Titanium (II) chloride
Crystal structure | ||||||||||||||||
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__ Ti 2+ __ Cl - | ||||||||||||||||
General | ||||||||||||||||
Surname | Titanium (II) chloride | |||||||||||||||
other names |
Titanium dichloride |
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Ratio formula | TiCl 2 | |||||||||||||||
Brief description |
black, self-igniting solid |
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External identifiers / databases | ||||||||||||||||
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properties | ||||||||||||||||
Molar mass | 118.79 g mol −1 | |||||||||||||||
Physical state |
firmly |
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density |
3.13 g cm −3 |
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Melting point |
1035 ° C |
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boiling point |
1500 ° C |
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solubility |
Decomposes in water |
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safety instructions | ||||||||||||||||
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As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Titanium (II) chloride is a chemical compound of titanium from the group of chlorides .
Extraction and presentation
Titanium (II) chloride is usually obtained by thermal disproportionation of titanium (III) chloride at 500 ° C, although this method does not result in the decomposition reaction of titanium ( II) chloride to titanium (IV) chloride and titanium already taking place pure product can be obtained and this always contains 2-3% free titanium.
Titanium (II) chloride can also be obtained by reacting titanium with titanium (IV) chloride.
Titanium (II) chloride can be obtained in a very pure and finely divided form by reducing titanium (IV) chloride with hydrogen in an electrodeless electrical discharge.
properties
Titanium (II) chloride is a strong reducing agent (reacts violently with water and oxygen) and has a layered Cadmiumdiiodid - crystal structure , wherein the titanium (II) octahedrally to six chloride ligands is positioned. It forms with derivatives or complex compounds in the TiCl 2 (R) 2, where R can be a chelate (e.g. dppe or TMEDA ) or a salt (e.g. sodium chloride ). It has a trigonal crystal structure of the cadmium (II) iodide type ( polytype 2H) with the space group P 3 m 1 (space group no.164) and the lattice parameters a = 356.1, c = 587.5 pm.
use
Titanium (II) chloride can be used for the production of pure titanium and as a mediator in organic syntheses.
safety instructions
Titanium (II) chloride is spontaneously flammable (depends, among other things, on the grain size) and forms extremely flammable gases on contact with water or moist air. The reaction with water is violent.
Individual evidence
- ↑ a b c d e f entry to titanium (II) chloride in the GESTIS database of IFA , retrieved on July 23, 2016(JavaScript required) .
- ↑ data sheet at WebElements (English)
- ↑ a b c d Georg Brauer (Ed.), With the collaboration of Marianne Baudler a . a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 1334.
- ↑ EL Gal'perin, RA Sandler: TiCl 2 . In: Kristallografiya. 1962, 7, pp. 217-219.
- ↑ NC Baenziger, RE Rundle: The structure of TiCl 2 . In: Acta Crystallographica. 1948, 1, p. 274-, doi : 10.1107 / S0365110X48000740 .