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| verifiedrevid = 443380627 |
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|verifiedrevid = 443382196 |
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| Name = Aluminium fluoride |
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| ImageFile = Aluminium-trifluoride-3D-polyhedra.png |
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|Name = Aluminium fluoride |
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|ImageFile = Aluminium-trifluoride-3D-polyhedra.png |
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|ImageCaption = Anhydrous {{chem2|AlF3}} |
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| ImageFile2 =FeF3structure.jpg |
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| ImageName = Aluminium trifluoride crystal structure |
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|OtherNames = Aluminium(III) fluoride<br />Aluminum trifluoride |
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|Section1={{Chembox Identifiers |
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| OtherNames = Aluminium(III) fluoride<br />Aluminum trifluoride |
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|InChI = 1/Al.3FH/h;3*1H/q+3;;;/p-3 |
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| Section1 = {{Chembox Identifiers |
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|ChEBI_Ref = {{ebicite|correct|EBI}} |
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| InChI = 1/Al.3FH/h;3*1H/q+3;;;/p-3 |
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|ChEBI = 49464 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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|StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| ChEBI = 49464 |
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|StdInChI = 1S/Al.3FH/h;3*1H/q+3;;;/p-3 |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/Al.3FH/h;3*1H/q+3;;;/p-3 |
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|StdInChIKey = KLZUFWVZNOTSEM-UHFFFAOYSA-K |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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|SMILES = F(F)F |
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| StdInChIKey = KLZUFWVZNOTSEM-UHFFFAOYSA-K |
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|SMILES_Comment = ] |
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| SMILES = F(F)F |
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|SMILES1 = F(F0(F)(F)(F)F)(F1(F)(F)(F)F)(F2(F)(F)(F)F)(F3(F)(F)(F)F)F(F(F4(F)(F)(F)F)(F5(F)(F)(F)F)(F6(F)(F)(F)F)(F0)F)(F(F7(F)(F)(F)F)(F8(F)(F)(F)F)(F1)(F4)F)(F(F9(F)(F)(F)F)(F0(F)(F)(F)F)(F5)(F7)F)(F(F1(F)(F)(F)F)(F2)(F8)(F9)F)F(F3)(F6)(F0)(F1)F |
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| InChIKey = KLZUFWVZNOTSEM-DFZHHIFOAC |
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|SMILES1_Comment = crystal form |
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| CASNo = 7784-18-1 |
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|InChIKey = KLZUFWVZNOTSEM-DFZHHIFOAC |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo1 = 32287-65-3 |
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|CASNo = 7784-18-1 |
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|CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo1_Comment = (monohydrate) |
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|CASNo1_Ref = {{cascite|correct|??}} |
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| CASNo2 = 15098-87-0 |
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|CASNo1 = 32287-65-3 |
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| CASNo2_Comment = (trihydrate) |
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|CASNo1_Comment = (monohydrate) |
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| PubChem = 2124 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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|CASNo2_Ref = {{cascite|correct|??}} |
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|CASNo2 = 15098-87-0 |
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| ChemSpiderID =2039 |
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|CASNo2_Comment = (trihydrate) |
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| RTECS = BD0725000 |
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|UNII_Ref = {{fdacite|correct|FDA}} |
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}} |
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|UNII = Z77H3IKW94 |
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| Section2 = {{Chembox Properties |
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|PubChem = 2124 |
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| Formula = AlF<sub>3</sub> |
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|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| MolarMass = 83.9767 g/mol (anhydrous) <br> 101.022 g/mol (monohydrate) <br> 138.023 (trihydrate) |
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|ChemSpiderID =2039 |
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| Appearance = white, crystalline solid<br />odorless |
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|RTECS = BD0725000 |
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| Density = 2.88 g/cm<sup></sup> (anhydrous) <br> 2.1 g/cm<sup>3</sup> (monohydrate) <br> 1.914 g/cm<sup>3</sup> (trihydrate) |
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}} |
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| Solubility = 0.56 g/100 mL (0 °C) <br> 0.67 g/100 mL (20 °C) <br> 1.72 g/100 mL (100 °C) |
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|Section2={{Chembox Properties |
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| MeltingPt = 1291 °C (anhydrous) |
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|Formula = {{chem2|AlF3}} |
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}} |
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|MolarMass = {{ubl|83.977 g/mol (anhydrous)|101.992 g/mol (monohydrate)|138.023 (trihydrate)}}<ref name=b92>{{RubberBible92nd|page=4.45}}</ref> |
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| Section3 = {{Chembox Structure |
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|Appearance = Colorless to white crystalline solid |
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| CrystalStruct = ], ] |
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|Odor = Odorless |
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| SpaceGroup = R-3c, No. 167 |
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|Density = {{ubl|3.10 g/cm<sup>3</sup> (anhydrous)|2.17 g/cm<sup>3</sup> (monohydrate)|1.914 g/cm<sup>3</sup> (trihydrate)}}<ref name=b92/> |
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}} |
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|Solubility = {{ubl|5.6 g/L (0 °C)|6.7 g/L (20 °C)|17.2 g/L (100 °C)}} |
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|MeltingPtC = 1290 |
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| Section7 = {{Chembox Hazards |
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|MeltingPt_notes = (anhydrous) (sublimes) |
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| EUClass = No classification according to EU Regulation (EC) No. 1272/2008. |
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|MeltingPt_ref = <ref name=g233/> |
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| NFPA-H = 0 |
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|RefractIndex = 1.3767 (visible range)<ref>{{Cite book|url=https://books.google.com/books?id=kTnxSi2B2FcC|title=CRC Handbook of Chemistry and Physics|edition=84th|last=Lide|first=David R.|date=2003-06-19|publisher=CRC Press|isbn=9780849304842|series=] |
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| NFPA-F = 0 |
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}}</ref> |
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| NFPA-R = 0 |
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|MagSus = {{val|-13.4e-6|u=cm<sup>3</sup>/mol}}<ref>{{RubberBible92nd|page=4.131}}</ref> |
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| RPhrases = - |
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}} |
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| SPhrases = - |
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|Section3={{Chembox Structure |
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}} |
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|CrystalStruct = ], ] |
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|SpaceGroup = R{{overline|3}}c, No. 167<ref>{{cite journal|doi=10.1016/S0022-1139(00)81321-4|title=Zur kenntnis von AlF<sub>3</sub> und InF<sub>3</sub> |journal=Journal of Fluorine Chemistry|volume=24|issue=3|pages=327|year=1984|last1=Hoppe|first1=R.|last2=Kissel|first2=D.}}</ref> |
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|LattConst_a = 0.49254 nm |
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|LattConst_c = 1.24477 nm |
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|UnitCellFormulas = 6 |
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|UnitCellVolume =0.261519 |
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}} |
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|Section4={{Chembox Thermochemistry |
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|DeltaHf = −1510.4 kJ/mol<ref name=b92t>{{RubberBible92nd|page=5.5}}</ref> |
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|Entropy = 66.5 J/(mol·K)<ref name=b92t/> |
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|DeltaGf = −1431.1 kJ/mol<ref name=b92t/> |
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|HeatCapacity = 75.1 J/(mol·K)<ref name=b92t/> |
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}} |
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|Section5={{Chembox Hazards |
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|Hazards_ref = <ref>{{Cite book|url=https://books.google.com/books?id=3Tbl2W8j-3oC&q=nfpa+704+aluminum+fluoride|title=HazMat Data: For First Response, Transportation, Storage, and Security|last=Pohanish|first=Richard P.|date=2005-03-04|publisher=John Wiley & Sons|isbn=9780471726104|language=en}}</ref><ref>{{Cite web|url=https://pubchem.ncbi.nlm.nih.gov/compound/aluminum_fluoride|title=Aluminum Fluoride|website=PubChem|publisher=National Institute of Health|access-date=October 12, 2017}}</ref><ref name=PGCH>{{PGCH|0024}}</ref> |
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|NFPA-H = 3 |
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|NFPA-F = 0 |
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|NFPA-R = 0 |
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|ExternalSDS = |
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|GHSPictograms = {{GHS05|Corrosive}} {{GHS06|Acute toxicity}} {{GHS08|Reproductive toxicity, target organ toxicity, aspiration hazard}} |
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|GHSSignalWord = DANGER |
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|HPhrases = {{H-phrases|301|302|314|315|319|335|361|372}} |
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|PPhrases = {{P-phrases|260|261|264|270|271|280|301+310|301+312|301+330+331|302+352|303+361+353|304+340|305+351+338|310|312|321|330|332+313|337+313|362|363|403+233|405|501}} |
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|IDLH = N.D. |
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|PEL = none |
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|REL = 2 mg/m<sup>3</sup> |
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}} |
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|Section9={{Chembox Related |
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|OtherAnions = {{ubl|]|]|]}} |
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|OtherCations = {{ubl|]|]|]|]}} |
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|OtherCompounds = {{ubl|]|]|]|]|]|]}} |
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'''Aluminium fluoride''' ({{Aluminium}}{{Fluorine|3}}) is an ] used primarily in the production of ]. This colourless solid can be prepared synthetically but also occurs in nature. |
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'''Aluminium fluoride''' is an ] with the formula {{chem2|AlF3|auto=1}}. It forms ] {{chem2|AlF3*''x''H2O}}. Anhydrous {{chem2|AlF3}} and its hydrates are all colorless solids. Anhydrous {{chem2|AlF3}} is used in the production of aluminium. Several occur as minerals. |
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==Production and occurrence== |
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==Occurrence and production== |
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Aside from anhydrous {{chem2|AlF3}}, several hydrates are known. With the formula {{chem2|AlF3*''x''H2O}}, these compounds include monohydrate (''x'' = 1), two polymorphs of the trihydrate (''x'' = 3), a hexahydrate (''x'' = 6), and a nonahydrate (''x'' = 9).<ref>{{cite journal|title=The missing Hydrate AlF<sub>3</sub>·6H<sub>2</sub>O F<sub>3</sub>: Ionothermal Synthesis, Crystal Structure and Characterization of Aluminum Fluoride Hexahydrate|year=2016|journal=Solid State Sciences|page=61|doi=10.1016/j.solidstatesciences.2016.09.007|author=Guangmei Wang|author2=Anja-Verena Mudring|volume=61}}</ref> |
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The majority of aluminium fluoride is mainly produced by treating ] with ]: |
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:H<sub>2</sub>SiF<sub>6</sub> + Al<sub>2</sub>O<sub>3</sub> → 2 AlF<sub>3</sub> + SiO<sub>2</sub> + H<sub>2</sub>O |
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Alternatively, it is manufactured by thermal decomposition of ammonium hexafluoroaluminate.<ref name=Ullmann>J. Aigueperse, P. Mollard, D. Devilliers, M. Chemla, R. Faron, R. Romano, J. P. Cuer, “Fluorine Compounds, Inorganic” in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.{{DOI|10.1002/14356007.a11_307}}</ref> For small scale laboratory preparations, AlF<sub>3</sub> can also be prepared by treating ] or aluminium metal with ]. |
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The majority of aluminium fluoride is produced by treating ] with ] at 700 °C:<ref name=g233>{{Greenwood&Earnshaw2nd|page=233}}</ref> ] may also be used make aluminium fluoride.<ref>{{Cite journal|last=Dreveton|first=Alain|date=2012-01-01|title=Manufacture of Aluminium Fluoride of High Density and Anhydrous Hydrofluoric Acid from Fluosilicic Acid|journal=Procedia Engineering|series=SYMPHOS 2011 - 1st International Symposium on Innovation and Technology in the Phosphate Industry|volume=46|issue=Supplement C|pages=255–265|doi=10.1016/j.proeng.2012.09.471|doi-access=free}}</ref> |
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Aluminium fluoride trihydrate is found in nature as the rare mineral rosenbergite. |
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:{{chem2|H2 + Al2O3 + 3 H2O → 2 AlF3 + SiO2 + 4 H2O}} |
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Alternatively, it is manufactured by thermal decomposition of ].<ref name=Ullmann>{{Ullmann|author=Aigueperse, J.|author2=Mollard, P.|author3=Devilliers, D.|author4=Chemla, M.|author5=Faron, R.|author6=Romano, R.|author7=Cuer, J. P.|date=2005|title=Fluorine Compounds, Inorganic|DOI=10.1002/14356007.a11_307}}</ref> For small scale laboratory preparations, {{chem2|AlF3}} can also be prepared by treating ] or aluminium with ]. |
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Aluminium fluoride trihydrate is found in nature as the rare mineral ]. |
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The anhydrous form appears as the relatively recently (as of 2020) recognized mineral ].<ref>{{Cite web|url=https://www.mindat.org/min-43853.html|title = Óskarssonite}}</ref><ref name="List of Minerals">{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> A related, exceedingly rare mineral, is zharchikhite, {{chem2|Al(OH)2F}}.<ref>{{Cite web|url=https://www.mindat.org/min-4399.html|title=Zharchikhite}}</ref><ref name="List of Minerals" /> |
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==Structure== |
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==Structure== |
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Its ] adopts the ] motif, featuring distorted AlF<sub>6</sub> ]. Each fluoride is connected to two Al centers. Because of it is a 3-dimensional polymer, AlF<sub>3</sub> has a higher ]. In contrast, the other trihalides of aluminium, ], ], and ], which are either molecular or 1-dimensional polymers, have low melting points and evaporate readily to give dimers.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> In the gas phase, at ca. 1000 °C, aluminium fluoride exists as trigonal molecules of ''D<sub>3h</sub>'' ]. The Al-F bond lengths of this gaseous molecule are 163 ]. |
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According to ], anhydrous {{chem2|AlF3}} adopts the ] motif, featuring distorted {{chem2|AlF6}} ]. Each fluoride is connected to two Al centers. Because of its three-dimensional polymeric structure, {{chem2|AlF3}} has a high ]. The other trihalides of aluminium in the solid state differ, ] has a layer structure and ] and ], are molecular dimers.<ref>{{Greenwood&Earnshaw}}</ref>{{page needed|date=January 2020}} Also they have low melting points and evaporate readily to give dimers.<ref>{{cite book|last1=Holleman|first1=A. F.|last2=Wiberg|first2=E.|title=Inorganic Chemistry|publisher=Academic Press|location=San Diego, CA|date=2001 |isbn=0-12-352651-5}}.</ref>{{page needed|date=January 2020}} In the gas phase aluminium fluoride exists as trigonal molecules of ''D<sub>3h</sub>'' ]. The Al–F bond lengths of this gaseous molecule are 163 ]. |
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<center>] ]</center> |
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] |
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==Applications== |
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==Applications== |
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Aluminium fluoride is an important additive for the production of aluminium by electrolysis. Together with ] lowers the melting point to below 1000 °C and increases the conductivity of the ]. It is into this molten salt that aluminium oxide is dissolved and then electrolyzed to give bulk Al metal.<ref name=Ullmann/> |
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Aluminium fluoride is an important additive for the production of aluminium by electrolysis.<ref name=g233/> Together with ], it lowers the melting point to below 1000 °C and increases the conductivity of the ]. It is into this molten salt that aluminium oxide is dissolved and then electrolyzed to give bulk Al metal.<ref name=Ullmann/> |
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Aluminium fluoride complexes are used to study the mechanistic aspects of phosphoryl transfer reactions in biology, which are of fundamental importance to cells, as phosphoric acid anhydrides such as ] and ] control most of the reactions involved in metabolism, growth and differentiation.<ref>{{Cite journal|last=Wittinghofer|first=Alfred|date=1997-11-01|title=Signaling mechanistics: Aluminum fluoride for molecule of the year|journal=Current Biology|volume=7|issue=11|pages=R682–R685|doi=10.1016/S0960-9822(06)00355-1|pmid=9382787|s2cid=17666164|doi-access=free}}</ref> The observation that aluminium fluoride can bind to and activate heterotrimeric ]s has proven to be useful for the study of G protein activation in vivo, for the elucidation of three-dimensional structures of several GTPases, and for understanding the biochemical mechanism of GTP ], including the role of ]s.<ref>{{Cite journal|last1=Vincent|first1=Sylvie|last2=Brouns|first2=Madeleine|last3=Hart|first3=Matthew J.|last4=Settleman|first4=Jeffrey|date=1998-03-03|title=Evidence for distinct mechanisms of transition state stabilization of GTPases by fluoride|journal=Proceedings of the National Academy of Sciences|language=en|volume=95|issue=5|pages=2210–2215|issn=0027-8424|pmid=9482864|doi=10.1073/pnas.95.5.2210|pmc=19296|bibcode=1998PNAS...95.2210V|doi-access=free}}</ref> |
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===Niche uses=== |
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===Niche uses=== |
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Together with ], aluminium fluoride is an ingredient for the production of ]es. |
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Together with ], aluminium fluoride is an ingredient for the production of ]es. |
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It is also used to inhibit ]. |
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It is also used to inhibit ]. |
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Like ] it is used as a low-index optical ], particularly when far ] transparency is required. Its deposition by ], particularly by ], is favorable. |
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It is a sputtering target for preparation of low index films. |
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==Safety== |
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The reported oral animal lethal dose (]) of aluminium fluoride is 100 mg/kg.<ref>{{Cite web|url=https://toxnet.nlm.nih.gov/cgi-bin/sis/search/a?dbs+hsdb:@term+@DOCNO+600|title=ALUMINUM FLUORIDE, CASRN: 7784-18-1|date=June 24, 2005|website=National Library of Medicine HSDB Database|publisher=CDC.gov|access-date=October 12, 2017}}</ref> Repeated or prolonged inhalation exposure may cause ], and may have effects on the bone and nervous system, resulting in bone alterations (]), and nervous system impairment.<ref name=":0">{{Cite web|url=https://www.cdc.gov/niosh/ipcsneng/neng1324.html|title=ALUMINIUM FLUORIDE (ANHYDROUS) International Chemical Safety Cards (ICSC)|date=July 22, 2015|website=CDC.gov National Institute for Occupational Safety and Health (NIOSH)|access-date=July 17, 2017}}</ref> |
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Many of the ] effects of fluoride are due to the formation of aluminium fluoride complexes, which mimic the chemical structure of a ] and influence the activity of ] and ]. Only ] concentrations of aluminium are needed to form aluminium fluoride.<ref name=":1">{{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, 219|language=en|doi=10.17226/11571}}</ref> |
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Human exposure to aluminium fluoride can occur in an industrial setting, such as emissions from aluminium reduction processes,<ref>{{Cite book|title=TOXICOLOGICAL PROFILE FOR FLUORIDES, HYDROGEN FLUORIDE, AND FLUORINE|publisher=U.S. DEPARTMENT OF HEALTH AND HUMAN SERVICES Public Health Service Agency for Toxic Substances and Disease Registry|year=2003|url=https://www.atsdr.cdc.gov/toxprofiles/tp11.pdf|pages=211}}</ref> or when a person ingests both a fluoride source (e.g., fluoride in drinking water or residue of fluoride-based ]s) and an aluminium source; sources of human exposure to aluminium include drinking water, tea, food residues, infant formula, aluminium-containing antacids or medications, deodorants, cosmetics, and glassware.<ref name=":1" /> Fluoridation chemicals may also contain aluminium fluoride.<ref>{{Cite journal|last=Mullenix|first=Phyllis J|date=2014|title=A new perspective on metals and other contaminants in fluoridation chemicals|journal=International Journal of Occupational and Environmental Health|volume=20|issue=2|pages=157–166|doi=10.1179/2049396714Y.0000000062|issn=1077-3525|pmc=4090869|pmid=24999851}}</ref> Data on the potential neurotoxic effects of chronic exposure to the aluminium species existing in water are limited.<ref>. Prepared for National Institute of Environmental Health Sciences. ''NTP.gov Nomination Summary for Aluminum contaminants of drinking water (N20025).'' October 2001</ref> |
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==See also== |
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* ] |
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==References== |
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==References== |
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{{Reflist}} |
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<references /> |
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==External links== |
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==External links== |
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{{Commons category|Aluminium fluoride}} |
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{{Aluminium compounds}} |
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{{Aluminium compounds}} |
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{{fluorine compounds}} |
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{{Authority control}} |
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