Aluminium fluoride: Difference between revisions

|Watchedfields = changed

|verifiedrevid = 443382196

|

ImageFile = Aluminium-trifluoride-3D-polyhedra.png

|ImageCaption = Anhydrous {{chem2|AlF3}}

| = Aluminium

|Section1={{Chembox Identifiers

|InChI = 1/Al.3FH/h;3*1H/q+3;;;/p-3

|ChEBI_Ref = {{ebicite|correct|EBI}}

|ChEBI = 49464

|StdInChI_Ref = {{stdinchicite|correct|chemspider}}

|StdInChI = 1S/Al.3FH/h;3*1H/q+3;;;/p-3

|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

|StdInChIKey = KLZUFWVZNOTSEM-UHFFFAOYSA-K

|SMILES = F[Al](F)F

|SMILES_Comment = [[monomer]]

|SMILES1 = F[Al](F[Al]0(F)(F)(F)F)(F[Al]1(F)(F)(F)F)(F[Al]2(F)(F)(F)F)(F[Al]3(F)(F)(F)F)F[Al](F[Al](F[Al]4(F)(F)(F)F)(F[Al]5(F)(F)(F)F)(F[Al]6(F)(F)(F)F)(F0)F)(F[Al](F[Al]7(F)(F)(F)F)(F[Al]8(F)(F)(F)F)(F1)(F4)F)(F[Al](F[Al]9(F)(F)(F)F)(F[Al]0(F)(F)(F)F)(F5)(F7)F)(F[Al](F[Al]1(F)(F)(F)F)(F2)(F8)(F9)F)F[Al](F3)(F6)(F0)(F1)F

|SMILES1_Comment = crystal form

|InChIKey = KLZUFWVZNOTSEM-DFZHHIFOAC

| = --

|CASNo_Ref = {{cascite|correct|CAS}}

|CASNo1_Ref = {{cascite|correct|??}}

|CASNo1 = 32287-65-3

|CASNo1_Comment = (monohydrate)

| = {{|correct|}}

|CASNo2 = 15098-87-0

|CASNo2_Comment = (trihydrate)

|UNII_Ref = {{fdacite|correct|FDA}}

|UNII = Z77H3IKW94

|PubChem = 2124

|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

|ChemSpiderID =2039

|RTECS = BD0725000

}}

|Section2={{Chembox Properties

|Formula = {{chem2|AlF3}}

|MolarMass = {{ubl|83.977 g/mol (anhydrous)|101.992 g/mol (monohydrate)|138.023 (trihydrate)}}<ref name=b92>{{RubberBible92nd|page=4.45}}</ref>

|Appearance = Colorless to white crystalline solid

|Odor = Odorless

|Density = {{ubl|3.10 g/cm³ (anhydrous)|2.17 g/cm³ (monohydrate)|1.914 g/cm³ (trihydrate)}}<ref name=b92/>

|Solubility = {{ubl|5.6 g/L (0&nbsp;°C)|6.7 g/L (20&nbsp;°C)|17.2 g/L (100&nbsp;°C)}}

|MeltingPtC = 1290

|MeltingPt_notes = (anhydrous) (sublimes)

|MeltingPt_ref = <ref name=g233/>

|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=[[CRC Handbook]]

}}</ref>

|MagSus = {{val|-13.4e-6|u=cm³/mol}}<ref>{{RubberBible92nd|page=4.131}}</ref>

}}

|Section3={{Chembox Structure

|CrystalStruct = [[Rhombohedral lattice system|Rhombohedral]], [[Pearson symbol|hR24]]

|SpaceGroup = R{{overline|3}}c, No. 167<ref>{{cite journal|doi=10.1016/S0022-1139(00)81321-4|title=Zur kenntnis von AlF₃ und InF₃ [1]|journal=Journal of Fluorine Chemistry|volume=24|issue=3|pages=327|year=1984|last1=Hoppe|first1=R.|last2=Kissel|first2=D.}}</ref>

|LattConst_a = 0.49254 nm

|LattConst_c = 1.24477 nm

|UnitCellFormulas = 6

|UnitCellVolume =0.261519

}}

|Section4={{Chembox Thermochemistry

|DeltaHf = −1510.4 kJ/mol<ref name=b92t>{{RubberBible92nd|page=5.5}}</ref>

|Entropy = 66.5 J/(mol·K)<ref name=b92t/>

|DeltaGf = −1431.1 kJ/mol<ref name=b92t/>

|HeatCapacity = 75.1 J/(mol·K)<ref name=b92t/>

}}

|Section5={{Chembox Hazards

|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>

|NFPA-H = 3

|NFPA-F = 0

|NFPA-R = 0

|ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics1324.htm InChem MSDS]

|GHSPictograms = {{GHS05|Corrosive}} {{GHS06|Acute toxicity}} {{GHS07|Irritant}} {{GHS08|Reproductive toxicity, target organ toxicity, aspiration hazard}}

|GHSSignalWord = DANGER

|HPhrases = {{H-phrases|301|302|314|315|319|335|361|372}}

|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}}

|IDLH = N.D.

|PEL = none

|REL = 2 mg/m³

}}

|Section9={{Chembox Related

|OtherAnions = {{ubl|[[Aluminium chloride]]|[[Aluminium bromide]]|[[Aluminium iodide]]}}

|OtherCations = {{ubl|[[Boron trifluoride]]|[[Gallium trifluoride]]|[[Indium trifluoride]]|[[Thallium trifluoride]]}}

|OtherCompounds = {{ubl|[[Scandium(III) fluoride]]|[[Yttrium(III) fluoride]]|[[Lutetium(III) fluoride]]|[[Lanthanum(III) fluoride]]|[[Cerium(III) fluoride]]|[[Actinium(III) fluoride]]}}

}}

'''Aluminium fluoride''' is an [[inorganic compound]] [[]]. in .

== and ==

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 AlF₃·6H₂O [Al(H₂O)₆]F₃: 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>

The majority of aluminium fluoride is produced by treating [[alumina]] with [[hydrogen fluoride]] at 700&nbsp;°C:<ref name=g233>{{Greenwood&Earnshaw2nd|page=233}}</ref> [[Hexafluorosilicic acid]] 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>

:{{chem2|H2[SiF6] + Al2O3 + 3 H2O → 2 AlF3 + SiO2 + 4 H2O}}

Alternatively, it is manufactured by thermal decomposition of [[ammonium hexafluoroaluminate]].<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 [[aluminium hydroxide]] or aluminium with [[hydrogen fluoride]].

Aluminium fluoride trihydrate is found in nature as the rare mineral [[rosenbergite]].

The anhydrous form appears as the relatively recently (as of 2020) recognized mineral [[óskarssonite]].<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" />

[[ ]] adopts the [[rhenium trioxide]] motif, featuring distorted [[octahedron|octahedra]]. Each fluoride is connected to two Al centers. Because of -dimensional , has a [[melting point]]. other trihalides of aluminium, [[Aluminium chloride|]] [[aluminium bromide|]] and [[aluminium iodide|]], are molecular have low melting points and evaporate readily to give dimers.<ref>HollemanA. F.WibergE.Inorganic ChemistryAcademic PressSan Diego, 2001 0-12-352651-5.</ref> In the gas phase aluminium fluoride exists as trigonal molecules of ''D_3h'' [[symmetry group|symmetry]]. The bond lengths of this gaseous molecule are 163[[|pm]].

[[Image:Aluminium-trifluoride-monomer-2D-dimensions.png|100px| .]]

Aluminium fluoride is an important additive for the production of aluminium by electrolysis. Together with [[cryolite]] lowers the melting point to below 1000°C and increases the conductivity of the [[electrolyte|solution]]. It is into this molten salt that aluminium oxide is dissolved and then electrolyzed to give bulk Al metal.<ref name=Ullmann/>

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 [[adenosine triphosphate]] and [[guanosine triphosphate]] 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 [[G protein]]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 [[hydrolysis]], including the role of [[GTPase-activating protein]]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>

It is also used to inhibit [[fermentation (biochemistry)|fermentation]].

Like [[magnesium fluoride]] it is used as a low-index optical [[thin film]], particularly when far [[UV]] transparency is required. Its deposition by [[physical vapor deposition]], particularly by [[evaporation]], is favorable.

==Safety==

The reported oral animal lethal dose ([[LD50|LD₅₀]]) 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 [[asthma]], and may have effects on the bone and nervous system, resulting in bone alterations ([[Skeletal fluorosis|fluorosis]]), 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>

Many of the [[Neurotoxicity|neurotoxic]] effects of fluoride are due to the formation of aluminium fluoride complexes, which mimic the chemical structure of a [[phosphate]] and influence the activity of [[ATP phosphohydrolase (H+-transporting)|ATP phosphohydrolases]] and [[phospholipase D]]. Only [[micromolar]] 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>

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 [[pesticide]]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>[https://ntp.niehs.nih.gov/ntp/htdocs/chem_background/exsumpdf/aluminum_508.pdf Aluminum Compounds Review of Toxicological Literature Abridged Final Report]. Prepared for National Institute of Environmental Health Sciences. ''NTP.gov Nomination Summary for Aluminum contaminants of drinking water (N20025).'' October 2001</ref>

==See also==

* [[Aluminium monofluoride]]

{{Reflist}}

{{Commons category|Aluminium fluoride}}

* [https://web.archive.org/web/20110722155414/http://www.solvaychemicals.us/static/wma/pdf/5/1/1/9/ALF.pdf MSDS]

* [https://toxnet.nlm.nih.gov/cgi-bin/sis/search/a?dbs+hsdb:@term+@DOCNO+600 ToxNet Profile]

* [https://pubchem.ncbi.nlm.nih.gov/compound/aluminum_fluoride PubChem]

{{fluorine compounds}}

{{Authority control}}