Titanium (III) bromide
Crystal structure | |||||||||||||
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__ Ti 3+ __ Br - | |||||||||||||
General | |||||||||||||
Surname | Titanium (III) bromide | ||||||||||||
other names |
Titanium tribromide |
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Ratio formula | TiBr 3 | ||||||||||||
Brief description |
black-blue solid |
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External identifiers / databases | |||||||||||||
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properties | |||||||||||||
Molar mass | 287.58 g mol −1 | ||||||||||||
Physical state |
firmly |
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density |
4.24 g cm −3 |
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Melting point |
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solubility |
soluble 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 (III) bromide is an inorganic chemical compound of titanium from the group of bromides .
Extraction and presentation
Titanium (III) bromide can be produced by reacting titanium (IV) bromide with hydrogen
or obtained directly from the elements.
The hexahydrate can be prepared by reducing titanium (IV) bromide in a hydrochloric acid solution, which precipitates when the solution is saturated with hydrobromic acid .
properties
Titanium (III) bromide is available as black-blue, transparent blue-green crystals, which are soluble in water and decompose at 550 ° C into titanium (II) bromide and titanium (IV) bromide. Titanium (III) bromide occurs in two different crystal structures, the alpha form being the trigonal form of titanium (III) chloride with the space group R 3 (space group no.146) (a = 640 pm , c = 1870 pm) corresponds. The hexahydrate, which also exists, is a reddish-purple crystalline solid that melts at 115 ° C and decomposes at 400 ° C. It is soluble in water, methanol , ethanol and acetone , but insoluble in carbon tetrachloride and benzene .
Individual evidence
- ↑ a b c d e f g h i j Georg Brauer (Ed.), With the collaboration of Marianne Baudler u. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , pp. 1341ff.
- ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
- ^ Jean D'Ans, Ellen Lax: Pocket book for chemists and physicists . Springer DE, 1997, ISBN 3-540-60035-3 , pp. 766 ( limited preview in Google Book search).