Titanium tetraiodide
Names | |
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IUPAC name
Titanium(IV) iodide
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Other names
Titanium tetraiodide
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Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.028.868 |
EC Number |
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PubChem CID
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CompTox Dashboard (EPA)
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Properties | |
TiI4 | |
Molar mass | 555.485 g/mol |
Appearance | red-brown crystals |
Density | 4.3 g/cm3 |
Melting point | 150 °C (302 °F; 423 K) |
Boiling point | 377 °C (711 °F; 650 K) |
hydrolysis | |
Solubility in other solvents | soluble in CH2Cl2 CHCl3 CS2 |
Structure | |
cubic (a = 12.21 Å) | |
tetrahedral | |
0 D | |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
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violent hydrolysis corrosive |
GHS labelling:[1] | |
Danger | |
H314 | |
P260, P264, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P405, P501 | |
Related compounds | |
Other anions
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Titanium(IV) fluoride
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Other cations
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Silicon tetraiodide Zirconium(IV) iodide Hafnium(IV) iodide |
Related compounds
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Titanium(III) iodide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Titanium tetraiodide is an inorganic compound with the formula TiI4. It is a black volatile solid, first reported by Rudolph Weber in 1863.[2] It is an intermediate in the van Arkel–de Boer process for the purification of titanium.
Physical properties
TiI4 is a rare molecular binary metal iodide, consisting of isolated molecules of tetrahedral Ti(IV) centers. The Ti-I distances are 261
Two
Production
Three methods are well known: 1) From the elements, typically using a tube furnace at 425 °C:[4]
- Ti + 2 I2 → TiI4
This reaction can be reversed to produce highly pure films of Ti metal.[5]
2) Exchange reaction from titanium tetrachloride and HI.
- TiCl4 + 4 HI → TiI4 + 4 HCl
3) Oxide-iodide exchange from aluminium iodide.
- 3 TiO2 + 4 AlI3 → 3 TiI4 + 2 Al2O3
Reactions
Like TiCl4 and TiBr4, TiI4 forms adducts with Lewis bases, and it can also be reduced. When the reduction is conducted in the presence of Ti metal, one obtains polymeric Ti(III) and Ti(II) derivatives such as CsTi2I7 and the chain CsTiI3, respectively.[6]
TiI4 exhibits extensive reactivity toward alkenes and alkynes resulting in organoiodine derivatives. It also effects
References
- ^ "Titanium tetraiodide". pubchem.ncbi.nlm.nih.gov. Retrieved 12 December 2021.
- ^ Weber, R. (1863). "Ueber die isomeren Modificationen der Titansäure und über einige Titanverbindungen". .
- ^ a b Tornqvist, E. G. M.; Libby, W. F. (1979). "Crystal Structure, Solubility, and Electronic Spectrum of Titanium Tetraiodide". .
- ^
Lowry, R. N.; Fay, R. C. (1967). "Titanium(IV) Iodide". Inorganic Syntheses. Vol. 10. pp. 1–6. ISBN 978-0-470-13241-8.
- ^ Blumenthal, W. B.; Smith, H. (1950). "Titanium tetraiodide, Preparation and Refining". .
- ^ Jongen, L.; Gloger, T.; Beekhuizen, J.; Meyer, G. (2005). "Divalent Titanium: The Halides ATiX3 (A = K, Rb, Cs; X = Cl, Br, I)". .
- ^ Shimizu, M.; Hachiya, I. (2014). "Chemoselective Reductions and Iodinations using Titanium Tetraiodide". Tetrahedron Letters. 55 (17): 2781–2788. .