titanium tetrachloride

{{chem2|TiCl4}} is a dense, colourless liquid, although crude samples may be yellow or even red-brown. It is one of the rare transition metal halides that is a liquid at room temperature, vanadium tetrachloride being another example. This property reflects the fact that molecules of {{chem2|TiCl4}} weakly self-associate. Most metal chlorides are polymers, wherein the chloride atoms bridge between the metals. Its melting point is similar to that of Carbon tetrachloride.{{cite book|last1=Earnshaw|first1=A.|last2=Greenwood|first2=N.|year=1997|title=Chemistry of the Elements|edition=2nd|publisher=Butterworth-Heinemann}}

{{chem2|Ti(4+)}} has a "closed" electronic shell, with the same number of electrons as the noble gas argon. The tetrahedral structure for {{chem2|TiCl4}} is consistent with its description as a d⁰ metal center ({{chem2|Ti(4+)}}) surrounded by four identical ligands. This configuration leads to highly symmetrical structures, hence the tetrahedral shape of the molecule. {{chem2|TiCl4}} adopts similar structures to Titanium tetrabromide and Titanium tetraiodide; the three compounds share many similarities. {{chem2|TiCl4}} and {{chem2|TiBr4}} react to give mixed halides {{chem2|TiCl_{4−x}Br_{x}|}}, where x = 0, 1, 2, 3, 4. Magnetic resonance measurements also indicate that halide exchange is also rapid between {{chem2|TiCl4}} and {{chem2|VCl4}}.{{cite journal|first1= S. P. |last1=Webb |first2=M. S. |last2=Gordon |title= Intermolecular Self-Interactions of the Titanium Tetrahalides TiX₄ (X = F, Cl, Br)|journal=J. Am. Chem. Soc.|year=1999|volume=121| pages=2552–2560 |doi=10.1021/ja983339i|issue= 11|bibcode=1999JAChS.121.2552W |url=https://lib.dr.iastate.edu/cgi/viewcontent.cgi?article=1355&context=chem_pubs|url-access=subscription}}

{{chem2|TiCl4}} is soluble in toluene and chlorocarbons. Certain arenes form complexes of the type {{chem2|[(C6R6)TiCl3]+}}. {{chem2|TiCl4}} reacts exothermically with donor solvents such as THF to give hexacoordinated adducts.{{cite book|first1= L. E. |last1=Manzer|chapter=31. Tetragtdrfuran Complexes of Selected Early Transition Metals |title= Inorganic Syntheses|year=1982| volume=21| pages=135–40|doi=10.1002/9780470132524.ch31|isbn= 978-0-470-13252-4}} Bulkier ligands (L) give pentacoordinated adducts {{chem2|TiCl4L}}.

{{chem2|TiCl4}} is produced by the chloride process, which involves the reduction of titanium oxide ores, typically ilmenite ({{chem2|FeTiO3}}), with carbon under flowing chlorine at 900 °C. Impurities are removed by distillation.{{cite encyclopedia|author1=Heinz Sibum |author2=Volker Güther |author3=Oskar Roidl |author4=Fathi Habashi |author5=Hans Uwe Wolf |author6=Carsten Siemers |title=Titanium, Titanium Alloys, and Titanium Compounds

|encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry |publisher=Wiley-VCH |location=Weinheim |date=2017 |pages=1–35 |doi=10.1002/14356007.a27_095.pub2|isbn=978-3-527-30673-2 }}

:{{chem2|2 FeTiO3 + 7 Cl2 + 6 C → 2 TiCl4 + 2 FeCl3 + 6 CO}}

The coproduction of Iron(III) chloride is undesirable, which has motivated the development of alternative technologies. Instead of directly using ilmenite, "rutile slag" is used. This material, an impure form of {{chem2|TiO2}}, is derived from ilmenite by removal of iron, either using carbon reduction or extraction with sulfuric acid. Crude {{chem2|TiCl4}} contains a variety of other volatile halides, including vanadyl chloride ({{chem2|VOCl3}}), silicon tetrachloride ({{chem2|SiCl4}}), and tin tetrachloride ({{chem2|SnCl4}}), which must be separated.

The world's supply of titanium metal, about 250,000 tons per year, is made from {{chem2|TiCl4}}. The conversion involves the reduction of the tetrachloride with magnesium metal. This procedure is known as the Kroll process:

:{{chem2|2 Mg + TiCl4 → 2 MgCl2 + Ti}}

In the Hunter process, liquid sodium is the reducing agent instead of magnesium.{{Cite encyclopedia |entry=Hunter process |dictionary=A Dictionary of Chemical Engineering |date=2014 |url=http://www.oxfordreference.com/view/10.1093/acref/9780199651450.001.0001/acref-9780199651450-e-1447 |url-access=subscription |language=en|doi=10.1093/acref/9780199651450.001.0001|last1=Schaschke |first1=Carl |publisher=Oxford University Press |isbn=978-0-19-965145-0 }}

Around 90% of the {{chem2|TiCl4}} production is used to make the pigment titanium dioxide ({{chem2|TiO2}}). The conversion involves hydrolysis of {{chem2|TiCl4}}, a process that forms hydrogen chloride:{{cite encyclopedia|first=Hans G. |last=Völz |display-authors=etal |title=Inorganic Pigments|encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry |publisher=Wiley-VCH |location=Weinheim |date=2006 |doi=10.1002/14356007.n20_n04|chapter=Pigments, Inorganic |isbn=978-3-527-30673-2 }}

:{{chem2|TiCl4 + 2 H2O → TiO2 + 4 HCl}}

In some cases, {{chem2|TiCl4}} is oxidised directly with oxygen:

:{{chem2|TiCl4 + O2 → TiO2 + 2 Cl2}}

It has been used to produce smoke screens since it produces a heavy, white smoke that has little tendency to rise. "Tickle" was the standard means of producing on-set smoke effects for motion pictures, before being phased out in the 1980s due to concerns about hydrated HCl's effects on the respiratory system.{{Citation needed|date=April 2025}}

Titanium tetrachloride is a versatile reagent that forms diverse derivatives including those illustrated below.{{cite book |last1=Reetz |first1=Manfred T. |title=Organotitanium reagents in organic synthesis |date=1986 |publisher=Springer-Verl |location=Berlin Heidelberg New York Tokyo |isbn=0-387-15784-0 |edition=Reactivity and Structure Concepts in Organic Chemistry, Vol 24}}

Image:TiCl4cmpds.png

A characteristic reaction of {{chem2|TiCl4}} is its easy hydrolysis, signaled by the release of HCl vapors and titanium oxides and oxychlorides. Titanium tetrachloride has been used to create naval smokescreens, as the hydrochloric acid aerosol and titanium dioxide that is formed scatter light very efficiently. This smoke is corrosive, however.

Alcohols react with {{chem2|TiCl4}} to give alkoxides with the formula {{chem2|[Ti(OR)4]_{n}|}} (R = alkyl, n = 1, 2, 4). As indicated by their formula, these alkoxides can adopt complex structures ranging from monomers to tetramers. Such compounds are useful in materials science as well as organic synthesis. A well known derivative is titanium isopropoxide, which is a monomer. Titanium bis(acetylacetonate)dichloride results from treatment of titanium tetrachloride with excess acetylacetone:{{cite journal|first1=C. A. |last1=Wilkie |first2=G. |last2=Lin |first3=D. T. |last3=Haworth |title=Cis-[Dihalobis(2,4-Pentaedionato)Titanium(IV)] Complexes |journal=Inorg. Synth.|year= 1979 |volume=19 |pages=145–148 |doi=10.1002/9780470132500.ch33|isbn=978-0-470-13250-0 }}

:{{chem2|TiCl4 + 2 Hacac → Ti(acac)2Cl2 + 2 HCl}}

Organic amines react with {{chem2|TiCl4}} to give complexes containing amido ({{chem2|R2N−}}-containing) and imido ({{chem2|RN(2−)}}-containing) complexes. With ammonia, titanium nitride is formed. An illustrative reaction is the synthesis of tetrakis(dimethylamido)titanium {{chem2|Ti(N(CH3)2)4}}, a yellow, benzene-soluble liquid:{{cite journal|first1= D. C. |last1=Bradey |first2=M. |last2=Thomas|title= Some Dialkylamino-derivatives of Titanium and Zirconium|journal=J. Chem. Soc.| year=1960| pages=3857–3861| doi= 10.1039/JR9600003857}} This molecule is tetrahedral, with planar nitrogen centers.{{cite journal|author1=M. E. Davie |author2=T. Foerster |author3=S. Parsons |author4=C. Pulham |author5=D. W. H. Rankin |author6=B. A. Smart |title= The Crystal Structure of Tetrakis(dimethylamino)titanium(IV)|journal=Polyhedron| year=2006| volume=25| pages=923–929|doi= 10.1016/j.poly.2005.10.019|issue= 4}}

:{{chem2|4 LiN(CH3)2 + TiCl4 → 4 LiCl + Ti(N(CH3)2)4}}

{{chem2|TiCl4}} is a Lewis acid as implicated by its tendency to hydrolyze. With the ether THF, {{chem2|TiCl4}} reacts to give yellow crystals of {{chem2|TiCl4(THF)2}}. With chloride salts, {{chem2|TiCl4}} reacts to form sequentially {{chem2|[Ti2Cl9]−}}, {{chem2|[Ti2Cl10](2−)}} (see figure above), and {{chem2|[TiCl6](2−)}}.{{cite journal|first1= C. S.|last1= Creaser |first2=J. A. |last2=Creighton|title= Pentachloro- and Pentabromotitanate(IV) ions|journal= Dalton Trans.| year=1975| pages= 1402–1405|doi= 10.1039/DT9750001402|issue= 14 }} The reaction of chloride ions with {{chem2|TiCl4}} depends on the counterion. {{chem2|[N(CH2CH2CH2CH3)4]Cl}} and {{chem2|TiCl4}} gives the pentacoordinate complex {{chem2|[N(CH2CH2CH2CH3)4][TiCl5]}}, whereas smaller {{chem2|[N(CH2CH3)4]+}} gives {{chem2|[N(CH2CH3)4]2[Ti2Cl10]}}. These reactions highlight the influence of electrostatics on the structures of compounds with highly ionic bonding.

Reduction of {{chem2|TiCl4}} with aluminium results in one-electron reduction. The trichloride (Titanium(III) chloride) and tetrachloride have contrasting properties: the trichloride is a colored solid, being a coordination polymer, and is paramagnetic. When the reduction is conducted in THF solution, the Ti(III) product converts to the light-blue adduct {{chem2|TiCl3(THF)3}}.

{{Main|Organotitanium compound}}

The organometallic chemistry of titanium typically starts from {{chem2|TiCl4}}. An important reaction involves sodium cyclopentadienyl to give titanocene dichloride, {{chem2|TiCl2(C5H5)2}}. This compound and many of its derivatives are precursors to Ziegler–Natta catalysts. Tebbe's reagent, useful in organic chemistry, is an aluminium-containing derivative of titanocene that arises from the reaction of titanocene dichloride with trimethylaluminium. It is used for the "olefination" reactions.

Arenes, such as {{chem2|C6(CH3)6}} react to give the piano-stool complexes {{chem2|[Ti(C6R6)Cl3]+}} (R = H, {{chem2|CH3}}; see figure above). This reaction illustrates the high Lewis acidity of the {{chem2|TiCl3+}} entity, which is generated by abstraction of chloride from {{chem2|TiCl4}} by aluminium trichloride.{{cite journal|first1=F. |last1=Calderazzo |first2=I. |last2=Ferri |first3=G. |last3=Pampaloni |first4=S. |last4=Troyanov |title= η⁶-Arene Derivatives of Titanium(IV), Zirconium(IV) and Hafnium(IV)|journal=J. Organomet. Chem.| year=1996| volume=518|issue=1–2 | pages=189–196|doi= 10.1016/0022-328X(96)06194-3}}

{{chem2|TiCl4}} finds occasional use in organic synthesis, capitalizing on its Lewis acidity, its oxophilicity, and the electron-transfer properties of its reduced titanium halides. It is used in the Lewis acid catalysed aldol additionMariappan Periasamy (2002): "New synthetic methods using the TiCl4-NR3 reagent system", Arkivoc, p. 151-166. Key to this application is the tendency of {{chem2|TiCl4}} to activate aldehydes (RCHO) by formation of adducts such as {{chem2|(RCHO)TiCl4OC(H)R}}.{{cite encyclopedia|first1= L.-L. |last1=Gundersen |first2=F. |last2=Rise |first3=K. |last3=Undheim |encyclopedia=Encyclopedia of Reagents for Organic Synthesis| publisher = J. Wiley & Sons|year=2004 |title=Titanium(IV) chloride |editor-first =L. |editor-last=Paquette |location=New York, NY |doi=10.1002/047084289X.rt119.pub2}}

Hazards posed by titanium tetrachloride generally arise from its reaction with water that releases hydrochloric acid, which is severely corrosive itself and whose vapors are also extremely irritating. {{chem2|TiCl4}} is a strong Lewis acid, which exothermically forms adducts with even weak bases such as THF and water.

{{reflist|30em}}

• {{cite book|last1=Holleman |first1=A. F. |last2=Wiberg |first2=E. |title=Inorganic Chemistry |publisher=Academic Press |location=San Diego, CA |date=2001 |isbn=978-0-12-352651-9}}
• {{Greenwood&Earnshaw}}

• [http://www.epa.gov/ttn/atw/hlthef/titanium.html Titanium tetrachloride: Health Hazard Information]
• [http://webbook.nist.gov/chemistry/ NIST Standard Reference Database]
• [http://chemsub.online.fr/name/titanium_tetrachloride ChemSub Online: Titanium tetrachloride]

{{Titanium compounds}}

{{Chlorides}}

Category:Titanium(IV) compounds

Category:Chlorides

Category:Titanium halides

Category:Reagents for organic chemistry