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Titanium


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Atomic symbol: Ti
Atomic number: 22
Atomic weight: 47.90
Atomic volume: 10.64 cm3/mol
Density: 4.50 g/cm3
Period Number: 4
Group number: 4
Group name: Trans. Met.
Element classification: Metal


States


Phase at room temperature: Solid
Melting Point: 1933.2 K
Boiling point: 3558 K
Heat of fusion: 15.450 kJ/mol
Heat of vaporization: 421.00 kJ/mol


Energies


Ionization Energy: 6.828 eV
1st ionization energy: 658 kJ/mole
2nd ionization energy: 1310.3 kJ/mole
3rd ionization energy: 2652.5 kJ/mole
Electronegativity: 1.54
Electron affinity: 7.6 kJ/mole
Specific heat: 0.52 J/gK
Heat atomization: 470 kJ/mole atoms


Oxidation & Electrons


Shells: 2,8,10,2
Electron Shell Configuration: [Ar] 3d2 4s2
Minimum oxidation number: -1
Maximum oxidation number: 4
Minimum common oxidation number: 0
Maximum common oxidation no: 4


Appearance & Characteristics


Structure:: hcp: hexagonal close pkd
Color: gray
Hardness: mohs
Toxicity: ?
Characteristics: max strength/weight ratio
Uses: steel,white pigment(TiO2)


Reactions


Reaction with air: mild, w/ht =>TiO2, TiN
Reaction with 6M HCl: none
Reaction with 15M HNO3: passivated
Reaction with 6M NaOH: none


Other Forms


Number of isotopes: 5
Oxide(s): TiO Ti2O3 TiO2 + more
Hydride(s): TiH2
Chloride(s): TiCl2 TiCl3 TiCl4


Radius


Atomic Radius: 147 pm
Ionic radius (1- ion): pm
Ionic radius (1+ ion): pm
Ionic radius (2- ion): pm
Ionic radius (2+ ion): 100 pm
Ionic radius (3+ ion): 81 pm


Conductivity


Thermal conductivity: 21.9 J/m-sec-deg
Electrical conductivity: 23.81 1/mohm-cm
Polarizability: 14.6 A^3


Abundance


Source: Ilmenite, rutile(oxide)
Relative abundance solar system: 3.380 log
Abundance earth's crust: 3.8 log
Estimated crustal abundance: 5.65×103 milligrams per kilogram
Estimated oceanic abundance: 1×10-3 milligrams per liter
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 


History


(Latin. titans, the first sons of the Earth, mythology)

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 when Hunter heated TiCl4 with sodium in a steel bomb.


Sources


Titanium is present in meteorites and the sun. Rocks obtained during the Apollo 17 lunar mission showed presence of 12.1% TiO2; rocks obtained during earlier Apollo missions show lower percentages.

Titanium oxide bands are prominent 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, ilmenite, and sphene, and is present in titanates and in many iron ores. Titanium is present in ash of coal, in plants, and in 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 still largely used for producing the metal. The metal can be purified by decomposing the iodide.


Properties


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, which burns in air, is the only element that burns in nitrogen.

Titanium is resistant to dilute sulfuric and hydrochloric acid, most organic acids, most chlorine gas, and chloride solutions.

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 8800C. The metal combines with oxygen at red heat, and with chlorine at 5500C.

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.


Uses


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.

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, because 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 viewing conditions.

Titanium tetrachloride is used to iridize glass. This compound fumes strongly in air and has been used to produce smoke screens.


Isotopes


Natural titanium consists of five isotopes with atomic masses from 46 to 50. All are stable. Eight other unstable isotopes are known.

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