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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] 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. [12] 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. [22] Because of its high reactivity with oxygen, nitrogen, and many other gases, titanium that is evaporated from filaments is the basis for titanium sublimation pumps, in which titanium serves as a scavenger for these gases by chemically binding to them. Such pumps inexpensively produce extremely low pressures in ultra-high vacuum systems. See also: van Arkel–de Boer process Titanium (mineral concentrate) Basic titanium products: plate, tube, rods, and powder 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]

Titanium | Element, Meaning, Symbol, Density, Properties

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] The +4 oxidation state dominates titanium chemistry, [29] but compounds in the +3 oxidation state are also numerous. [30] Commonly, titanium adopts an octahedral coordination geometry in its complexes, [31] [32] but tetrahedral TiCl 4 is a notable exception. Because of its high oxidation state, titanium(IV) compounds exhibit a high degree of covalent bonding. [29] Oxides, sulfides, and alkoxides

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] Following the success of platinum-based chemotherapy, titanium(IV) complexes were among the first non-platinum compounds to be tested for cancer treatment. The advantage of titanium compounds lies in their high efficacy and low toxicity in vivo. [50] In biological environments, hydrolysis leads to the safe and inert titanium dioxide. Despite these advantages the first candidate compounds failed clinical trials due to insufficient efficacy to toxicity ratios and formulation complications. [50] Further development resulted in the creation of potentially effective, selective, and stable titanium-based drugs. [50] History Martin Heinrich Klaproth named titanium for the Titans of Greek mythology. FeTiO 3 + 7 Cl 2 + 6 C → 900 o C 2 FeCl 3 + 2 TiCl 4 + 6 CO {\displaystyle {\ce {2FeTiO3 + 7Cl2 + 6C ->[900 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]

ThoughtCo Chart of Common Charges of Chemical Elements - ThoughtCo

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 nitride (TiN) is a refractory solid exhibiting extreme hardness, thermal/electrical conductivity, and a high melting point. [39] TiN has a hardness equivalent to sapphire and carborundum (9.0 on the Mohs scale), [40] and is often used to coat cutting tools, such as drill bits. [41] It is also used as a gold-colored decorative finish and as a barrier layer in semiconductor fabrication. [42] Titanium carbide (TiC), which is also very hard, is found in cutting tools and coatings. [43] Halides Titanium(III) compounds are characteristically violet, illustrated by this aqueous solution of titanium trichloride.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 process After extensive purification by fractional distillation, the TiCl 4 is reduced with 800°C (1,470°F) molten magnesium in an argon atmosphere. [12] Titanium metal can be further purified by the van Arkel–de Boer process, which involves thermal decomposition of titanium tetraiodide. Titanium of very high purity was made in small quantities when Anton Eduard van Arkel and Jan Hendrik de Boer discovered the iodide process in 1925, by reacting with iodine and decomposing the formed vapors over a hot filament to pure metal. [59]

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Naturally occurring titanium is composed of five stable isotopes: 46Ti, 47Ti, 48Ti, 49Ti, and 50Ti, with 48Ti being the most abundant (73.8% natural abundance). At least 21 radioisotopes have been characterized, the most stable of which are 44Ti with a half-life of 63 years; 45Ti, 184.8 minutes; 51Ti, 5.76 minutes; and 52Ti, 1.7 minutes. All other radioactive isotopes have half-lives less than 33 seconds, with the majority less than half a second. [13]As a metal, titanium is recognized for its high strength-to-weight ratio. [12] It is a strong metal with low density that is quite ductile (especially in an oxygen-free environment), [7] lustrous, and metallic-white in color. [14] The relatively high melting point (1,668°C or 3,034°F) makes it useful as a refractory metal. It is paramagnetic and has fairly low electrical and thermal conductivity compared to other metals. [7] Titanium is superconducting when cooled below its critical temperature of 0.49K. [15] [16]