Titanium (IV) sulfide

Crystal structure
	__ Ti 4+ __ S 2−00
General
Surname	Titanium (IV) sulfide
Ratio formula	TiS 2
Brief description	green powder with a rotten egg smell
External identifiers / databases
EC number	234-883-0
ECHA InfoCard	100,031,699
PubChem	61544
Wikidata	Q4445889
properties
Molar mass	112.01 g mol −1
Physical state	firmly
density	3.22 g cm −3
solubility	reacts with water releasing hydrogen sulfide
safety instructions
GHS labeling of hazardous substances Caution
H and P phrases	H: 261-315-319-335
	EUH: 031
	P: 231 + 232-302 + 352-305 + 351 + 338-231-405-501
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Titanium (IV) sulfide or titanium disulfide is a chemical compound from the group of sulfides with the formula Ti S ₂ .

presentation

Titanium disulfide can be produced from titanium tetrachloride TiCl ₄ and hydrogen sulfide H ₂ S.

{\ displaystyle \ mathrm {TiCl_ {4} +2 \ H_ {2} S \ longrightarrow TiS_ {2} +4 \ HCl}}

Synthesis from the elements is also possible.

{\ displaystyle \ mathrm {Ti + 2 \ S \ longrightarrow TiS_ {2}}}

properties

Titanium disulfide is a bronze colored, diamagnetic crystalline powder. The crystals have a layered structure, namely the cadmium iodide structure. The sulfur atoms are arranged in a hexagonal closest packing of spheres. The titanium ions occupy the octahedral gaps between each anion layer after that.

The connection is sensitive to moisture. Contact with water, but especially with aqueous acids, leads to hydrolysis and the formation of hydrogen sulfide and titanium dioxide . Due to its sulphide content, the substance is flammable, producing sulfur dioxide gas. It is air-resistant at room temperature, but changes to titanium dioxide when heated in air. It is decomposed by nitric acid and hot concentrated sulfuric acid with sulfur separation. It is dissolved by boiling caustic soda and potassium hydroxide to form alkali titanate and alkali sulfide.

Titanium disulfide has an electrical conductivity that corresponds to that of a semimetal , which when used in batteries has the advantage that no substances such as e.g. B. Soot must be added to increase conductivity.

Titanium disulfide (like graphite, for example) can reversibly store lithium in its layer structure ( intercalation ), with Li _x TiS _{2 being} formed, with x between 0 and 1. N bases such as NH3, N2H4, acid amides can also be stored .

use

Titanium disulfide is used as a solid lubricant. It can also be used as an electrode material in lithium batteries or lithium-ion accumulators , the low atomic weight of titanium being an advantage.

Individual evidence

↑ ^a ^b ^c ^d ^e data sheet titanium (IV) sulfide from AlfaAesar, accessed on 23 August 2011 ( PDF )(JavaScript required) .
^ ^A ^b ^c A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 91st – 100th, improved and greatly expanded edition. Walter de Gruyter, Berlin 1985, ISBN 3-11-007511-3 , p. 1065.
↑ ^a ^b ^c 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. 1371.
^ Entry on titanium (IV) sulfide at ChemicalBook , accessed on September 19, 2011.
^ MS Whittingham: Lithium Batteries and Cathode Materials , Chem. Rev. 104 (2004) 4273

[Alfa-1] ↑ ^a ^b ^c ^d ^e data sheet titanium (IV) sulfide from AlfaAesar, accessed on 23 August 2011 ( PDF )(JavaScript required) .

[Holleman-2] A ^b ^c A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 91st – 100th, improved and greatly expanded edition. Walter de Gruyter, Berlin 1985, ISBN 3-11-007511-3 , p. 1065.

[brauer-3] 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. 1371.

[4] Entry on titanium (IV) sulfide at ChemicalBook , accessed on September 19, 2011.

[5] MS Whittingham: Lithium Batteries and Cathode Materials , Chem. Rev. 104 (2004) 4273