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Revision as of 13:09, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,084 edits Saving copy of the {{chembox}} taken from revid 472693105 of page Beryllium_fluoride for the Chem/Drugbox validation project (updated: '').		Latest revision as of 22:08, 26 September 2024 edit Smokefoot (talk | contribs)Autopatrolled, Extended confirmed users, Pending changes reviewers, Rollbackers75,064 edits →Structure and bonding: Gaseous vs Gas
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	{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}}
	{{chembox		{{chembox
			| Watchedfields = changed
	| verifiedrevid = 451031801
			| verifiedrevid = 476998806
	| ImageFile = Beryllium-fluoride-3D-vdW.png
			| ImageFile1 = BeF2str.PNG
	| ImageSize = 200px
			| ImageSize1 = 240px
	| ImageName = beryllium fluoride in gas phase
			| ImageFile2 =
	| IUPACName = Berylium fluoride
			| ImageSize2 = 240px
	| OtherNames =
			| ImageFile3 = Beryllium fluoride.JPG
	| Section1 = {{Chembox Identifiers
			| ImageSize3 = 240px
			| IUPACName = Beryllium fluoride
			| OtherNames = Beryllium difluoride<br /> Difluoroberyllane
			| Section1 = {{Chembox Identifiers
	| Abbreviations =		| Abbreviations =
	| ChEBI_Ref = {{ebicite|correct|EBI}}		| ChEBI_Ref = {{ebicite|correct|EBI}}
	| ChEBI = 49499		| ChEBI = 49499
	| SMILES = ..		| SMILES = ..
			| SMILES_Comment = solid ionic form
			| SMILES1 = FF
			| SMILES1_Comment = solid covalent form
			| SMILES2 = ==
			| SMILES2_Comment = gas form
	| InChIKey = JZKFIPKXQBZXMW-NUQVWONBAD		| InChIKey = JZKFIPKXQBZXMW-NUQVWONBAD
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
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	| StdInChIKey = JZKFIPKXQBZXMW-UHFFFAOYSA-L		| StdInChIKey = JZKFIPKXQBZXMW-UHFFFAOYSA-L
	| CASNo = 7787-49-7		| CASNo = 7787-49-7
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
			| UNII_Ref = {{fdacite|correct|FDA}}
			| UNII = 499FU9DQ5C
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID=22992		| ChemSpiderID=22992
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	| RTECS = DS2800000		| RTECS = DS2800000
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = BeF<sub>2</sub>		| Formula = BeF<sub>2</sub>
	| MolarMass = 47.01 g/mol <br> ]		| MolarMass = 47.01 g/mol <br /> ]
	| Appearance = colorless lumps		| Appearance = colorless, glassy lumps
	| Density = 1.986 g/cm<sup>3</sup>		| Density = 1.986 g/cm<sup>3</sup>
	| MeltingPtC = 554		| MeltingPtC = 554
			| MeltingPt_ref =<ref>{{cite web |title=Beryllium Fluoride |url=https://www.americanelements.com/beryllium-fluoride-7787-49-7 |website=American Elements |access-date=10 July 2023}}</ref>
	| Melting_notes =
	| BoilingPtC = 1169		| BoilingPtC = 1169
	| Boiling_notes =<ref>{{RubberBible87th}}</ref>		| BoilingPt_ref =<ref>{{RubberBible87th}}</ref>
	| Solubility = very soluble		| Solubility = very soluble
	| SolubleOther = sparingly soluble in ]		| SolubleOther = sparingly soluble in ]
	| Solvent =		| Solvent =
	| pKa =		| pKa =
	| pKb = }}		| pKb = }}
	| Section4 = {{Chembox Thermochemistry		| Section4 = {{Chembox Thermochemistry
	| DeltaHf = -21.84 kJ/g		| DeltaHf = -1028.2 kJ/g or -1010 kJ/mol
	| DeltaHc =		| DeltaHc =
			| DeltaGf = -941 kJ/mol
	| Entropy =
	| HeatCapacity = 1.102 J/K		| Entropy = 45 J/mol K
			| HeatCapacity = 1.102 J/K or 59 J/mol K
	}}		}}
	| Section3 = {{Chembox Structure		| Section3 = {{Chembox Structure
	| MolShape = ]		| MolShape = ]
			| CrystalStruct = Trigonal, α-quartz
			| SpaceGroup = P3<sub>1</sub>21 (No. 152), ] hP9<ref>{{cite journal|doi=10.1016/0022-4596(88)90113-2|title=The preparation and structure of the α- and β-quartz polymorphs of beryllium fluoride|year=1988|last1=Wright|first1=Albert F.|last2=Fitch|first2=Andrew N.|last3=Wright|first3=Adrian C.|journal=Journal of Solid State Chemistry|volume=73|issue=2|page=298|bibcode = 1988JSSCh..73..298W }}</ref>
			| LattConst_a = 473.29 pm
			| LattConst_c = 517.88 pm
	}}		}}
	| Section7 = {{Chembox Hazards		| Section7 = {{Chembox Hazards
			| Hazards_ref = <ref>{{Cite web|url=https://pubchem.ncbi.nlm.nih.gov/compound/24589|title=Beryllium Difluoride|website=PubChem|publisher=National Institute of Health|access-date=October 13, 2017}}</ref>
	| EUClass = ]<br/>Highly toxic ('''T+''')<br/>Irritant ('''Xi''')<br/>Dangerous for the environment ('''N''')
	| EUIndex = 004-002-00-2
	| NFPA-H =		| NFPA-H =
	| NFPA-F =		| NFPA-F =
	| NFPA-R =		| NFPA-R =
	| NFPA-O =		| NFPA-S =
			| ExternalSDS =
	| RPhrases = {{R49}}, {{R25}}, {{R26}}, {{R36/37/38}}, {{R43}}, {{R48/23}}, {{R51/53}}
			| GHSPictograms = {{GHS05|Corrosive}}{{GHS06|Acute Toxicity}}{{GHS08|Reproductive toxicity, target organ toxicity, carcinogen, aspiration hazard}}{{GHS09|Environment, aquatic toxicity}}
	| SPhrases = {{S53}}, {{S45}}, {{S61}}
			| GHSSignalWord = DANGER
	| FlashPt = non-flammable
			| HPhrases = {{H-phrases|301|305|311|314|315|319|330|335|372|411}}
	| LD50 = 98 mg/kg (oral, rat)
			| PPhrases = {{P-phrases|201|202|260|264|270|271|273|280|281|284|301+310|301+330+331|302+352|303+361+353|304+340|305+351+338|308+313|310|312|314|320|321|322|330|361|363|391|403+233|405|501}}
	| PEL = }}
			| FlashPt = Non-flammable
	| Section8 = {{Chembox Related
			| LD50 = 90 mg/kg (oral, rat)<br />100 mg/kg (oral, mouse)<ref>{{IDLH|7440417|Beryllium compounds (as Be)}}</ref>
	| OtherAnions = ]<br>]<br>]
			| REL = Ca C 0.0005 mg/m<sup>3</sup> (as Be)<ref name=PGCH>{{PGCH|0054}}</ref>
	| OtherCations = ]<br/>]<br/>]<br/>]
			| 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 <ref name=PGCH/>
			}}
			| Section8 = {{Chembox Related
			| OtherAnions = ]<br />]<br />]
			| OtherCations = ]<br />]<br />]<br />]<br />]
			| OtherCompounds = {{ubl|]|]}}
	}}		}}
	}}		}}
			'''Beryllium fluoride''' is the ] with the ] ]]<sub>2</sub>. This white solid is the principal precursor for the manufacture of ] metal. Its structure resembles that of quartz, but BeF<sub>2</sub> is highly soluble in water.
			==Properties==
			Beryllium fluoride has distinctive optical properties. In the form of ] glass, it has the lowest ] for a solid at room temperature of 1.275. Its ] is the lowest for a solid at 0.0093, and the ] is also the lowest at 2 × 10<sup>−14</sup>.
			==Structure and bonding==
			]
			The structure of solid BeF<sub>2</sub> resembles that of ]. Be<sup>2+</sup> centers are four coordinate and tetrahedral and the fluoride centers are two-coordinate.<ref>Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}}</ref> The Be-F bond lengths are about 1.54 Å.<ref>Pallavi Ghalsasi, Prasanna S. Ghalsasi, "Single Crystal X-Ray Structure of BeF2: α-Quartz" Inorg. Chem., 2011, 50 (1), pp 86–89. {{doi|10.1021/ic101248g}}</ref> Analogous to ], BeF<sub>2</sub> can also adopt a number of related structures. An analogy also exists between BeF<sub>2</sub> and AlF<sub>3</sub>: both adopt extended structures at mild temperature.
			===Gaseous and liquid BeF<sub>2</sub>===
			Gaseous beryllium fluoride adopts a linear structure, with a Be-F distance of 143 ].<ref name=Holl/> BeF<sub>2</sub> reaches a ] of 10 ] at 686&nbsp;°C, 100 Pa at 767&nbsp;°C, 1 kPa at 869&nbsp;°C, 10 kPa at 999&nbsp;°C, and 100 kPa at 1172&nbsp;°C.<ref>Vapor pressure, physics.nyu.edu, , from Ohe, S. (1976) ''Computer Aided Data Book of Vapor Pressure'', Data Book Publishing Co., Tokyo.</ref> Molecular {{chem2|BeF2}} in the gaseous state is isoelectronic to ].
			As a liquid, beryllium fluoride has a ] structure. The density of liquid BeF<sub>2</sub> decreases near its freezing point, as Be<sup>2+</sup> and ] ions begin to coordinate more strongly with one another, leading to the expansion of voids between ]s.<ref>{{cite journal
			| title = Waterlike Structural and Excess Entropy Anomalies in Liquid Beryllium Fluoride
			|author1=Agarwal, M. |author2=Chakravarty C | journal = J. Phys. Chem. B
			| year = 2007
			| volume = 111
			| pages = 13294–300
			| doi = 10.1021/jp0753272
			| pmid = 17963376
			| issue = 46
			}}</ref>
			==Production==
			The processing of beryllium ores generates impure Be(OH)<sub>2</sub>. This material reacts with ] to give ammonium tetrafluoroberyllate:
			:Be(OH)<sub>2</sub> + 2 (NH<sub>4</sub>)HF<sub>2</sub> → (NH<sub>4</sub>)<sub>2</sub>BeF<sub>4</sub> + 2 H<sub>2</sub>O
			Tetrafluoroberyllate is a robust ion, which allows its purification by precipitation of various impurities as their hydroxides. Heating purified (NH<sub>4</sub>)<sub>2</sub>BeF<sub>4</sub> gives the desired product:
			:(NH<sub>4</sub>)<sub>2</sub>BeF<sub>4</sub> → 2 NH<sub>3</sub> + 2 HF + BeF<sub>2</sub>
			In general the reactivity of BeF<sub>2</sub> ions with fluoride are quite analogous to the reactions of SiO<sub>2</sub> with oxides.<ref>{{Greenwood&Earnshaw}}</ref>
			==Applications==
			Reduction of BeF<sub>2</sub> at 1300&nbsp;°C with magnesium in a ] ] provides the most practical route to metallic beryllium:<ref name=Holl>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref>
			:BeF<sub>2</sub> + Mg → Be + MgF<sub>2</sub>
			The ] is not a useful precursor because of its volatility. {{citation needed|reason = The page on Beryllium specifically states that electrolysis of BeCl2 is a practical industrial path to metallic beryllium.|date=November 2018}}
			===Niche uses===
			Beryllium fluoride is used in biochemistry, particularly protein crystallography as a mimic of phosphate. Thus, ] and beryllium fluoride together tend to bind to ] sites and inhibit protein action, making it possible to crystallise proteins in the bound state.<ref>{{cite journal
			| title = The structure of bovine F1-ATPase inhibited by ADP and beryllium fluoride
			| author = Reiko Kagawa
			| author2 = Martin G. Montgomery
			| author3 = Kerstin Braig
			| author4 = Andrew G. W. Leslie
			| author5 = John E. Walker
			| journal =The EMBO Journal
			| year = 2004
			| volume = 23
			| issue = 5
			| pages = 2734–2744
			| doi = 10.1038/sj.emboj.7600293
			| pmid = 15229653
			| pmc = 514953
			}}</ref><ref>{{cite journal | title=Fluoride complexes of aluminium or beryllium act on G-proteins as reversibly bound analogues of the gamma phosphate of GTP |author=Bigay J. |author2=Deterre P. |author3=Pfister C. |author4=Chabre M. | journal = The EMBO Journal | year=1987 | volume=6 | issue=10 | pages=2907–2913 |doi=10.1002/j.1460-2075.1987.tb02594.x | pmid=2826123 | pmc=553725}}</ref>
			Beryllium fluoride forms a basic constituent of the preferred fluoride salt mixture used in ]s. Typically beryllium fluoride is mixed with ] to form a base solvent (]), into which fluorides of uranium and thorium are introduced. Beryllium fluoride is exceptionally chemically stable, and LiF/BeF<sub>2</sub> mixtures (]) have low melting points (360–459&nbsp;°C) and the best neutronic properties of fluoride salt combinations appropriate for reactor use. ] used two different mixtures in the two cooling circuits.
			==Safety==
			{{see|Beryllium poisoning}}
			Beryllium compounds are highly toxic. The increased toxicity of beryllium in the presence of fluoride has been noted as early as 1949.<ref>{{Cite book |url=https://www.nap.edu/read/11571 |title=Fluoride in Drinking Water: A Scientific Review of EPA's Standards |publisher=The National Academies Press |year=2006 |isbn=978-0-309-10128-8 |pages=51–52 |language=en |doi=10.17226/11571}}</ref> The {{LD50}} in mice is about 100&nbsp;mg/kg by ingestion and 1.8&nbsp;mg/kg by intravenous injection.
			==References==
			{{Reflist}}
			==External links==
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			*
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			*
			{{Beryllium compounds}}
			{{Fluorides}}
			{{DEFAULTSORT:Beryllium Fluoride}}
			]
			]
			]