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TiCl 3 is produced usually by reduction of titanium(IV) chloride.Older reduction methods used hydrogen: [4]. 2 TiCl 4 + H 2 → 2 HCl + 2 TiCl 3. It can also be produced by the reaction of titanium metal and hot, concentrated hydrochloric acid; the reaction does not proceed at room temperature, as titanium is passivated against most mineral acids by a thin surface layer of titanium dioxide.
The McMurry reaction of benzophenone. The McMurry reaction is an organic reaction in which two ketone or aldehyde groups are coupled to form an alkene using a titanium chloride compound such as titanium(III) chloride and a reducing agent. The reaction is named after its co-discoverer, John E. McMurry.
Titanium(III) compounds are characteristically violet, illustrated by this aqueous solution of titanium trichloride. Titanium tetrachloride (titanium(IV) chloride, TiCl 4 [ 18 ] ) is a colorless volatile liquid (commercial samples are yellowish) that, in air, hydrolyzes with spectacular emission of white clouds.
The chloride process is used to separate titanium from its ores. The goal of the process is to win high purity titanium dioxide from ores such as ilmenite (FeTiO 3 ) and rutile (TiO 2 ). The strategy exploits the volatility of TiCl 4 , which is readily purified and converted to the dioxide.
Titanium products: plate, tube, rod, powder Pourbaix diagram for titanium in pure water, perchloric acid, or sodium hydroxide [26] Like aluminium and magnesium , the surface of titanium metal and its alloys oxidize immediately upon exposure to air to form a thin non-porous passivation layer that protects the bulk metal from further oxidation or ...
Compounds of titanium in the +2 oxidation state are rarer, examples being titanocene dicarbonyl and Ti(CH 3) 2 2. [Ti(CO) 6] 2− is formally a complex of titanium in the oxidation state of −2. [4] Although Ti(III) is involved in Ziegler–Natta catalysis, the organic derivatives of Ti(III) are uncommon. One example is the dimer [Cp 2 Ti III ...
Titanium trichloride (titanium(III) chloride), TiCl 3; Titanium dichloride (titanium(II) chloride), TiCl 2 This page was last edited on 20 October ...
Valid point. The article is reasonably well curated, but indeed many anhydrous compounds could explode if treated with water in some idiotic way. If we wrote to prevent idiocy, Wikipedia would be less useful.--Smokefoot 19:17, 4 January 2023 (UTC) Does the ferocity of the reaction depend on the quantity of TiCl 3 in