Ion Color Brilliance Brights Semi-Permanent Hair Color Titanium by Ion

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The metal is a dimorphic allotrope of an hexagonal α form that changes into a body-centered cubic (lattice) β form at 882°C (1,620°F). [18] The specific heat of the α form increases dramatically as it is heated to this transition temperature but then falls and remains fairly constant for the β form regardless of temperature. [18] Chemical properties Pourbaix diagram for titanium in pure water, perchloric acid, or sodium hydroxide [19]

Ion induced effects and defects on surface, structural and Ion induced effects and defects on surface, structural and

The isotopes of titanium range in atomic weight from 39.002 u ( 39Ti) to 63.999 u ( 64Ti). [28] The primary decay mode for isotopes lighter than 46Ti is positron emission (with the exception of 44Ti which undergoes electron capture), leading to isotopes of scandium, and the primary mode for isotopes heavier than 50Ti is beta emission, leading to isotopes of vanadium. [13]The term titanates usually refers to titanium(IV) compounds, as represented by barium titanate (BaTiO 3). With a perovskite structure, this material exhibits piezoelectric properties and is used as a transducer in the interconversion of sound and electricity. [12] Many minerals are titanates, such as ilmenite (FeTiO 3). Star sapphires and rubies get their asterism (star-forming shine) from the presence of titanium dioxide impurities. [20] Commercially pure (99.2% pure) grades of titanium have ultimate tensile strength of about 434 MPa (63,000 psi), equal to that of common, low-grade steel alloys, but are less dense. Titanium is 60% denser than aluminium, but more than twice as strong [11] as the most commonly used 6061-T6 aluminium alloy. Certain titanium alloys (e.g., Beta C) achieve tensile strengths of over 1,400MPa (200,000psi). [17] However, titanium loses strength when heated above 430°C (806°F). [18] Common titanium-containing minerals are anatase, brookite, ilmenite, perovskite, rutile, and titanite (sphene). [20] Akaogiite is an extremely rare mineral consisting of titanium dioxide. Of these minerals, only rutile and ilmenite have economic importance, yet even they are difficult to find in high concentrations. About 6.0 and 0.7 million tonnes of those minerals were mined in 2011, respectively. [24] Significant titanium-bearing ilmenite deposits exist in Australia, Canada, China, India, Mozambique, New Zealand, Norway, Sierra Leone, South Africa, and Ukraine. [20] About 210,000 tonnes of titanium metal sponge were produced in 2020, mostly in China (110,000 t), Japan (50,000 t), Russia (33,000 t) and Kazakhstan (15,000 t). Total reserves of anatase, ilmenite, and rutile are estimated to exceed 2 billion tonnes. [24] 2017 production of titanium minerals and slag [24] Country Titanium can be alloyed with iron, aluminium, vanadium, and molybdenum, among other elements, to produce strong, lightweight alloys for aerospace ( jet engines, missiles, and spacecraft), military, industrial processes (chemicals and petrochemicals, desalination plants, pulp, and paper), automotive, agriculture (farming), medical prostheses, orthopedic implants, dental and endodontic instruments and files, dental implants, sporting goods, jewelry, mobile phones, and other applications. [7] See also: van Arkel–de Boer process Titanium (mineral concentrate) Basic titanium products: plate, tube, rods, and powder

Titanium - Element information, properties and uses

The alkoxides of titanium(IV), prepared by treating TiCl 4 with alcohols, are colorless compounds that convert to the dioxide on reaction with water. They are industrially useful for depositing solid TiO 2 via the sol-gel process. Titanium isopropoxide is used in the synthesis of chiral organic compounds via the Sharpless epoxidation. [37]Around the same time, Franz-Joseph Müller von Reichenstein produced a similar substance, but could not identify it. [9] The oxide was independently rediscovered in 1795 by Prussian chemist Martin Heinrich Klaproth in rutile from Boinik (the German name of Bajmócska), a village in Hungary (now Bojničky in Slovakia). [51] [a] FeTiO 3 + 7 Cl 2 + 6 C → 900 o C 2 FeCl 3 + 2 TiCl 4 + 6 CO {\displaystyle {\ce {2FeTiO3 + 7Cl2 + 6C ->[900

Titanium (Ti2+,Ti3+,Ti4+ ions) Electron Configuration for Titanium (Ti2+,Ti3+,Ti4+ ions)

The two most useful properties of the metal are corrosion resistance and strength-to-density ratio, the highest of any metallic element. [10] In its unalloyed condition, titanium is as strong as some steels, but less dense. [11] There are two allotropic forms [12] and five naturally occurring isotopes of this element, 46Ti through 50Ti, with 48Ti being the most abundant (73.8%). [13] Characteristics Physical properties Titanium tetrachloride (titanium(IV) chloride, TiCl 4 [44]) is a colorless volatile liquid (commercial samples are yellowish) that, in air, hydrolyzes with spectacular emission of white clouds. Via the Kroll process, TiCl 4 is used in the conversion of titanium ores to titanium metal. Titanium tetrachloride is also used to make titanium dioxide, e.g., for use in white paint. [45] It is widely used in organic chemistry as a Lewis acid, for example in the Mukaiyama aldol condensation. [46] In the van Arkel–de Boer process, titanium tetraiodide (TiI 4) is generated in the production of high purity titanium metal. [47] The currently known processes for extracting titanium from its various ores are laborious and costly; it is not possible to reduce the ore by heating with carbon (as in iron smelting) because titanium combines with the carbon to produce titanium carbide. [51] Pure metallic titanium (99.9%) was first prepared in 1910 by Matthew A. Hunter at Rensselaer Polytechnic Institute by heating TiCl 4 with sodium at 700–800°C (1,292–1,472°F) under great pressure [57] in a batch process known as the Hunter process. [8] Titanium metal was not used outside the laboratory until 1932 when William Justin Kroll produced it by reducing titanium tetrachloride (TiCl 4) with calcium. [58] Eight years later he refined this process with magnesium and with sodium in what became known as the Kroll process. [58] Although research continues to seek cheaper and more efficient routes, such as the FFC Cambridge process, the Kroll process is still predominantly used for commercial production. [8] [9] Titanium "sponge", made by the Kroll processTitanium is a chemical element with the symbol Ti and atomic number 22. Found in nature only as an oxide, it can be reduced to produce a lustrous transition metal with a silver color, low density, and high strength, resistant to corrosion in sea water, aqua regia, and chlorine.