| Titanium - Ti
CAS: 7440-32-6 Description: Lightweight, silver-gray metal Classification: Transition Metal Date of Discovery: 1791 Discoverer: William Gregor Name Origin: Greek titanos, Latin titans, the first sons of the Earth |
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Atomic Number: 22
Number of Neutrons: 26 Atomic Mass: 47.867(1) amu Melting Point: 1668 ± 10& deg;C Boiling Point: 3287 °C Density (293 K): 4.54 g/cm3 Atomic volume: 10.64 cm3/mol Electrical resistivity: 0.0234 10-6/cm 
Thermal conductivity: 0.219 W/cmK Enthalpy of atomization: 468.61 kJ/mol Enthalpy of vaporization: 421.00 kJ/mol Enthalpy of fusion: 15.481 kJ/mol Specific heat capacity: 0.52 J/gK |
Energy levels: 2-8-10-2
Electron configuration: [Ar]3d24s2 Crystal Structure: Hexagonal Atomic radius: 2.00 Å Covalent radius: 1.32 Å Oxidation States: +2, +3, +4 Electronegativity, Pauling: 1.54 Electron affinity: 0.079 eV First ionization energy: 6.82 eV 2nd ionization energy: 13.58 eV 3rd ionization energy: 27.491 eV Polarizability: 14.6 10-24cm3 |
| Isotope | Natural Abundance | Atomic Mass | Half-life | Decay Mode | Spin |
| 39Ti | 39.0013 | 28 ms |  + |
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| 40Ti | 39.9905 | 0.06 s | + |
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| 41Ti | 40.98313 | 80 ms | +, p |
3/2+ | |
| 42Ti | 41.97303 | 0.20 s | + |
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| 43Ti | 42.96852 | 0.50 s | + |
7/2- | |
| 44Ti | 43.959690 | 67 y | EC | 0+ | |
| 45Ti | 44.958124 | 3.078 h | +; EC |
7/2- | |
| 46Ti | 8.25(3) | 45.952630 | Stable | 0+ | |
| 47Ti | 7.44(2) | 46.951764 | Stable | - | 5/2- |
| 48Ti | 73.72(3) | 47.947947 | Stable | 0+ | |
| 49Ti | 5.41(2) | 48.947871 | Stable | 7/2- | |
| 50Ti | 5.18(2) | 49.944792 | Stable | 0+ | |
| 51Ti | 50.946616 | 5.76 m | - |
3/2- | |
| 52Ti | 51.94690 | 1.7 m | - |
0+ | |
| 53Ti | 52.9497 | 33 s | - |
3/2- | |
| 54Ti | 53.9510 | - |
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| 55Ti | 54.9552 | - |
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| 56Ti | 55.9580 | - |
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| 57Ti | 56.964 | - |
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| 58Ti | |||||
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Discovered by Gregor in 1791; named by Klaproth in 1795. Impure titanium was prepared by Nilson and Pettersson in 1887; however, the pure metal (99.9%) was not made until 1910 by Hunter by heating TiCl4 with sodium in a steel bomb. Titanium is present in meteorites and in the sun. Rocks obtained during the Apollo 17 lunar mission showed presence of 12.1% TiO2. Analyses of rocks obtained during earlier Apollo missions show lower percentages. Titanium oxide bands are priminent in the spectra of M-type stars. The element is the ninth most abundant in the crust of the earth. Titanium is almost always present in igneous rocks and in the sediments derived from them. It occurs in the minerals rutile (TiO2), ilmenite (Fe2+TiO3), and sphene (CaTiOSiO4), and is present in titanates and in many iron ores. Titanium is present in the ash of coal, in plants, and in the human body. The metal was a laboratory curiosity until Kroll, in 1946, showed that titanium could be produced commercially by reducing titanium tetrachloride with magnesium. This method is largely used for producing the metal today. The metal can be purified by decomposing the iodide. Titanium, when pure, is a lustrous, white metal. It has a low density, good strength, is easily fabricated, and has excellent corrosion resistance. It is ductile only when it is free of oxygen. The metal burns in air and is the only element that burns in nitrogen. Titanium is resistant to dilute sulfuric and
hydrohloric acid, most organic acids, most chlorine gas, and chloride solutions.
Natural titanium consists of five isotopes with atomic masses from 46 to 50. All are
stable. Eight other unstable isotopes are known. Natural titanium is reported to
become very radioactive after bombardment with deuterons. The emitted radiations
are mostly positrons and hard gamma rays. The metal is dimorphic. The hexagonal
alpha form changes to the cubic beta form very slowly at about 880 °C. The metal
combines with oxygen at red heat, and with chlorine at 550 °C. Titanium is important
as an alloying agent with aluminum, molybdenum, manganese, iron, and other
metals. Alloys of titanium are principally used for aircraft and missiles where
lightweight strength and ability to withstand extremes of temperature are important.
Titanium is as strong as steel, but 45% lighter. It is 60% heavier than aluminum,
but twice as strong. Titanium has potential use in desalination plants for converting
sea water into fresh water. The metal has excellent resistance to sea water and is
used for propeller shafts, rigging, and other parts of ships exposed to salt water. A
titanium anode coated with platinum has been used to provide cathodic protection
from corrosion by salt water. Titanium metal is considered to be physiologically
inert. When pure, titanium dioxide is relatively clear and has an extremely high
index of refraction with an optical dispersion higher than diamond. It is produced
artificially for use as a gemstone, but it is relatively soft. Star sapphires and rubies
exhibit their asterism as a result of the presence of TiO2. Titanium dioxide is extensively used for both house paint and artist's paint, as it is permanent and has good covering power. Titanium oxide pigment accounts for the largest use of the element. Titanium paint is an excellent reflector of infrared, and is extensively used in solar observatories where heat causes poor seeing conditions. Titanium tetrachloride is used to iridize glass. This compound fumes strongly in air and has been used to produce smoke screens.
LINKS: International Titanium Association Titanium Data and Reference Manual Titanium Deposition Processes Titanium . . .the future in eyewear Titanium prosthesis gives crowded lungs room to grow Return
Sources for the information on this website include: Lide, David R., ed. CRC Handbook of Chemistry and Physics, 78th Ed., 1997-1998. |
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