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{{chembox
{{chembox
| verifiedrevid = 401635842
| verifiedrevid = 401635842
| Name = Titanium(IV) fluoride
| Name = Titanium(IV) fluoride
| ImageFile = Titanium(IV)-fluoride-from-xtal-column-3D-bs-17.png
| ImageFile =
<!-- | ImageSize = 200px -->
| ImageSize = 160px
| ImageName = Titanium(IV) fluoride
| ImageName = Titanium(IV) fluoride
| IUPACName = Titanium(IV) fluoride
| OtherNames = titanium tetrafluoride
| OtherNames = Titanium tetrafluoride
| Section1 = {{Chembox Identifiers
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 7988529
| ChemSpiderID = 7988529
| InChI = 1/4FH.Ti/h4*1H;/q;;;;+4/p-4
| InChI = 1/4FH.Ti/h4*1H;/q;;;;+4/p-4
| InChIKey = XROWMBWRMNHXMF-XBHQNQODAM
| InChIKey = XROWMBWRMNHXMF-XBHQNQODAM
| SMILES = [Ti+4].[F-].[F-].[F-].[F-]
| SMILES = F[Ti](F)(F)F
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/4FH.Ti/h4*1H;/q;;;;+4/p-4
| StdInChI = 1S/4FH.Ti/h4*1H;/q;;;;+4/p-4
Line 17: Line 18:
| StdInChIKey = XROWMBWRMNHXMF-UHFFFAOYSA-J
| StdInChIKey = XROWMBWRMNHXMF-UHFFFAOYSA-J
| CASNo = 7783-63-3
| CASNo = 7783-63-3
| CASNo_Ref = {{cascite|correct|CAS}}
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = T08RW8YRG1
| PubChem = 121824
| PubChem = 121824
| EINECS = 232-017-6
| EINECS = 232-017-6
}}
}}
| Section2 = {{Chembox Properties
|Section2={{Chembox Properties
| Formula = TiF<sub>4</sub>
| Formula = TiF<sub>4</sub>
| MolarMass = 123.861 g/mol
| MolarMass = 123.861 g/mol
| Appearance = white powder<br /> [[hygroscopic]]
| Appearance = white powder
| Density = 2.798 g/cm<sup>3</sup>
| Density = 2.798 g/cm<sup>3</sup>
| MeltingPt = 377 °C
| MeltingPtC = 377
| BoilingPt = sublimes
| BoilingPt = sublimes
⚫
}}
| Solubility =
⚫
|Section7={{Chembox Hazards
⚫
}}
| GHS_ref=<ref>{{cite web |title=Titanium tetrafluoride |url=https://pubchem.ncbi.nlm.nih.gov/compound/121824#section=Safety-and-Hazards |website=pubchem.ncbi.nlm.nih.gov |access-date=12 December 2021 |language=en}}</ref>
| Section3 = {{Chembox Structure
| GHSPictograms = {{GHS05}}{{GHS07}}
| CrystalStruct =
| GHSSignalWord = Danger
⚫
}}
| HPhrases = {{H-phrases|302|312|314|332}}
⚫
| Section7 = {{Chembox Hazards
| PPhrases = {{P-phrases|260|261|264|270|271|280|301+312|301+330+331|302+352|303+361+353|304+312|304+340|305+351+338|310|312|322|330|363|405}}
| EUClass = not listed
| NFPA-H = 3
| NFPA-H = 3
| NFPA-F = 0
| NFPA-F = 0
| NFPA-R = 0
| NFPA-R = 0
⚫
}}
| NFPA-O =
|Section8={{Chembox Related
⚫
}}
| OtherAnions = [[Titanium(IV) bromide]] <br/> [[Titanium(IV) chloride]] <br/> [[Titanium(IV) iodide]]
| OtherCompounds = [[Titanium(III) fluoride]]
⚫
}}
}}
}}


'''Titanium(IV) fluoride''' is the [[inorganic compound]] with the [[chemical formula|formula]] [[Titanium|Ti]][[Fluoride|F<sub>4</sub>]]. It is a white [[hygroscopic]] solid. In contrast to the other halides of titanium, it adopts a polymeric structure consisting of octahedral Ti centres.<ref>{{Greenwood&Earnshaw2nd}}</ref>
'''Titanium(IV) fluoride''' is the [[inorganic compound]] with the [[chemical formula|formula]] [[Titanium|Ti]][[Fluoride|F<sub>4</sub>]]. It is a white [[hygroscopic]] solid. In contrast to the other tetrahalides of titanium, it adopts a polymeric structure.<ref>{{Greenwood&Earnshaw2nd}}</ref> In common with the other tetrahalides, TiF<sub>4</sub> is a strong [[Lewis acid]].


==Preparation==
==Preparation and structure==
The traditional method involves treatment of titanium tetrachloride with excess [[hydrogen fluoride]], and purification by sublimation:<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref>
The traditional method involves treatment of [[titanium tetrachloride]] with excess [[hydrogen fluoride]]:<ref name=KO>{{cite book |doi=10.1002/0471238961.2009200113051908.a01 |chapter=Fluorine Compounds, Inorganic, Titanium |title=Kirk-Othmer Encyclopedia of Chemical Technology |year=2000 |last1=Meshri |first1=Dayal T. |isbn=978-0-471-48494-3 }}</ref>
:TiCl<sub>4</sub> + 4 HF → TiF<sub>4</sub> + 4 HCl
:TiCl<sub>4</sub> + 4 HF → TiF<sub>4</sub> + 4 HCl
Purification is by sublimation, which involves reversible [[Cracking (chemistry)|cracking]] of the polymeric structure.<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref>
X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.<ref>{{cite journal|author1=Bialowons, H.|author2=Mueller, M.|author3=Mueller, B.G.|title=Titantetrafluorid - Eine Überraschend einfache Kolumnarstruktur|journal=Zeitschrift für Anorganische und Allgemeine Chemie|year=1995|volume= 621|issue=7 |pages=1227–1231|doi=10.1002/zaac.19956210720}}</ref>

==Reactions==
[[File:CSD CIF AJAZAN.jpg|thumb|Structure of the [Ti<sub>4</sub>F<sub>18</sub>]<sup>2-</sup> dianion|left]]
TiF<sub>4</sub> forms adducts with many ligands. One example is the complex ''cis''-TiF<sub>4</sub>(CH<sub>3</sub>CN)<sub>2</sub>, which is formed by treatment with [[acetonitrile]].<ref>{{cite journal|title=A survey of Titanium Fluoride Complexes, Their Preparation, Reactivity, and Applications|author1=Nikiforov, Grigory B.|author2=Roesky, Herbert W.|author3=Koley, Debasis|journal=Coordination Chemistry Reviews |year=2014|volume=258-259|pages=16–57|doi=10.1016/j.ccr.2013.09.002}}</ref> It is also used as a reagent in the preparation of [[organofluorine compound]]s.<ref>{{cite book |doi=10.1002/047084289X.rn00123.pub2 |chapter=Titanium(IV) Fluoride |title=Encyclopedia of Reagents for Organic Synthesis |year=2014 |last1=Blizzard |first1=T. A. |last2=Sikervar |first2=Vikas |pages=1–5 |isbn=978-0-470-84289-8 }}</ref> With fluoride, the cluster [Ti<sub>4</sub>F<sub>18</sub>]<sup>2-</sup> forms. It has an adamantane-like Ti<sub>4</sub>F<sub>6</sub> core.<ref>{{cite journal |doi=10.1021/ic9009338 |title=Poly&#91;perfluorotitanate(IV)&#93; Salts of &#91;H<sub>3</sub>O&#93;<sup>+</sup>, Cs<sup>+</sup>, &#91;Me<sub>4</sub>N&#93;<sup>+</sup>, and &#91;Ph<sub>4</sub>P&#93;<sup>+</sup> and about the Existence of an Isolated &#91;Ti<sub>2</sub>F<sub>9</sub>&#93;<sup>−</sup> Anion in the Solid State |year=2009 |last1=Mazej |first1=Zoran |last2=Goreshnik |first2=Evgeny |journal=Inorganic Chemistry |volume=48 |issue=14 |pages=6918–6923 |pmid=19545141 }}</ref>

Related to its [[Lewis acid]]ity, TiF<sub>4</sub> forms a variety of hexafluorides also called hexafluorotitanates. Hexafluorotitanic acid has been used commercially to clean metal surfaces. These salts are stable at pH<4 in the presence of [[hydrogen fluoride]], otherwise they hydrolyze to give [[oxide]]s.<ref name=KO/>


==References==
==References==
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{{Titanium compounds}}
{{Titanium compounds}}
{{fluorides}}


[[Category:Fluorides]]
[[Category:Fluorides]]
[[Category:Titanium compounds]]
[[Category:Titanium halides]]
[[Category:Titanium(IV) compounds]]

[[Category:Adamantane-like molecules]]
{{inorganic-compound-stub}}

[[ar:فلوريد تيتانيوم رباعي]]
[[de:Titan(IV)-fluorid]]
[[fa:تترافلورید تیتانیوم]]
[[ja:フッ化チタン(IV)]]
[[ru:Фторид титана(IV)]]
[[zh:四氟化钛]]

Latest revision as of 03:00, 19 February 2024

Titanium(IV) fluoride
Titanium(IV) fluoride
Names
IUPAC name
Titanium(IV) fluoride
Other names
Titanium tetrafluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.106 Edit this at Wikidata
EC Number
  • 232-017-6
UNII
  • InChI=1S/4FH.Ti/h4*1H;/q;;;;+4/p-4 checkY
    Key: XROWMBWRMNHXMF-UHFFFAOYSA-J checkY
  • InChI=1/4FH.Ti/h4*1H;/q;;;;+4/p-4
    Key: XROWMBWRMNHXMF-XBHQNQODAM
  • F[Ti](F)(F)F
Properties
TiF4
Molar mass 123.861 g/mol
Appearance white powder
Density 2.798 g/cm3
Melting point 377 °C (711 °F; 650 K)
Boiling point sublimes
Hazards
GHS labelling:[1]
GHS05: CorrosiveGHS07: Exclamation mark
Danger
H302, H312, H314, H332
P260, P261, P264, P270, P271, P280, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P310, P312, P322, P330, P363, P405
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Related compounds
Other anions
 Titanium(IV) bromide
Titanium(IV) chloride
Titanium(IV) iodide
Related compounds
 Titanium(III) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Titanium(IV) fluoride is the inorganic compound with the formula TiF4. It is a white hygroscopic solid. In contrast to the other tetrahalides of titanium, it adopts a polymeric structure.[2] In common with the other tetrahalides, TiF4 is a strong Lewis acid.

Preparation and structure

[edit]

The traditional method involves treatment of titanium tetrachloride with excess hydrogen fluoride:[3]

TiCl4 + 4 HF → TiF4 + 4 HCl

Purification is by sublimation, which involves reversible cracking of the polymeric structure.[4] X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.[5]

Reactions

[edit]
Structure of the [Ti4F18]2- dianion

TiF4 forms adducts with many ligands. One example is the complex cis-TiF4(CH3CN)2, which is formed by treatment with acetonitrile.[6] It is also used as a reagent in the preparation of organofluorine compounds.[7] With fluoride, the cluster [Ti4F18]2- forms. It has an adamantane-like Ti4F6 core.[8]

Related to its Lewis acidity, TiF4 forms a variety of hexafluorides also called hexafluorotitanates. Hexafluorotitanic acid has been used commercially to clean metal surfaces. These salts are stable at pH<4 in the presence of hydrogen fluoride, otherwise they hydrolyze to give oxides.[3]

References

[edit]
  1. ^ "Titanium tetrafluoride". pubchem.ncbi.nlm.nih.gov. Retrieved 12 December 2021.
  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  3. ^ a b Meshri, Dayal T. (2000). "Fluorine Compounds, Inorganic, Titanium". Kirk-Othmer Encyclopedia of Chemical Technology. doi:10.1002/0471238961.2009200113051908.a01. ISBN 978-0-471-48494-3.
  4. ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.
  5. ^ Bialowons, H.; Mueller, M.; Mueller, B.G. (1995). "Titantetrafluorid - Eine Überraschend einfache Kolumnarstruktur". Zeitschrift für Anorganische und Allgemeine Chemie. 621 (7): 1227–1231. doi:10.1002/zaac.19956210720.
  6. ^ Nikiforov, Grigory B.; Roesky, Herbert W.; Koley, Debasis (2014). "A survey of Titanium Fluoride Complexes, Their Preparation, Reactivity, and Applications". Coordination Chemistry Reviews. 258–259: 16–57. doi:10.1016/j.ccr.2013.09.002.
  7. ^ Blizzard, T. A.; Sikervar, Vikas (2014). "Titanium(IV) Fluoride". Encyclopedia of Reagents for Organic Synthesis. pp. 1–5. doi:10.1002/047084289X.rn00123.pub2. ISBN 978-0-470-84289-8.
  8. ^ Mazej, Zoran; Goreshnik, Evgeny (2009). "Poly[perfluorotitanate(IV)] Salts of [H3O]+, Cs+, [Me4N]+, and [Ph4P]+ and about the Existence of an Isolated [Ti2F9]− Anion in the Solid State". Inorganic Chemistry. 48 (14): 6918–6923. doi:10.1021/ic9009338. PMID 19545141.
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