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Titanium(II) chloride



Titanium(II) chloride is the chemical compound with the formula TiCl2. The black solid has been studied only moderately, probably because of its high reactivity.[1] Ti(II) is a strong reducing agent: it has a high affinity for oxygen and reacts irreversibly with water to produce H2. The usual preparation is the thermal disproportionation of TiCl3 at 500 °C. The equilibrium is "driven" by the loss of volatile TiCl4:

2 TiCl3 → TiCl2 + TiCl4

The method is similar to that for the conversion of VCl3 into VCl2 and VCl4.

TiCl2 crystallizes as the layered CdI2 structure. Thus, the Ti(II) centers are octahedrally coordinated to six chloride ligands.[2][3]

Derivatives

Molecular complexes are known such as TiCl2(chel)2, where chel is (CH3)2PCH2CH2P(CH3)2 and (CH3)2NCH2CH2N(CH3)2.[4] Such species are prepared by reduction of related Ti(III) and Ti(IV) complexes.

Unusual electronic effects have been observed in these species: TiCl2[(CH3)2PCH2CH2P(CH3)2]2 is paramagnetic with a triplet ground state, but Ti(CH3)2[(CH3)2PCH2CH2P(CH3)2]2 is diamagnetic.[5]

A solid-state derivative of TiCl2 is Na2TiCI4, which has been prepared by the reaction of Ti metal with TiCl3 in a NaCl flux.[6] This species adopts a linear chain structure wherein again the Ti(II) centers are octahedral with terminal, axial halides.[7]

References

  1. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  2. ^ Gal'perin, E. L.; Sandler, R. A. (1962). ""TiCI2"". Kristallografiya 7: 217-19..
  3. ^ Baenziger, N. C.; Rundle, R. E. (1948,). ""TiCI2" Acta Crystallographica" 1,: 274ff. doi:doi:10.1107/S0365110X48000740.
  4. ^ Girolami, G. S.; Wilkinson, G.; Galas, A. M. R.; Thornton-Pett, M.; Hursthouse, M. B. “Synthesis and properties of the divalent 1,2-bis(dimethylphosphino)ethane (dmpe) complexes MCl2(dmpe)2 and MMe2(dmpe)2 (M = Ti, V, Cr, Mn, or Fe). X-Ray crystal structures of MCl2(dmpe)2 (M = Ti, V, or Cr), MnBr2(dmpe)2, TiMe1.3Cl0.7(dmpe)2, and CrMe2(dmpe)2” Journal of the Chemical Society, Dalton Transactions, 1985, pages 1339 - 1348.
  5. ^ Jensen, J. A.; Wilson, S. R.; Schultz, A. J.; Girolami, G. S. (1987,). ""Divalent Titanium Chemistry. Synthesis, Reactivity, and X-ray and Neutron Diffraction Studies of Ti(BH4)2(dmpe)2 and Ti(CH3)2(dmpe)2,"". Journal of the American Chemical Societry 109,: 8094-5..
  6. ^ Hinz, D. J.; Dedecke, T.; Urland, W.; Meyer, G.. "“Synthese, Kristallstruktur und Magnetismus von Natriumtetrachlorotitanat(lI), Na2TiCI4”". Zeitschrift fur anorganische und allgemeine Chemie, 620,: 801-804..
  7. ^ Jongen, L.; Gloger, T.; Beekhuizen, J. and Meyer, G. (2005). "Divalent titanium: The halides ATiX3 (A = K, Rb, Cs; X = Cl, Br, I)". Zeitschrift für Anorganische und Allgemeine Chemie 631: 582-586. DOI}}
 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Titanium(II)_chloride". A list of authors is available in Wikipedia.
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