7440-32-6 Usage
Uses
Used in Aerospace Industry:
Titanium is used as a structural material for constructing aircraft, jet engines, and missiles due to its strength, resistance to corrosion, and low density.
Used in Armor Plating:
Titanium is used as armor plates for tanks and warships because of its strength and resistance to corrosion.
Used in Stealth Aircraft:
Titanium is the major metal used for constructing stealth aircraft that are difficult to detect by radar.
Used in Medical Equipment:
Titanium's noncorrosive and lightweight properties make it useful in the manufacture of laboratory and medical equipment that will withstand acid and halogen salt corrosion.
Used in Surgical Applications:
Titanium is used as surgical pins and screws in the repair of broken bones and joints due to its noncorrosive and lightweight properties.
Used in Titanium Bronze:
Titanium is alloyed with copper and iron in titanium bronze to enhance its properties.
Used in Steel and Aluminum:
Titanium is added to steel and aluminum to enhance their tensile strength and acid resistance.
Used in Incandescent Lamps:
Titanium is used to remove traces of oxygen and nitrogen from incandescent lamps.
Used in Cement and Paint Industries:
Titanium is used as an ingredient in cements and as a paint pigment in the oxide form.
Used in Paper and Ink Industries:
Titanium is used in the paper and ink industries due to its properties.
Used in Batteries for Space Vehicles:
Titanium is used in batteries for space vehicles because of its resistance to chlorine (seawater) corrosion.
Physical Properties:
Titanium is a white lustrous metal that is ductile when free of oxygen. It has a low density and high strength. Titanium has two allotropic modifications: the alpha form with a close-packed hexagonal crystal structure and the beta modification with a body-centered cubic structure. The metal melts at 1,610 ±10°C and vaporizes at 3,287°C. It has an electrical resistivity of 42 microhm-cm and a modulus of elasticity of 15.5x10^6 psi at 25°C. Titanium is insoluble in water but soluble in dilute acids.
History, Occurrence and Uses
Titanium was discovered in 1790 by English chemist William Gregor. Five years later in 1795, Klaproth confirmed Gregor’s findings from his independent investigation and named the element titanium after the Latin name Titans, the mythical first sons of the Earth. The metal was prepared in impure form first by Nilson and Pettersson in 1887. Hunter, in 1910, prepared the metal in pure form by reducing titanium tetrachloride with sodium.
Titanium occurs in nature in the minerals rutile( TiO2), ilmenite (FeTiO3), geikielite, (MgTiO3) perovskite (CaTiO3) and titanite or sphene (CaTiSiO4(O,OH,F)). It also is found in many iron ores. Abundance of titanium in the earth’s crust is 0.565%. Titanium has been detected in moon rocks and meteorites. Titanium oxide has been detected in the spectra of M-type stars and interstellar space.
Titanium is found in plants, animals, eggs, and milk.
Many titanium alloys have wide industrial applications. Titanium forms alloys with a number of metals including iron, aluminum, manganese, and molybdenum. Its alloys are of high tensile strength, lightweight, and can withstand extreme temperatures. They are used in aircraft and missiles. The metal also has high resistance to sea water corrosion and is used to protect parts of the ships exposed to salt water. Also, titanium is used to combine with and remove traces of oxygen and nitrogen from incandescent lamps. Titanium compounds, notably the dioxide and the tetrachloride, have many uses (See Titanium Dioxide and Titanium Tetrachloride.)
Production
The production of titanium always encounters difficulties because of a tendency to react with oxygen, nitrogen and moisture at elevated temperatures. Most high purity elemental titanium can be produced by the Kroll process from titanium tetrachloride. The tetrachloride is reduced with magnesium in a mild steel vessel at about 800°C under an inert atmosphere of helium or argon. The net reaction is as follows:
TiCl4 + 2Mg → Ti + 2 MgCl2
The reaction is highly exothermic providing heat needed to maintain high temperature required for reaction. The Kroll process is applied commercially to produce elemental titanium.
Sodium metal can be used instead of magnesium in thermally reducing titanium tetrachloride.
Titanium metal also can be produced by electrolytic methods. In electrolysis, fused mixtures of titanium tetrachloride or lower chlorides with alkaline earth metal chlorides are electrolyzed to produce metal. Also, pure titanium can be prepared from electrolysis of titanium dioxide in a fused bath of calcium-, magnesiumor alkali metal fluorides. Other alkali or alkaline metal salts can be substituted for halides in these fused baths. Other titanium compouds that have been employed successfully in electrolytic titanium production include sodium fluotitanate and potassium fluotitanate.
Very highly pure titanium metal can be prepared in small amounts by decomposition of pure titanium tetraiodide, (TiI4) vapor on a hot wire under low pressure (Van Arkel–de Boer method).
Reactions
Titanium metal is very highly resistant to corrosion. It is unaffected by atmospheric air, moisture and sea water, allowing many of its industrial applications. The metal burns in air at about 1,200°C incandescently forming titanium dioxide TiO2. The metal also burns on contact with liquid oxygen. Titanium forms four oxides, all of which have been well described. It forms a weakly basic monoxide, TiO; a basic dititanium trioxide, Ti2O3; the amphoteric dioxide, TiO2; and the acidic trioxide, TiO3.
Titanium combines with nitrogen at about 800°C forming the nitride and producing heat and light. It is one of the few elements that burns in nitrogen. Titanium reacts with all halogens at high temperatures. It reacts with fluorine at 150°C forming titanium tetrafluoride, TiF4. Reaction with chlorine occurs at 300°C giving tetrachloride TiCl4. Bromine and iodine combine with the metal at 360°C forming their tetrahalides.
Water does not react with Ti metal at ambient temperatures, but tianium reacts with steam at 700°C forming the oxide and hydrogen:
Ti + 2H2O → TiO2 + 2H2
Titanium is soluble in hot concentrated sulfuric acid, forming sulfate. It also reacts with hydrofluoric acid forming the fluoride.
Nitric acid at ordinary temperatures does not react with Ti metal, but hot concentrated nitric acid oxidizes titanium to titanium dioxide.
The metal is stable with alkalies.
Titanium combines with several metals, such as, iron, copper, aluminum, chromium, cobalt, nickel, lead and tin at elevated temperatures forming alloys.
Isotopes
There are 23 known isotopes of titanium. All but five are radioactive, rangingfrom Ti-38 to Ti-61, and have half-lives varying from a few nanoseconds to a few hours.The percentages of the five stable isotopes found in nature are as follows: 46Ti = 8.25%,47Ti = 7.44%, 48Ti = 73.72%, 49Ti = 5.41%, and 50Ti = 5.18%.
Origin of Name
It was named after “Titans,” meaning the first sons of the Earth as
stated in Greek mythology.
Characteristics
As the first element in group 4, titanium has characteristics similar to those of the othermembers of this group: Zr, Hf, and Rf. Titanium is a shiny, gray, malleable, and ductile metalcapable of being worked into various forms and drawn into wires.
History
In 1791 Reverend William Gregor (1761–1817), an amateur mineralogist, discoveredan odd black sandy substance in his neighborhood. Because it was somewhat magnetic, hecalculated that it was almost 50% magnetite (a form of iron ore). Most of the remainder ofthe sample was a reddish-brown powder he dissolved in acid to produce a yellow substance.Thinking he had discovered a new mineral, he named it “menachanite,” after the Menachanregion in Cornwall where he lived. During this period, Franz Joseph Muller (1740–1825) alsoproduced a similar substance that he could not identify. In 1793 Martin Heinrich Klaproth(1743–1817), who discovered several new elements and is considered the father of modernanalytical chemistry, identified the substance that Gregor called a mineral as a new element.Klaproth named it “titanium,” which means “Earth” in Latin.
Production Methods
Titanium is the ninth most abundant element and accounts for about 0.63% of the Earth’s crust. Analyses of rock samples from the moon indicate that titanium is far more abundant there; some lunar rocks consist of 12% titanium by weight. World production of titanium sponge metal was estimated at 69,000 metric tons in 1991. The most important titaniumbearing minerals are ilmenite, rutile, and leucoxene. Ilmenite (FeTiO3) is found in beach sands (Australia, India, and Florida) and in rock deposits associated with iron (Norway and Finland). Ilmenite accounts for about 91%of the world’s consumption of titanium minerals and world resources of anatase, ilmenite, and rutile total more than 2 billion tons. Rutile (a form ofTiO2) is less abundant; its chief source is certain Australian beach sands. Two other less prominent forms of TiO2 exist, anatase and brookite. The ores vary around the world in TiO2 content from 39% to 96%. Anatase is used as a food color.
Air & Water Reactions
Highly flammable. Pyrophoric in dust form [Bretherick 1979, p. 104]. Titanium is water-reactive at 700C, releasing hydrogen, which may cause an explosion [Subref: Mellor, 1941, vol. 7, 19].
Reactivity Profile
TITANIUM reacts violently with cupric oxide and lead oxide when heated. When titanium is heated with potassium chlorate, potassium nitrate, or potassium permanganate, an explosion occurs [Mellor 7:20. 1946-47]. The residue from the reaction of titanium with red fuming nitric acid exploded violently when the flask was touched [Allison 1969]. Liquid oxygen gives a detonable mixture when combined with powdered titanium, [Kirchenbaum 1956].
Hazard
Almost all of titanium’s compounds, as well as the pure metal when in powder form, areextremely flammable and explosive. Titanium metal will ignite in air at 1200°C and willburn in an atmosphere of nitrogen. Titanium fires cannot be extinguished by using water orcarbon dioxide extinguishers. Sand, dirt, or special foams must be used to extinguish burningtitanium.
Health Hazard
Inhalation of metal powder may cause coughing,irritation of the respiratory tract, anddyspnea. Intramuscular administration of titaniumin rats caused tumors in blood. Animalcarcinogenicity is not fully established.Human carcinogenicity is not known.
Health Hazard
Fire will produce irritating, corrosive and/or toxic gases. Inhalation of decomposition products may cause severe injury or death. Contact with substance may cause severe burns to skin and eyes. Runoff from fire control may cause pollution.
Fire Hazard
Flammable/combustible material. May ignite on contact with moist air or moisture. May burn rapidly with flare-burning effect. Some react vigorously or explosively on contact with water. Some may decompose explosively when heated or involved in a fire. May re-ignite after fire is extinguished. Runoff may create fire or explosion hazard. Containers may explode when heated.
Flammability and Explosibility
Nonflammable
Safety Profile
Questionable
carcinogen with experimental tumorigenic
data. Experimental reproductive effects.
The dust may ignite spontaneously in air.
Flammable when exposed to heat or flame
or by chemical reaction. Titanium can burn
in an atmosphere of carbon dioxide,
nitrogen, or air. Also reacts violently with
BrF3, CuO, PbOx (Ni + KClO3), metaloxy
salts, halocarbons, halogens, CO2, metal
carbonates, Al, water, AgF, O2 , nitryl
fluoride, HNO3,O2, KClO3, KNO3 ,
KMnO4, steam @ 704°, trichloroethylene,
trichlorotrifluoroethane. Ordinary
extinguishers are often ineffective against
titanium fires. Such fires require special
extinguishers designed for metal fires. In
airtight enclosures, titanium fires can be
controlled by the use of argon or helium.
Titanium, in the absence of moisture, burns
slowly, but evolves much heat. The
application of water to burning titanium can
cause an explosion. Finely dwided titanium
dust and powders, like most metal powders,
are potential explosion hazards when
exposed to sparks, open flame, or high-heat
sources. See also TITANIUM
COMPOUNDS, POWDERED METALS,
and MAGNESIUM.
Potential Exposure
Titanium metal, because of its low weight, high strength, and heat resistance, is used in the aerospace and aircraft industry as tubing, fittings, fire walls; cowlings, skin sections; jet compressors; and it is also used in surgical appliances. It is used, too, as controlwire casings in nuclear reactors, as a protective coating for mixers in the pulp-paper industry and in other situations in which protection against chlorides or acids is required; in vacuum lamp bulbs and X-ray tubes; as an addition to carbon and tungsten in electrodes and lamp filaments; and to the powder in the pyrotechnics industry. It forms alloys with iron, aluminum, tin, and vanadium, of which ferrotitanium is especially important in the steel industry. Other titanium compounds are utilized in smoke screens, as mordants in dyeing; in the manufacture of cemented metal carbides; as thermal insulators; and in heat resistant surface coatings in paints and plastics.
Environmental Fate
Titanium is poorly absorbed by plants and animals and is
retained to only a certain extent. High levels of titanium in food
products can be detects, however, when soil is contaminated by
fly-ash fallout or titanium-containing sewage residues and
when titanium dioxide is used as a food whitener. Food, which
is considered to be the most important source of exposure to
titanium, contributes >99% of the daily intake of the element.
There are no relevant tolerable intakes for titanium against
which to compare estimated dietary intake. Typical diets may
contain approximately 0.3–0.5 mg titanium.
Titanium content of soil generally ranges from 0.3 to 6%,
high levels of which are found in the vicinity of power plants
because of combustion of coal.
Titanium concentrations in the atmosphere are comparatively
low. Annual average concentrations in urban air are
mostly <0.1 mgm-3 and they are lower still in rural air. Air
concentrations up to 0.5 mgm-3 have been reported in urban
and industrialized areas.
Shipping
UN2546 Titanium powder, dry, Hazard Class: 4.2; Labels: 4.2-Spontaneously combustible material.
Toxicity evaluation
Many data indicate that titanium is absorbed poorly from the
gastrointestinal tract in human beings. It is likely that transferrin
may act as a specific carrier of titanium ions and may play
a central role during the transport and biodistribution of
soluble titanium species throughout the organism. Titanium
concentrations found generally in urine suggest an absorption
of <5%, assuming a daily intake of at least 300 mg.
Incompatibilities
Powder and dust may ignite spontaneously in air. Violent reactions occur on contact with water, steam, halocarbons, halogens, and aluminum. The dry powder is a strong reducing agent; Incompatible with oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause firesor explosions. Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides.
Check Digit Verification of cas no
The CAS Registry Mumber 7440-32-6 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,4,4 and 0 respectively; the second part has 2 digits, 3 and 2 respectively.
Calculate Digit Verification of CAS Registry Number 7440-32:
(6*7)+(5*4)+(4*4)+(3*0)+(2*3)+(1*2)=86
86 % 10 = 6
So 7440-32-6 is a valid CAS Registry Number.
InChI:InChI=1S/Ti
7440-32-6Relevant articles and documents
Titanium powder production by preform reduction process (PRP)
Okabe, Toru H.,Oda, Takashi,Mitsuda, Yoshitaka
, p. 156 - 163 (2004)
To develop an effective process for titanium powder production, a new preform reduction process (PRP), based on the calciothermic reduction of preform containing titanium oxide (TiO2), was investigated. The feed preform was fabricated from slurry, which was made by mixing TiO2 powder, flux (e.g. CaCl2) and binder. Various types of preforms in the form of plates, spheres, or tubes were prepared using a conventional technique, and the fabricated preform was sintered at 1073 K before reduction in order to remove the binder and water. The sintered solid preform containing TiO2 was then placed in a stainless steel container, and reacted with calcium vapor at a constant temperature ranging between 1073 and 1273 K for 6 h. Titanium powder was recovered from the reduced preform by leaching it with acid. As a result, pure titanium powder with 99 mass% purity was obtained. This process was found to be suitable for producing a homogeneous fine powder when the composition of flux and the size of the preform are controlled.
Thermal decomposition of Ti5(Se,Te)8 in argon and nitrogen atmospheres
Pankratova,Zvinchuk,Suvorov,Hatanpaa,Kozlov,Leskela
, p. 1005 - 1009 (2005)
Chalcogenides TiSe1.60-x Tex (0 ≤.x ≤ 1.60), forming a continuous series of hexagonal solid solutions, were prepared by the direct ampule procedure. The thermal decomposition of TiSe1.60-x Tex was studied for the samples with x = 0, 0.16, 0.80, 1.44, and 1.60 in Ar and N2 atmospheres in the course of heating from 25 to 1000°C. The selenide undergoes no weight loss under Ar, in contrast to the telluride which disproportionates and loses weight owing to the formation of volatile TiTe2. At high temperatures, tellurides are more sensitive than selenides to the presence of nitrogen: The disproportionation is accompanied by the reaction of TiTe2 with N2, yielding low-volatile titanium nitride and free tellurium. Titanium selenide and telluride as components of the solid solutions behave similarly to the corresponding individual chalcogenides. 2005 Pleiades Publishing, Inc.
Revealing dehydrogenation effect and resultant densification mechanism during pressureless sintering of TiH2 powder
Chen,Yang,Liu,Ma,Kang,Wang,Zhang,Li,Li,Li
, (2021)
The use of TiH2 powder as a sintering precursor can produce nearly full-density titanium and titanium alloys with good mechanical properties. Unfortunately, there is a lack of research on the effect of lattice defects generated during the dehydrogenation of TiH2 powder, and the underlying sintering diffusion mechanism and activation energy have yet to be determined. In this work, we report a two-step sintering strategy to reveal the dehydrogenation effect and resultant densification mechanism during the pressureless sintering of a TiH2 powder precursor. The results show that, compared with hydrogenated-dehydrogenated (HDH) Ti powder, TiH2 powder, an intermediate of HDH-Ti powder, exhibited a higher instantaneous densification rate, greater onset relative density, rapid grain growth, and thus a smaller grain size. It also showed a grain boundary diffusion mechanism below 91% relative density and half the sintering activation energy in the intermediate sintering stage. Fundamentally, this was attributed to lattice defects generated during the dehydrogenation of TiH2 powder, which was confirmed by the greater relative density of a sintered TiH2 compact due to the two-step sintering strategy designed herein. Interestingly, the sintered sample obtained from the TiH2 powder precursor has a satisfying combination of strength and ductility that is far superior to other bulk Ti materials, especially sintered bulk Ti obtained from HDH-Ti powder. The results obtained in this paper provide theoretical guidance for using pressureless sintering to produce nearly full-density Ti and Ti alloys with good mechanical properties for structural applications.
Magnesium reduction of titanium tetrachloride
Evdokimov,Krenev
, p. 490 - 493 (2002)
The reasons for the slow rate of reaction between TiCl4 vapor and a clean Mg surface are clarified, and the role of the magnesium reduction of titanium chlorides in the gas phase and liquid magnesium chloride film is discussed. The mechanisms for the formation of spongy titanium and its deposition on the walls of commercial reactors are elucidated. A continuous procedure is proposed for the preparation of titanium powder.
Preparation of strong and ductile pure titanium via two-step rapid sintering of TiH2 powder
Sharma, Bhupendra,Vajpai, Sanjay Kumar,Ameyama, Kei
, p. 51 - 55 (2016)
The present work demonstrates the feasibility of preparing bulk-Ti, with high strength and good ductility, via spark plasma sintering of TiH2 powders. The microstructure and mechanical properties of bulk titanium prepared under two different pr
Kinetics of the iodide titanium process by the thermal decomposition of titanium tetraiodide
Cuevas,Fernandez,Sanchez
, p. 2589 - 2596 (2000)
An extensive study of the kinetics of the iodide titanium process, performed in a flow system by the thermal decomposition of titanium tetraiodide over a tungsten filament substrate, is presented in this paper. The influence of the substrate temperature, TF, and reactant pressure, PTiI(4)o, on the process rate has been analyzed. It has been found that the overall process is rate limited by the transfer of gases in the neighborhood of the substrate. In addition, it has been determined that the rate of titanium transfer is modulated at the filament surface by a certain deposition efficiency that depends on reactant pressure and reaction temperature. The available thermodynamic data for the gaseous titanium iodides at high temperatures fail to explain such an efficiency factor, although the calculations described herein indicate that such data are probably incorrect. Eventually, the titanium growth rate results from the noninterfering contributions of titanium deposition and evaporation rates. The overall reaction rate for the process can be expressed as a function of the operational parameters by the following equation: rG(TF, PTiI(4)o) = 0.9εD(TF, PTiI(4)o)PTiI(4)oTF-rE(TF) mg cm-2 min-1. εD represents the determined deposition efficiency and rE the titanium evaporation rate in vacuum. Owing to the similarities between the iodide process for titanium and zirconium, the general characteristics for the titanium growth kinetics here described are expected to be also fulfilled for the zirconium case.
Electrochemical reduction of TiO2 in molten LiCl-Li2O
Hur, Jin-Mok,Lee, Su-Chul,Jeong, Sang-Mun,Seo, Chung-K
, p. 1028 - 1029 (2007)
An investigation into the electrochemical reduction of TiO2 to Ti in molten LiCI-Li2O has been performed. Analysis of the time-dependent changes of a phase composition shows that the reduction proceeds through lithium-containing intermediates consisting of LiTi2O 4 and LiTiO2. The reduction of TiO2 in molten LiCl-Li2O allows a much lower reaction temperature compared to the conventional reduction process in molten CaCl2. Copyright
A new, energy-efficient chemical pathway for extracting ti metal from ti minerals
Fang, Zhigang Zak,Middlemas, Scott,Guo, Jun,Fan, Peng
, p. 18248 - 18251 (2013)
Titanium is the ninth most abundant element, fourth among common metals, in the Earth's crust. Apart from some high-value applications in, e.g., the aerospace, biomedicine, and defense industries, the use of titanium in industrial or civilian applications has been extremely limited because of its high embodied energy and high cost. However, employing titanium would significantly reduce energy consumption of mechanical systems such as civilian transportation vehicles, which would have a profound impact on the sustainability of a global economy and the society of the future. The root cause of the high cost of titanium is its very strong affinity for oxygen. Conventional methods for Ti extraction involve several energy-intensive processes, including upgrading ilmenite ore to Ti-slag and then to synthetic rutile, high-temperature carbo-chlorination to produce TiCl4, and batch reduction of TiCl4 using Mg or Na (Kroll or Hunter process). This Communication describes a novel chemical pathway for extracting titanium metal from the upgraded titanium minerals (Ti-slag) with 60% less energy consumption than conventional methods. The new method involves direct reduction of Ti-slag using magnesium hydride, forming titanium hydride, which is subsequently purified by a series of chemical leaching steps. By directly reducing Ti-slag in the first step, Ti is chemically separated from impurities without using high-temperature processes.
Fabrication of a micro-porous Ti-Zr alloy by electroless reduction with a calcium reductant for electrolytic capacitor applications
Kikuchi, Tatsuya,Yoshida, Masumi,Taguchi, Yoshiaki,Habazaki, Hiroki,Suzuki, Ryosuke O.
, p. 148 - 154 (2014)
A metallic titanium and zirconium micro-porous alloy for electrolytic capacitor applications was produced by electroless reduction with a calcium reductant in calcium chloride molten salt at 1173 K. Mixed TiO2-70 at%ZrO2 oxides, metallic calcium, and calcium chloride were placed in a titanium crucible and heated under argon atmosphere to reduce the oxides with the calcium reductant. A metallic Ti-Zr alloy was obtained by electroless reduction in the presence of excess calcium reductant and showed a micro-porous morphology due to the sintering of each of the reduced particles during the reduction. The residual oxygen content and surface area of the reduced Ti-Zr alloy decreased over time during the electroless reduction. The element distributions were slightly different at the positions of the alloy and were in the composition range of Ti-69.3 at% to 74.3 at%Zr. A micro-porous Ti-Zr alloy with low oxygen content (0.20 wt%) and large surface area (0.55 m2 g-1) was successfully fabricated by electroless reduction under optimal conditions. The reduction mechanisms of the mixed and pure oxides by the calcium reductant are also discussed.
Reactions of ground state Ti atoms with NO: Insertion versus complexation. An IR matrix isolation study
Krim, Lahouari,Prot, Christophe,Alikhani, Esm? M.,Manceron, Laurent
, p. 267 - 274 (2000)
The reaction of ground state Ti atoms with NO during condensation in solid argon has been reinvestigated. The NTiO molecule, already characterized in reactions of laser-ablated Ti, is the only product observed for the reaction between one Ti atom and one nitric oxide molecule. Isotopic data on ν1, ν2, ν3, 2ν1 and 2ν2 have been measured in the mid- and far-infrared regions. This enables a complete harmonic force-field calculation based on a bent geometry, in agreement with the conclusions of the previous study. No evidence is found, however, of a metastable nitrosyl complex intermediate, as previously proposed. This study confirms that the insertion reaction proceeds directly from the ground electronic state reagents, with no or very little activation energy. (C) 2000 Published by Elsevier Science B.V.
