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| Identifiers | |
|---|---|
3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.030.137 |
| EC Number |
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| UNII | |
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| Properties | |
| Cl2Ti | |
| Molar mass | 118.77 g·mol−1 |
| Appearance | blackhexagonal 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] | |
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| 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 theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Titanium(II) chloride is thechemical compound with theformula 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 thermaldisproportionation ofTiCl3 at 500 °C. The reaction is driven by the loss of volatileTiCl4:
The method is similar to that for the conversion ofVCl3 intoVCl2 andVCl4.
TiCl2 crystallizes as the layeredCdI2 structure. Thus, the Ti(II) centers are octahedrally coordinated to six chloride ligands.[3][4]
Molecular complexes are known such as TiCl2(chel)2, where chel isDMPE (CH3)2PCH2CH2P(CH3)2 andTMEDA ((CH3)2NCH2CH2N(CH3)2).[5] Such species are prepared by reduction of related Ti(III) and Ti(IV) complexes.
Unusualelectronic effects have been observed in these species: TiCl2[(CH3)2PCH2CH2P(CH3)2]2 is paramagnetic with a tripletground 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 NaClflux.[7] This species adopts a linear chain structure wherein again the Ti(II) centers are octahedral with terminal, axial halides.[8]
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