greenwood&}}</ref>


==Reactions==
==Reactions==
With alkalis it dissolves to form the tetrahydroxidoberyllate(2-) anion.<ref name = "Wiberg&Holleman">Egon Wiberg, Arnold Frederick Holleman (2001) ''Inorganic Chemistry'', Elsevier ISBN 0123526515</ref> With [[sodium hydroxide]] solution:
With alkalis it dissolves to form the () anion.<ref name="Wiberg&Holleman">Egon Wiberg, Arnold Frederick Holleman (2001) ''Inorganic Chemistry'', Elsevier ISBN</ref> With [[sodium hydroxide]] solution:
⚫
:(aq) + Be(OH)<sub>2</sub>(s) → Na<sub>2</sub>Be(OH)<sub>4</sub>(aq)


⚫
With acids, beryllium salts are formed.<ref name="Wiberg&Holleman"/> For example, with [[sulfuric acid]], H<sub>2</sub>SO<sub>4</sub>, [[beryllium sulfate]] is formed:
⚫
:2NaOH(aq) + Be(OH)<sub>2</sub>(s) → Na<sub>2</sub>Be(OH)<sub>4</sub>(aq)
⚫
:Be(OH)<sub>2</sub> + H<sub>2</sub>SO<sub>4</sub> → BeSO<sub>4</sub> + <sub>2</sub>O


⚫
Beryllium hydroxide dehydrates at 400°C to form the soluble white powder, [[beryllium oxide]]:<ref name="Wiberg&Holleman"/>
⚫
With acids, beryllium salts are formed.<ref name = "Wiberg&Holleman"/> For example, with [[sulfuric acid]], H<sub>2</sub>SO<sub>4</sub>, [[beryllium sulfate]] is formed:

⚫
:Be(OH)<sub>2</sub> + H<sub>2</sub>SO<sub>4</sub> → BeSO<sub>4</sub> + 2H<sub>2</sub>O

⚫
Beryllium hydroxide dehydrates at 400 °C to form the soluble white powder, [[beryllium oxide]]:<ref name = "Wiberg&Holleman"/>
:Be(OH)<sub>2</sub> → BeO + H<sub>2</sub>O
:Be(OH)<sub>2</sub> → BeO + H<sub>2</sub>O
Further heating at higher temperature produces acid insoluble BeO.<ref name = "Wiberg&Holleman"/>
Further heating at higher temperature produces acid insoluble BeO.<ref name="Wiberg&Holleman"/>


==References==
==References==
{{reflist}}
{{}}


{{Beryllium compounds}}
{{Beryllium compounds}}
{{Hydroxides}}
{{Hydroxides}}


[[Category:Amphoteric compounds]]
[[Category:Beryllium compounds]]
[[Category:Beryllium compounds]]
[[Category:Hydroxides]]
[[Category:Hydroxides]]


{{inorganic-compound-stub}}

[[ar:هيدروكسيد البيريليوم]]
[[nl:Berylliumhydroxide]]
[[ja:水酸化ベリリウム]]
[[pl:Wodorotlenek berylu]]
[[ru:Гидроксид бериллия]]
[[zh:氫氧化鈹]]
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