Titanium(II) chloride

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Titanium(II) chloride
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
100.030.137 Edit this at Wikidata
EC Number
  • 233-164-9
UNII
  • InChI=1S/2ClH.Ti/h2*1H;/q;;+2/p-2 checkY
    Key: ZWYDDDAMNQQZHD-UHFFFAOYSA-L checkY
  • InChI=1/2ClH.Ti/h2*1H;/q;;+2/p-2
    Key: ZWYDDDAMNQQZHD-NUQVWONBAH
  • [Ti+2].[Cl-].[Cl-]
Properties
Cl2Ti
Molar mass 118.77 g·mol−1
Appearance black
hexagonal
crystals
Density 3.13 g/cm3
Melting point 1,035 °C (1,895 °F; 1,308 K)
Boiling point 1,500 °C (2,730 °F; 1,770 K)
+570.0·10−6 cm3/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
pyrophoric
GHS labelling:[1]
GHS02: FlammableGHS05: Corrosive
Danger
H250, H314
P210, P222, P260, P264, P280, P301+P330+P331, P302+P334, P303+P361+P353, P304+P340, P305+P351+P338, P310, P363, P370+P378, P405, P422
Safety data sheet (SDS) External MSDS
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(II) chloride is the chemical compound with the formula TiCl2. The black solid has been studied only moderately, probably because of its high reactivity.[2] 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 reaction is driven by the loss of volatile TiCl4:

2 TiCl3 → TiCl2 + TiCl4

The method is similar to that for the conversion of

VCl4
.

TiCl2 crystallizes as the layered CdI2 structure. Thus, the Ti(II) centers are octahedrally coordinated to six chloride ligands.[3][4]

Derivatives

Molecular complexes are known such as TiCl2(chel)2, where chel is

TMEDA ((CH3)2NCH2CH2N(CH3)2).[5]
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.[6]

A solid-state derivative of TiCl2 is Na2TiCl4, which has been prepared by the reaction of Ti metal with TiCl3 in a NaCl flux.[7] This species adopts a linear chain structure wherein again the Ti(II) centers are octahedral with terminal, axial halides.[8]

References

  1. ^ "Titanium dichloride". pubchem.ncbi.nlm.nih.gov. Retrieved 12 December 2021.
  2. .
  3. ^ Gal'perin, E. L.; Sandler, R. A. (1962). "TiCI2". Kristallografiya. 7: 217–19.
  4. .
  5. doi:10.1039/dt9850001339.{{cite journal}}: CS1 maint: multiple names: authors list (link
    )
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