Editing Titanium tetrachloride (section)

==Properties and structure==
{{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|{{chem2|VCl4}}]] being another example. This property reflects the fact that molecules of {{chem2|TiCl4}} weakly self-associate. Most metal chlorides are [[polymer]]s, wherein the chloride atoms bridge between the metals. Its [[melting point]] is similar to that of [[Carbon tetrachloride|{{chem2|CCl4}}]].<ref name="Earnshaw1997">{{cite book|last1=Earnshaw|first1=A.|last2=Greenwood|first2=N.|year=1997|title=Chemistry of the Elements|edition=2nd|publisher=[[Butterworth-Heinemann]]}}</ref><ref name="ullmann" />

{{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 d<sup>0</sup> metal center ({{chem2|Ti(4+)}}) surrounded by four identical ligands. This configuration leads to highly [[symmetry|symmetrical]] structures, hence the tetrahedral shape of the molecule. {{chem2|TiCl4}} adopts similar structures to [[Titanium tetrabromide|{{chem2|TiBr4}}]] and [[Titanium tetraiodide|{{chem2|TiI4}}]]; 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}}.<ref>{{cite journal|first1= S. P. |last1=Webb |first2=M. S. |last2=Gordon |title= Intermolecular Self-Interactions of the Titanium Tetrahalides TiX<sub>4</sub> (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}}</ref>

{{chem2|TiCl4}} is soluble in [[toluene]] and [[chlorocarbon]]s. Certain [[arene]]s form complexes of the type {{chem2|[(C6R6)TiCl3]+}}.<ref name="TiCplx" /> {{chem2|TiCl4}} reacts [[exothermic]]ally with donor [[solvent]]s such as [[THF]] to give hexacoordinated [[adduct]]s.<ref>{{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}}</ref> Bulkier [[ligand]]s (L) give pentacoordinated [[adduct]]s {{chem2|TiCl4L}}.