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	{{chembox		{{Chembox
			| Verifiedfields = changed
	| Watchedfields = changed		| Watchedfields = changed
	| verifiedrevid = 399727535		| verifiedrevid = 417786650
	| Name = Cobalt(III) fluoride		| Name = Cobalt(III) fluoride
	| ImageFile = Cobalt(III)-fluoride-3D-balls.png		| ImageFile = Aluminium-trifluoride-3D-polyhedra.png
	| ImageName = Cobalt(III) fluoride		| ImageName = Cobalt(III) fluoride
	| OtherNames = Cobalt trifluoride<br />Cobaltic fluoride<br />Cobalt fluoride<br />Cobaltic trifluoride		| ImageFile1 = Cobalt(III) fluoride.png
			| ImageSize1 =
			| OtherNames = Cobalt trifluoride<br />Cobaltic fluoride<br />Cobalt fluoride<br />Cobaltic trifluoride
	| Section1 = {{Chembox Identifiers		|Section1={{Chembox Identifiers
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 59593		| ChemSpiderID = 59593
	| InChI = 1/Co.3FH/h;3*1H/q+3;;;/p-3		| InChI = 1/Co.3FH/h;3*1H/q+3;;;/p-3
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	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = WZJQNLGQTOCWDS-UHFFFAOYSA-K		| StdInChIKey = WZJQNLGQTOCWDS-UHFFFAOYSA-K
			| CASNo_Ref = {{cascite|correct|??}}
	| CASNo = 10026-18-3		| CASNo = 10026-18-3
	| PubChem = 66208		| CASNo2 = 54496-71-8
			| CASNo2_Comment = dihydrate
⚫	}}
			| UNII_Ref = {{fdacite|changed|FDA}}
⚫	| Section2 = {{Chembox Properties
			| UNII = O3R680UKNX
⚫	| Formula = CoF<sub>3</sub>
			| PubChem = 66208
⚫	| Appearance = brown solid
			| EINECS = 233-062-4
⚫	| MolarMass = 115.9284 g/mol
		⚫	}}
⚫	| Density = 3.88 g/cm<sup>3</sup>
		⚫	|Section2={{Chembox Properties
	| MeltingPt = 927 °C<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref>
		⚫	| Formula = {{chem2|CoF3}}
	| Solubility = reacts
		⚫	| Appearance = brown powder
⚫	}}
		⚫	| MolarMass = 115.928 g/mol
⚫	| Section3 = {{Chembox Hazards
		⚫	| Density = 3.88 g/cm<sup>3</sup>
⚫	| NFPA-H = 3
	| NFPA-F = 0		| MeltingPtC = 927
	| NFPA-R = 2		| Solubility = reacts
			| MagSus = +1900.0·10<sup>−6</sup> cm<sup>3</sup>/mol
⚫	| NFPA-O =
	}}		}}
	| Section4 = {{Chembox Related		|Section3={{Chembox Structure
			| CrystalStruct = hexagonal
⚫	| OtherAnions = ], ]
		⚫	}}
⚫	| OtherCations = ], ]
		⚫	|Section4={{Chembox Hazards
⚫	| OtherCpds = ] }}
		⚫	| NFPA-H = 3
			| NFPA-F = 0
			| NFPA-R = 2
		⚫	| NFPA-S =
			}}
			|Section5={{Chembox Related
		⚫	| OtherAnions = ], ]
		⚫	| OtherCations = ], ]
		⚫	| OtherCompounds = ] }}
	}}		}}
		⚫	'''Cobalt(III) fluoride''' is the ] with the formula {{chem2|CoF3}}. ]s are also known. The anhydrous compound is a hygroscopic brown solid. It is used to synthesize ] compounds.<ref name=Coe>{{cite encyclopedia|author=Coe, P. L.|title=Cobalt(III) Fluoride|encyclopedia=Encyclopedia of Reagents for Organic Synthesis|year=2004|publisher=J. Wiley|doi=10.1002/047084289X.rc185|isbn=0471936235}}</ref>
			The related ] is also known but is extremely unstable.<ref name=chester>Arthur W. Chester, El-Ahmadi Heiba, Ralph M. Dessau, and William J. Koehl Jr. (1969): "The interaction of cobalt(III) with chloride ion in acetic acid". ''Inorganic and Nuclear Chemistry Letters'', volume 5, issue 4, pages 277-283. {{doi|10.1016/0020-1650(69)80198-4}}</ref> Cobalt(III) bromide and cobalt(III) iodide have not been synthesized.
⚫	'''Cobalt(III) fluoride''' is the ] with the formula CoF<sub>3</sub>. This highly reactive, hygroscopic brown solid is used to synthesize ] compounds.<ref name=Coe>Coe, P. L. "Cobalt(III) Fluoride" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.</ref> CoF<sub>3</sub> is a powerful fluorinating agent, the product being ]. It decomposes upon contact with water to give oxygen:
⚫	:4 CoF<sub>3</sub> + 2 H<sub>2</sub>O &rarr; 4 HF + 4 CoF<sub>2</sub> + O<sub>2</sub>
			==Structure==
⚫	CoF<sub>3</sub> is prepared in the laboratory by treating CoCl<sub>2</sub> with ] at 250 °C:<ref>Priest, H. F. “Anhydrous Metal Fluorides” Inorganic Syntheses McGraw-Hill: New York, 1950; Vol. 3, pages 171-183.</ref>
	:] + 3/2 F<sub>2</sub> &rarr; CoF<sub>3</sub> + Cl<sub>2</sub>
	This conversion is a redox reaction, Co<sup>2+</sup> is converted to Co<sup>3+</sup> and chloride to ] at the expense of fluorine, which is converted to fluoride. Cobalt(II) oxide (CoO) and cobalt(II) fluoride (CoF<sub>2</sub>) can also be converted to cobalt(III) fluoride using fluorine.
			===Anhydrous===
⚫	CoF<sub>3</sub> is hygroscopic and can be converted to the anion <sup>3-</sup>, a rare example of a high-spin, octahedral cobalt(III) complex.
			Anhydrous cobalt trifluoride crystallizes in the ] group, specifically according to the ] motif, with ''a'' = 527.9 ], ''α'' = 56.97°. Each cobalt atom is bound to six fluorine atoms in octahedral geometry, with Co–F distances of 189 pm. Each fluoride is a doubly bridging ligand.<ref name=levason/>
			===Hydrates===
⚫	Used as slurry, CoF<sub>3</sub> converts ]s to the ]:
			A hydrate {{chem2|CoF3*3.5H2O}} is known. It is conjectured to be better described as {{chem2|*0.5H2O}}.<ref name=levason/>
	:2CoF<sub>3</sub> + R-H &rarr; 2CoF<sub>2</sub> + R-F + HF
			There is a report of an hydrate {{chem2|CoF3*3.5H2O}}, isomorphic to {{chem2|AlF3*3H2O}}.<ref name=levason/>
⚫	Such reactions are sometimes accompanied by rearrangements or other reactions.<ref name=Coe/> The related reagent KCoF<sub>4</sub> is more selective.<ref>Coe, P. L. "Potassium Tetrafluorocobaltate(III)" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.</ref>
			==Preparation==
		⚫	Cobalt trifluoride can be prepared in the laboratory by treating ] with ] at 250&nbsp;°C:<ref name=priest>H. F. Priest (1950): "Anhydrous Metal Fluorides". In ''Inorganic Syntheses'', McGraw-Hill, volume 3, pages 171-183. {{doi|10.1002/9780470132340.ch47}}</ref><ref name=levason/>
			:{{chem2|CoCl2}} + 3/2 {{chem2|F2}} → {{chem2|CoF3}} + {{chem2|Cl2}}
			In this redox reaction, {{chem2|Co(2+)}} and {{chem2|Cl(-)}} are oxidized to {{chem2|Co(3+)}} and {{chem2|Cl2}}, respectively, while {{chem2|F2}} is reduced to {{chem2|F(-)}}. Cobalt(II) oxide (CoO) and cobalt(II) fluoride ({{chem2|CoF2}}) can also be converted to cobalt(III) fluoride using fluorine.<ref name=levason>W. Levason and C. A. McAuliffe (1974): "Higher oxidation state chemistry of iron, cobalt, and nickel". ''Coordination Chemistry Reviews'', volume 12, issue 2, pages 151-184. {{doi|10.1016/S0010-8545(00)82026-3}}</ref>
			The compound can also be formed by treating {{chem2|CoCl2}} with ] {{chem2|ClF3}} or ] {{chem2|BrF3}}.<ref name=levason/>
			==Reactions==
			{{chem2|CoF3}} decomposes upon contact with water to give oxygen:
		⚫	:4 {{chem2|CoF3}} + 2 H<sub>2</sub>O → 4 HF + 4 Co{{chem2|F2}} + O<sub>2</sub>
		⚫	It reacts with fluoride salts to give the anion <sup>3−</sup>, which is also features high-spin, octahedral cobalt(III) center.
			==Applications==
		⚫	{{chem2|CoF3}} is a powerful fluorinating agent. Used as slurry, {{chem2|CoF3}} converts ]s to the ]:
			:2 {{chem2|CoF3}} + R-H → 2 Co{{chem2|F2}} + R-F + HF
			] is the byproduct.
		⚫	Such reactions are sometimes accompanied by rearrangements or other reactions.<ref name=Coe/> The related reagent KCoF<sub>4</sub> is more selective.<ref>Coe, P. L. "Potassium Tetrafluorocobaltate(III)" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. {{doi|10.1002/047084289X.rp251}}.</ref>
			==Gaseous {{chem2|CoF3}}==
			In the gas phase, {{chem2|CoF3}} is calculated to be planar in its ground state, and has a 3-fold rotation axis (point group D<sub>3h</sub>). The {{chem2|Co(3+)}} ion has a ground state of 3d<sup>6</sup> <sup>5</sup>D. The fluoride ligands split this state into, in energy order, <sup>5</sup>A', <sup>5</sup>E", and <sup>5</sup>E' states. The first energy difference is small and the <sup>5</sup>E" state is subject to the ], so this effect needs to be considered to be sure of the ground state. The energy lowering is small and does not change the energy order.<ref>{{cite journal | last1=Yates | first1 =J. H. | last2=Pitzer | first2 = R. M. | date=1979 | title = Molecular and Electronic Structure of Transition Metal Trifluorides | journal = J. Chem. Phys. | volume = 70 | issue = 9 | pages = 4049–4055 | doi = 10.1063/1.438027| bibcode =1979JChPh..70.4049Y }}</ref> This calculation was the first treatment of the ] using calculated energy surfaces.
	==References==		==References==
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	==External links==		==External links==
	{{Commons cat|Cobalt(III) fluoride}}		{{Commons category|Cobalt(III) fluoride}}
	*		*
	*		*
	{{Cobalt compounds}}		{{Cobalt compounds}}
			{{fluorides}}
	]		]
	]		]
		⚫	]
	]		]
	]
	]
⚫	]
	]