Aluminium fluoride

Aluminium fluoride
	; Anhydrous AlF3
Names
	Other names Aluminium(III) fluoride; Aluminum trifluoride
Identifiers
CAS Number	7784-18-1 ; 32287-65-3 (monohydrate) ; 15098-87-0 (trihydrate) ;
3D model (JSmol)	monomer: Interactive image; crystal form: Interactive image;
ChEBI	CHEBI:49464 ;
ChemSpider	2039 ;
ECHA InfoCard	100.029.137
PubChem CID	2124;
RTECS number	BD0725000;
UNII	Z77H3IKW94 ;
CompTox Dashboard (EPA)	DTXSID8030712 ;
	show InChI
	show SMILES
Properties
Chemical formula	AlF3
Molar mass	83.977 g/mol (anhydrous) ; 101.992 g/mol (monohydrate) ; 138.023 (trihydrate)
Appearance	white, crystalline solid; odorless
Density	3.10 g/cm3 (anhydrous) ; 2.17 g/cm3 (monohydrate) ; 1.914 g/cm3 (trihydrate)
Melting point	1,290 °C (2,350 °F; 1,560 K) (anhydrous) (sublimes)
Solubility in water	5.6 g/L (0 °C) ; 6.7 g/L (20 °C) ; 17.2 g/L (100 °C)
Magnetic susceptibility (χ)	−13.4×10−6 cm3/mol
Refractive index (nD)	1.3767 (visible range)
Structure
Crystal structure	Rhombohedral, hR24
Space group	R3c, No. 167
Lattice constant	a = 0.49254 nm, c = 1.24477 nm
Lattice volume (V)	0.261519
Formula units (Z)	6
Thermochemistry
Heat capacity (C)	75.1 J/mol·K
Std molar; entropy (So298)	66.5 J/mol·K
Std enthalpy of; formation (ΔfH⦵298)	−1510.4 kJ/mol
Gibbs free energy (ΔfG˚)	−1431.1 kJ/mol
Hazards
Safety data sheet	InChem MSDS
GHS pictograms
GHS Signal word	Danger
GHS hazard statements	H301, H302, H314, H315, H319, H335, H361, H372
GHS precautionary statements	P260, P261, P264, P270, P271, P280, P301+310, P301+312, P301+330+331, P302+352, P303+361+353, P304+340, P305+351+338, P310, P312, P321, P330, P332+313, P337+313, P362, P363, P403+233, P405, P501
NFPA 704 (fire diamond)	3 0 0
	NIOSH (US health exposure limits):
PEL (Permissible)	none
REL (Recommended)	2 mg/m3
IDLH (Immediate danger)	N.D.
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	(what is ?)
	Infobox references

Aluminium fluoride refers to inorganic compounds with the formula AlF₃·xH₂O. They are all colorless solids. Anhydrous AlF₃ is used in the production of aluminium metal. Several occur as minerals.

Occurrence and production[]

Aside from anhydrous AlF₃, several hydrates are known. With the formula AlF₃·xH₂O, these compounds include monohydrate (x = 1), two polymorphs of the trihydrate (x = 3), a hexahydrate (x = 6), and a nonahydrate (x = 9).^[10]

The majority of aluminium fluoride is produced by treating alumina with hydrogen fluoride at 700 °C:^[4] Fluorosilicic acid may also be used make aluminum fluoride.^[11]

H₂SiF₆ + Al₂O₃ + 3 H₂O → 2 AlF₃ + SiO₂ + 4 H₂O

Alternatively, it is manufactured by thermal decomposition of ammonium hexafluoroaluminate.^[12] For small scale laboratory preparations, AlF₃ can also be prepared by treating aluminium hydroxide or aluminium metal 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 .^[13]^[14] A related, exceedingly rare mineral, is zharchikhite, Al(OH)₂F.^[15]^[16]

Structure[]

According to X-ray crystallography, anhydrous AlF₃ adopts the rhenium trioxide motif, featuring distorted AlF₆ octahedra. Each fluoride is connected to two Al centers. Because of its three-dimensional polymeric structure, AlF₃ has a high melting point. The other trihalides of aluminium in the solid state differ, AlCl₃ has a layer structure and AlBr₃ and AlI₃, are molecular dimers.^[17]^{[page needed]} Also they have low melting points and evaporate readily to give dimers.^[18]^{[page needed]} In the gas phase aluminium fluoride exists as trigonal molecules of D_3h symmetry. The Al–F bond lengths of this gaseous molecule are 163 pm.

Like most gaseous metal trifluorides, AlF₃ adopts a planar structure upon evaporation.

Applications[]

Aluminium fluoride is an important additive for the production of aluminium by electrolysis.^[4] Together with cryolite, it lowers the melting point to below 1000 °C and increases the conductivity of the solution. It is into this molten salt that aluminium oxide is dissolved and then electrolyzed to give bulk Al metal.^[12]

Aluminum 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 ATP and GTP control most of the reactions involved in metabolism, growth and differentiation.^[19] The observation that aluminum fluoride can bind to and activate heterotrimeric G proteins 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 proteins.^[20]

Niche uses[]

Together with zirconium fluoride, aluminium fluoride is an ingredient for the production of fluoroaluminate glasses.

It is also used to inhibit fermentation.

Like magnesium fluoride it 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) of aluminum fluoride is 0.1 g/kg.^[21] Repeated or prolonged inhalation exposure may cause asthma, and may have effects on the bone and nervous system, resulting in bone alterations (fluorosis), and nervous system impairment.^[22]

Many of the neurotoxic effects of fluoride are due to the formation of aluminum fluoride complexes, which mimic the chemical structure of a phosphate and influence the activity of ATP phosphohydrolases and phospholipase D. Only micromolar concentrations of aluminum are needed to form aluminum fluoride.^[23]

Human exposure to aluminum fluoride can occur in an industrial setting, such as emissions from aluminum reduction processes,^[24] or when a person ingests both a fluoride source (e.g., fluoride in drinking water or residue of fluoride-based pesticides) and an aluminum source; sources of human exposure to aluminum include drinking water, tea, food residues, infant formula, aluminum-containing antacids or medications, deodorants, cosmetics, and glassware.^[23] Fluoridation chemicals may also contain aluminum fluoride.^[25] Data on the potential neurotoxic effects of chronic exposure to the aluminum species existing in water are limited.^[26]

References[]

^ Jump up to: ^a ^b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.45. ISBN 1439855110.
^ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.131. ISBN 1439855110.
^ Lide, David R. (2003-06-19). CRC Handbook of Chemistry and Physics. CRC Handbook (84th ed.). CRC Press. ISBN 9780849304842.
^ Jump up to: ^a ^b ^c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 233. ISBN 978-0-08-037941-8.
^ Hoppe, R.; Kissel, D. (1984). "Zur kenntnis von AlF₃ und InF₃ [1]". Journal of Fluorine Chemistry. 24 (3): 327. doi:10.1016/S0022-1139(00)81321-4.
^ Jump up to: ^a ^b ^c ^d Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.5. ISBN 1439855110.
^ Pohanish, Richard P. (2005-03-04). HazMat Data: For First Response, Transportation, Storage, and Security. John Wiley & Sons. ISBN 9780471726104.
^ "Aluminum Fluoride". PubChem. National Institute of Health. Retrieved October 12, 2017.
^ NIOSH Pocket Guide to Chemical Hazards. "#0024". National Institute for Occupational Safety and Health (NIOSH).
^ Guangmei Wang; Anja-Verena Mudring (2016). "The missing Hydrate AlF₃·6H₂O [Al(H₂O)₆]F₃: Ionothermal Synthesis, Crystal Structure and Characterization of Aluminum Fluoride Hexahydrate". Solid State Sciences. 61: 61. doi:10.1016/j.solidstatesciences.2016.09.007.
^ Dreveton, Alain (2012-01-01). "Manufacture of Aluminium Fluoride of High Density and Anhydrous Hydrofluoric Acid from Fluosilicic Acid". Procedia Engineering. SYMPHOS 2011 - 1st International Symposium on Innovation and Technology in the Phosphate Industry. 46 (Supplement C): 255–265. doi:10.1016/j.proeng.2012.09.471.
^ Jump up to: ^a ^b Aigueperse, J.; Mollard, P.; Devilliers, D.; Chemla, M.; Faron, R.; Romano, R.; Cuer, J. P. "Fluorine Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH.
^ https://www.mindat.org/min-43853.html
^ https://www.ima-mineralogy.org/Minlist.htm
^ https://www.mindat.org/min-4399.html
^ https://www.ima-mineralogy.org/Minlist.htm
^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego, CA: Academic Press. ISBN 0-12-352651-5..
^ Wittinghofer, Alfred (1997-11-01). "Signaling mechanistics: Aluminum fluoride for molecule of the year". Current Biology. 7 (11): R682–R685. doi:10.1016/S0960-9822(06)00355-1. PMID 9382787. S2CID 17666164.
^ Vincent, Sylvie; Brouns, Madeleine; Hart, Matthew J.; Settleman, Jeffrey (1998-03-03). "Evidence for distinct mechanisms of transition state stabilization of GTPases by fluoride". Proceedings of the National Academy of Sciences. 95 (5): 2210–2215. Bibcode:1998PNAS...95.2210V. doi:10.1073/pnas.95.5.2210. ISSN 0027-8424. PMC 19296. PMID 9482864.
^ "ALUMINUM FLUORIDE, CASRN: 7784-18-1". National Library of Medicine HSDB Database. CDC.gov. June 24, 2005. Retrieved October 12, 2017.
^ "ALUMINIUM FLUORIDE (ANHYDROUS) International Chemical Safety Cards (ICSC)". CDC.gov National Institute for Occupational Safety and Health (NIOSH). July 22, 2015. Retrieved July 17, 2017.
^ Jump up to: ^a ^b Fluoride in Drinking Water: A Scientific Review of EPA's Standards. The National Academies Press. 2006. pp. 51–52, 219. doi:10.17226/11571. ISBN 978-0-309-10128-8.
^ TOXICOLOGICAL PROFILE FOR FLUORIDES, HYDROGEN FLUORIDE, AND FLUORINE (PDF). U.S. DEPARTMENT OF HEALTH AND HUMAN SERVICES Public Health Service Agency for Toxic Substances and Disease Registry. 2003. p. 211.
^ Mullenix, Phyllis J (2014). "A new perspective on metals and other contaminants in fluoridation chemicals". International Journal of Occupational and Environmental Health. 20 (2): 157–166. doi:10.1179/2049396714Y.0000000062. ISSN 1077-3525. PMC 4090869. PMID 24999851.
^ 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

External links[]

[b92-1] Jump up to: ^a ^b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.45. ISBN 1439855110.

[2] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.131. ISBN 1439855110.

[3] Lide, David R. (2003-06-19). CRC Handbook of Chemistry and Physics. CRC Handbook (84th ed.). CRC Press. ISBN 9780849304842.

[g233-4] Jump up to: ^a ^b ^c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 233. ISBN 978-0-08-037941-8.

[5] Hoppe, R.; Kissel, D. (1984). "Zur kenntnis von AlF₃ und InF₃ [1]". Journal of Fluorine Chemistry. 24 (3): 327. doi:10.1016/S0022-1139(00)81321-4.

[b92t-6] Jump up to: ^a ^b ^c ^d Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.5. ISBN 1439855110.

[7] Pohanish, Richard P. (2005-03-04). HazMat Data: For First Response, Transportation, Storage, and Security. John Wiley & Sons. ISBN 9780471726104.

[8] "Aluminum Fluoride". PubChem. National Institute of Health. Retrieved October 12, 2017.

[PGCH-9] NIOSH Pocket Guide to Chemical Hazards. "#0024". National Institute for Occupational Safety and Health (NIOSH).

[10] Guangmei Wang; Anja-Verena Mudring (2016). "The missing Hydrate AlF₃·6H₂O [Al(H₂O)₆]F₃: Ionothermal Synthesis, Crystal Structure and Characterization of Aluminum Fluoride Hexahydrate". Solid State Sciences. 61: 61. doi:10.1016/j.solidstatesciences.2016.09.007.

[11] Dreveton, Alain (2012-01-01). "Manufacture of Aluminium Fluoride of High Density and Anhydrous Hydrofluoric Acid from Fluosilicic Acid". Procedia Engineering. SYMPHOS 2011 - 1st International Symposium on Innovation and Technology in the Phosphate Industry. 46 (Supplement C): 255–265. doi:10.1016/j.proeng.2012.09.471.

[Ullmann-12] Jump up to: ^a ^b Aigueperse, J.; Mollard, P.; Devilliers, D.; Chemla, M.; Faron, R.; Romano, R.; Cuer, J. P. "Fluorine Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH.

[13] ttps://www.mindat.org/min-43853.html

[14] ttps://www.ima-mineralogy.org/Minlist.htm

[15] ttps://www.mindat.org/min-4399.html

[16] ttps://www.ima-mineralogy.org/Minlist.htm

[17] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[18] Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego, CA: Academic Press. ISBN 0-12-352651-5..

[19] Wittinghofer, Alfred (1997-11-01). "Signaling mechanistics: Aluminum fluoride for molecule of the year". Current Biology. 7 (11): R682–R685. doi:10.1016/S0960-9822(06)00355-1. PMID 9382787. S2CID 17666164.

[20] Vincent, Sylvie; Brouns, Madeleine; Hart, Matthew J.; Settleman, Jeffrey (1998-03-03). "Evidence for distinct mechanisms of transition state stabilization of GTPases by fluoride". Proceedings of the National Academy of Sciences. 95 (5): 2210–2215. Bibcode:1998PNAS...95.2210V. doi:10.1073/pnas.95.5.2210. ISSN 0027-8424. PMC 19296. PMID 9482864.

[21] "ALUMINUM FLUORIDE, CASRN: 7784-18-1". National Library of Medicine HSDB Database. CDC.gov. June 24, 2005. Retrieved October 12, 2017.

[:0-22] "ALUMINIUM FLUORIDE (ANHYDROUS) International Chemical Safety Cards (ICSC)". CDC.gov National Institute for Occupational Safety and Health (NIOSH). July 22, 2015. Retrieved July 17, 2017.

[:1-23] Jump up to: ^a ^b Fluoride in Drinking Water: A Scientific Review of EPA's Standards. The National Academies Press. 2006. pp. 51–52, 219. doi:10.17226/11571. ISBN 978-0-309-10128-8.

[24] TOXICOLOGICAL PROFILE FOR FLUORIDES, HYDROGEN FLUORIDE, AND FLUORINE (PDF). U.S. DEPARTMENT OF HEALTH AND HUMAN SERVICES Public Health Service Agency for Toxic Substances and Disease Registry. 2003. p. 211.

[25] Mullenix, Phyllis J (2014). "A new perspective on metals and other contaminants in fluoridation chemicals". International Journal of Occupational and Environmental Health. 20 (2): 157–166. doi:10.1179/2049396714Y.0000000062. ISSN 1077-3525. PMC 4090869. PMID 24999851.

[26] 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

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Names
Anhydrous AlF₃
Other names Aluminium(III) fluoride Aluminum trifluoride
Identifiers
CAS Number	7784-18-1^Y 32287-65-3 (monohydrate)^Y 15098-87-0 (trihydrate)^Y
3D model (JSmol)	monomer: Interactive image crystal form: Interactive image
ChEBI	CHEBI:49464^Y
ChemSpider	2039^Y
ECHA InfoCard	100.029.137
PubChem CID	2124
RTECS number	BD0725000
UNII	Z77H3IKW94^Y
CompTox Dashboard (EPA)	DTXSID8030712
show InChI InChI=1S/Al.3FH/h;31H/q+3;;;/p-3^Y Key: KLZUFWVZNOTSEM-UHFFFAOYSA-K^Y InChI=1/Al.3FH/h;31H/q+3;;;/p-3 Key: KLZUFWVZNOTSEM-DFZHHIFOAC
show SMILES monomer: F[Al](F)F crystal form: 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
Properties
Chemical formula	AlF₃
Molar mass	83.977 g/mol (anhydrous) 101.992 g/mol (monohydrate) 138.023 (trihydrate)^[1]
Appearance	white, crystalline solid odorless
Density	3.10 g/cm³ (anhydrous) 2.17 g/cm³ (monohydrate) 1.914 g/cm³ (trihydrate)^[1]
Melting point	1,290 °C (2,350 °F; 1,560 K)^[4] (anhydrous) (sublimes)
Solubility in water	5.6 g/L (0 °C) 6.7 g/L (20 °C) 17.2 g/L (100 °C)
Magnetic susceptibility (χ)	−13.4×10⁻⁶ cm³/mol^[2]
Refractive index (n_D)	1.3767 (visible range)^[3]
Structure
Crystal structure	Rhombohedral, hR24
Space group	R3c, No. 167^[5]
Lattice constant	a = 0.49254 nm, c = 1.24477 nm
Lattice volume (V)	0.261519
Formula units (Z)	6
Thermochemistry
Heat capacity (C)	75.1 J/mol·K^[6]
Std molar entropy (S^o₂₉₈)	66.5 J/mol·K^[6]
Std enthalpy of formation (Δ_fH^⦵₂₉₈)	−1510.4 kJ/mol^[6]
Gibbs free energy (Δ_fG˚)	−1431.1 kJ/mol^[6]
Hazards^[7]^[8]^[9]
Safety data sheet	InChem MSDS
GHS pictograms
GHS Signal word	Danger
GHS hazard statements	H301, H302, H314, H315, H319, H335, H361, H372
GHS precautionary statements	P260, P261, P264, P270, P271, P280, P301+310, P301+312, P301+330+331, P302+352, P303+361+353, P304+340, P305+351+338, P310, P312, P321, P330, P332+313, P337+313, P362, P363, P403+233, P405, P501
NFPA 704 (fire diamond)	3 0 0
NIOSH (US health exposure limits):
PEL (Permissible)	none
REL (Recommended)	2 mg/m³
IDLH (Immediate danger)	N.D.
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y (what is ^YN ?)
Infobox references