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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.
Titanium tetrachloride has been used to create naval smokescreens, as the hydrochloric acid aerosol and titanium dioxide that is formed scatter light very efficiently. This smoke is corrosive, however. [10] Alcohols react with TiCl 4 to give alkoxides with the formula [Ti(OR) 4] n (R = alkyl, n = 1, 2, 4).
Group 4 is the second group of transition metals in the periodic table. It contains only the four elements titanium (Ti), zirconium (Zr), hafnium (Hf), and rutherfordium (Rf). ). The group is also called the titanium group or titanium family after its lightest me
Because this reaction is highly exothermic (238 kJ/mol), the temperature is monitored, to guard against thermal degradation of the catalyst. The reaction is as follows: CH 2 =CH 2 + 2 CuCl 2 → 2 CuCl + ClH 2 C-CH 2 Cl. The copper(II) chloride is regenerated by sequential reactions of the cuprous chloride with oxygen and then hydrogen chloride:
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 readily reacts with oxygen at 1,200 °C (2,190 °F) in air, and at 610 °C (1,130 °F) in pure oxygen, forming titanium dioxide. [17] Titanium is one of the few elements that burns in pure nitrogen gas, reacting at 800 °C (1,470 °F) to form titanium nitride , which causes embrittlement. [ 29 ]