Titanium(IV) hydride (systematically named titanium tetrahydride) is an inorganic compound with the empirical chemical formula TiH
4. It has not yet been obtained in bulk, hence its bulk properties remain unknown. However, molecular titanium(IV) hydride has been isolated in solid gas matrices. The molecular form is a colourless gas, and very unstable toward thermal decomposition. As such the compound is not well characterised, although many of its properties have been calculated via computational chemistry.
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| Names | |||
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| Systematic IUPAC name
Titanium(IV) hydride | |||
| Other names
Titanium tetrahydride
Titane TiH4 | |||
| Identifiers | |||
3D model (JSmol)
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| ECHA InfoCard | 100.035.414 | ||
| EC Number |
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PubChem CID
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| UN number | 1871 | ||
CompTox Dashboard (EPA)
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| Properties | |||
| TiH4 | |||
| Molar mass | 51.899 g/mol | ||
| Appearance | Colourless gas | ||
| Reacts | |||
| Related compounds | |||
Other anions
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Titanium(IV) fluoride Titanium(IV) chloride Titanium(IV) bromide Titanium(IV) iodide | ||
Other cations
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Methane Silane Germane Stannane Plumbane | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Synthesis and stability
editTitanium(IV) hydride was first produced in 1963 by the photodissociation of mixtures of TiCl4 and H2, followed by immediate mass spectrometry.[1] Rapid analysis was required as titanium(IV) hydride is extremely unstable. Computational analysis of TiH4 has given a theoretical bond dissociation energy (relative to M+4H) of 132 kcal/mole.[2] As the dissociation energy of H2 is 104 kcal/mole the instability of TiH4 can be expected to be thermodynamic; with it dissociating to metallic titanium and hydrogen:
- TiH4 → Ti + 2 H2 (76 kcal/mole)
TiH4, along with other unstable molecular titanium hydrides, (TiH, TiH2, TiH3 and polymeric species) has been isolated at low temperature following laser ablation of titanium.[3]
Structure
editIt is suspected that within solid titanium(IV) hydride, the molecules form aggregations (polymers), being connected by covalent bonds.[4] Calculations suggest that TiH4 is prone to dimerisation.[3] This largely attributed to the electron deficiency of the monomer and the small size of the hydride ligands; which allows dimerisation to take place with a very low energy barrier as there is a negligible increase in inter-ligand repulsion.
The dimer is a calculated to be a fluxional molecule rapidly inter-converting between a number of forms, all of which display bridging hydrogens.[4] This is an example of three-center two-electron bonding.
Monomeric titanium(IV) hydride is the simplest transition metal molecule that displays sd3 orbital hybridisation.[5]
References
edit- ^ Breisacher, Peter; Siegel, Bernard (5 June 1963). "Formation of Gaseous Titanium(IV) Hydride and Chlorohydrides of Titanium". Journal of the American Chemical Society. 85 (11): 1705–1706. doi:10.1021/ja00894a049.
- ^ Hood, Diane M.; Pitzer, Russell M.; Schaefer, Henry F. (1 January 1979). "Electronic structure of homoleptic transition metal hydrides: TiH4, VH4, CrH4, MnH4, FeH4, CoH4, and NiH4". The Journal of Chemical Physics. 71 (2): 705. Bibcode:1979JChPh..71..705H. doi:10.1063/1.438357.
- ^ a b Chertihin, George V.; Andrews, Lester (September 1994). "Reactions of laser ablated Ti atoms with hydrogen during condensation in excess argon. Infrared spectra of the TiH, TiH2, TiH3, and TiH4 molecules". Journal of the American Chemical Society. 116 (18): 8322–8327. doi:10.1021/ja00097a045.
- ^ a b Webb, Simon P.; Gordon, Mark S. (July 1995). "The dimerization of TiH
4". Journal of the American Chemical Society. 117 (27): 7195–7201. doi:10.1021/ja00132a020. - ^ Jonas, V.; Boehme, C.; Frenking, G. (1996). "Bent's Rule and the Structure of Transition Metal Compounds". Inorg. Chem. 35 (7): 2097–2099. doi:10.1021/ic951397o.