10049-06-6

Basic information

• Product Name: TITANIUM(II) CHLORIDE
• Synonyms: TiCl2;Titanium chloride (TiCl2);titaniumchloride(ticl2);TITANIUM(II) CHLORIDE;titanium dichloride;Titanium(II) chloride, anhydrous, powder, 99.98% metals basis;Titanium(II) dichloride
• CAS NO: 10049-06-6
• Molecular Formula: Cl2Ti
• Molecular Weight: 118.77
• EINECS: 233-164-9
• Product Categories: Crystal Grade Inorganics;Metal and Ceramic Science;Salts;Titanium Salts;TitaniumMetal and Ceramic Science
• Mol File: 10049-06-6.mol
• Article Data: 13

Chemical Properties

• Melting Point: 1035°
• Boiling Point: 1652.26°C (estimate)
• Flash Point: °C
• Appearance: /powder
• Density: 3.13
• Vapor Pressure: 33900mmHg at 25°C
• Water Solubility: decomposed by H2O evolving H2and forming TiCl3 [KIR83]; soluble alcohol; insoluble chloroform, ether, CS2 [MER06]
• Stability: Stability Pyrophoric. Reacts violently with water. Incompatible with strong oxidizing agents. May decompose upon exposure to air
• Merck: 13,9548
• CAS DataBase Reference: TITANIUM(II) CHLORIDE(CAS DataBase Reference)
• NIST Chemistry Reference: TITANIUM(II) CHLORIDE(10049-06-6)
• EPA Substance Registry System: TITANIUM(II) CHLORIDE(10049-06-6)

Safety Data

• Hazard Codes: F,C
• Statements: 14/15-17-34
• Safety Statements: 16-24-26-36/37/39-45
• RIDADR: UN 3200 4.2/PG 1
• WGK Germany: 3
• HazardClass: 4.2
• PackingGroup: I
• Hazardous Substances Data: 10049-06-6(Hazardous Substances Data)

Usage

Description

Titanium(II) chloride, also known as titanous chloride, is a black powdery chemical compound with the formula TiCl2. It is known for its hygroscopic nature, meaning it readily absorbs moisture from the environment. TITANIUM(II) CHLORIDE is sensitive to water and decomposes at a temperature of 475°C when heated in a vacuum. It is soluble in alcohol but remains insoluble in chloroform, ether, and carbon disulfide.

Uses

Used in Chemical Synthesis:
Titanium(II) chloride is used as a reducing agent in various chemical synthesis processes. Its strong reducing properties make it suitable for reducing metal ions and other compounds, facilitating the production of various chemicals and materials.
Used in Organic Synthesis:
In the field of organic chemistry, titanium(II) chloride is employed as a catalyst to promote specific reactions, such as the reductive amination of carbonyl compounds. Its ability to form stable complexes with organic substrates allows for selective transformations and improved reaction rates.
Used in Inorganic Synthesis:
Titanium(II) chloride is also utilized in the synthesis of inorganic compounds, particularly those containing titanium. It serves as a precursor for the formation of various titanium-based materials, such as pigments, catalysts, and ceramics.
Used in Analytical Chemistry:
Due to its reactivity with certain elements and compounds, titanium(II) chloride is used in analytical chemistry as a reagent for the detection and quantification of specific substances. Its ability to form colored complexes with certain metal ions makes it a valuable tool in colorimetric analysis.
Used in the Electronics Industry:
Titanium(II) chloride is employed in the electronics industry for the etching of semiconductor materials, such as silicon and gallium arsenide. Its selective etching properties allow for precise patterning and shaping of these materials, which is crucial for the fabrication of electronic devices and components.
Used in the Metallurgical Industry:
In the metallurgical industry, titanium(II) chloride is used for the extraction and purification of metals, particularly those with high melting points or those that are difficult to process using conventional methods. Its reducing properties enable the efficient recovery of valuable metals from their ores or secondary sources.
Used in the Textile Industry:
Titanium(II) chloride is utilized in the textile industry as a mordant, which helps to fix dyes onto fabrics during the dyeing process. Its ability to form stable complexes with dye molecules and the fabric material ensures colorfastness and improved resistance to fading.
Used in the Pharmaceutical Industry:
Although not explicitly mentioned in the provided materials, titanium(II) chloride has been investigated for its potential applications in the pharmaceutical industry, particularly as a reducing agent in the synthesis of various drugs and pharmaceutical compounds. Its unique chemical properties may offer advantages in specific synthesis pathways, leading to more efficient production processes and improved drug formulations.

Hazard

Flammable, dangerous fire risk, ignites in air, store under water or inert gas.

InChI:InChI=1/2ClH.Ti/h2*1H;/q;;+2/p-2

Upstream product

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Downstream Products

• 16043-45-1 titanium(IV) 

Relevant articles and documents

Direct epimetallation of π-bonded organic substrates with titanium(II) isopropoxide: Intermediacy of biradical, oligomeric titanium(II) reagents

Extensive EPR experiments show that a titanium-containing molecular triplet state is formed in solution by the reaction of two equivalents of butyllithium with one equivalent of titanium(IV) isopropoxide. At higher concentrations this product, titanium(II) isopropoxide, admixed with two equivalents of lithium isopropoxide, is accompanied by the formation of a variety of nontitanium-containing side products. The powder EPR spectrum of the molecular triplet state in frozen solution is consistent with an asymmetric molecular chain of three Ti centers on which the unpaired electron centers are three metal atoms apart. Dilution experiments show that at lower concentrations, where the nontitanium-containing side products have dissipated, the intensity of the molecular triplet spectrum varies approximately linearly with concentration. Thus there is no evidence that the observed triplet molecule is one component in a series of concentration-dependent oligomerization steps. The bulky isopropoxy substituents and the coordination of the isopropoxide anions from the LiOiPr present appear to prevent closure of the Ti3 centers into an equilateral triangular diamagnetic structure. This steric hindrance, operative at the terminal diisopropoxytitanium centers and preventing closure to a ring, seems not to be observed with TiCl2·2THF, which is diamagnetic and may thus be expected to exist as an equilateral triangular cluster of three units of TiCl2·2THF, a structural model currently under further investigation. The smaller steric demand of the chloro and THF units would seem to permit octahedral coordination about each Ti center in such an equilateral trigonal array of Ti3 atoms. Chemical reactions carried out individually with diphenylacetylene, cis-stilbene or cis-stilbene oxide and titanium(II) diisopropoxide provide stoichiometric and stereochemical evidence that the attacking titanium(II) reagent is in fact the trimeric biradical. The role of the lithium isopropoxide byproduct in fostering the course of the previously reported SET reactions of titanium(II) isopropoxide and in determining the detailed structure of the open-chain Ti trimer biradical has been explicated. Wiley-VCH Verlag-GmbH & Co. KGaA, 2006.

Structural studies of the low-valent titanium "Solution": What goes on in the pinacol coupling reaction? [3]

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Gaseous Species in the Ti-Al-Cl System and Reaction with H2O

Chemical species in the Ti-Al-Cl system at elevated temperatures were studied by effusion-beam mass spectrometry up to 1400 K.Gaseous TiAlCl5 and TiAlCl6 were identified as products of the reaction of TiCl4(g) and a Ti-Al mixture above about 900 K, for which AlCl3, TiCl2, and TiCl3 were also present.No evidence was found for TiAlCl7.When gaseous TiCl4, AlCl3, and H2O and admitted simultaneously, TiOCl2, Al(OH)Cl2, and TiAl(OH)Cl5 were observed.All ion species showed the correct isotopic distribution.The results confirm earlier indications that AlCl3 forms gaseous complexes with divalent and trivalent Ti, but not with tetravalent Ti.

Fundamental study on synthesis and enrichment of titanium subchloride

In order to establish a new high-speed/(semi-)continuous titanium production process based on the magnesiothermic reduction of titanium subchlorides (subhalide reduction process), a novel synthetic process for obtaining titanium subchlorides (TiClx, x = 2, 3) by the reaction of titanium tetrachloride (TiCl4) with titanium metal at 1273 K was investigated. It was demonstrated that the efficiency of the TiClx formation improved drastically when molten salts were used as the reaction medium as compared with that of the synthesis by employing the direct reaction of TiCl4 gas with solid titanium. The feasibility of the enrichment process of TiClx in molten salt was also demonstrated. The method for producing the titanium subchlorides investigated in this study can be applied to the new high-speed production process of titanium.