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Title: Chemistry/Elements/Titanium - Lenntech: Titanium Physical data, chemical properties, and health effects.
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Titanium Data tables and historic information.
| USGS_Minerals_Information__Titanium Statistics and information on the worldwide supply, demand, and flow of the element (PDF format).
| Visual_Elements__Titanium Image, general and physical information, source, uses, key isotopes, and ionisation energies.
| WebElements__Titanium Extensive information on history, uses, occurrence, compounds, and properties of the element.
| Wikipedia__Titanium Properties of the element, including its history, applications, and characteristics.
| Radiochemistry_of_Titanium Full text of the monograph by Vincent J. Landis (San Diego State University, San Diego, California). [PDF] (January, 1971)
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Titanium (Ti) - Chemical properties, Health and Environmental effects
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Chemical properties of titanium - Health
effects of titanium -
Environmental effects of titanium
Atomic number
22
Atomic mass
47.90 g.mol -1
Electronegativity
according to Pauling
1.5
Density
4.51 g.cm-3 at 20°C
Melting point
1660 °C
Boiling point
3287 °C
Vanderwaals
radius
0.147 nm
Ionic radius
0.09 nm (+2) ; 0.068 nm (+4)
Isotopes
8
Electronic
shell
[ Ar ] 3d1 4s2
Energy of
first ionisation
658 kJ.mol -1
Energy of
second ionisation
1310 kJ.mol -1
Energy of
third ionisation
2652 kJ.mol -1
Energy of
fourth ionisation
4175 kJ.mol -1
Discovered by
William
Gregor in 1791
Titanium
Chemical element, Ti, atomic number 22 and atomic weight 47.90. Its
chemical behavior shows many similarities with that or silica and
zirconium, as an element belonging to the first transition group. Its
chemistry in aqueous solution, especially in the lower oxidation states,
has some similarities with that of chrome and vanadium. Titanium is a
transition metal
light
with a white-silvery-metallic colour. It is
stong,
lustrous, corrosion-resistant. Pure titanium is not soluble
in water but is soluble in concentrated acids.
This metal forms a passive but protective oxide coating (leading
to corrosion-resistance) when exposed to elevated temperatures in air
but at room temperatures it resists tarnishing.
The
main oxidation state is 4+, although the states 3+ and 2+ are also known, but are less
stable. This element burns in the air when it’s heated up to obtain
the dioxide, TiO2, and when it is combined with halogens. It
reduces the water vapor to form the dioxide and hydrogen, and it reacts
in a similar way with hot concentrated acids, although it forms
trichloride with chlorhydric acid. The metal absorbs hydrogen to give
TiH2, and forms the nitride, TiN, and the carbide, TiC. Other
known compounds are the sulfur TiS2, as well as the lowest
oxides, Ti2O3 and TiO, and the sulfurs Ti2S3
and TiS. Salts are known in the three oxidation states.
Applications
The
titanium dioxide is extensively used as a white pigment in outside paintings for being
chemically inert, for its great coating power, its opacity to UV light
damage and its autocleaning capacity. The dioxide was also used once as
a bleaching and opicifying agent in porcelain enamels, giving them a
final touch of great brightness, hardness and acid resistance. A typical
lipstick contais 10% titanium.
Titaium alloys are characterized by very high tensile strength even at high
temperatures, light weight, high corrosion resistance, and ability to
withstand extreme temperatures. ue to these properties they are principally used in
aircraft, pipes for power plants, armour plating, naval ships,
spacecraft and missiles. Titanium is as strong as steel but 45% lighter.
In medicine titanium is used to make hip and knee replacements,
pace-makers, bone-plates and screws and cranial plates for skull
fractures. It has also been used to attach false theet.
The
alkaline earth titanates have some remarkable properties. The level of
dielectric constants varies from 13 for the MgTiO3, to various milliards for
solid solutions of SrTiO3 in BaTiO3. The barium titanate also
has a dielectric constant of 10.000 close to 120ºC, which is its Curie
point; it has low dielectric histeresis. The ceramic transductors that
contain barium titanate are favorably compared with Rochelle salt in
terms of thermal stability and with quartz in terms of the strength of
the effect and the capacity to form the ceramics in various forms. The
compound has bee used as ultrasonic vibrations generator and as a sound
detector.
Titanium in the environment
Althoug it is not found unbound to other elements in nature, titamuim is the ninth most abundant element in the Earth's crust
(0.63% by mass) and is present in most igneous rocks and in sediments
derived from them. Important titanium minerals are rutile, brookite,
anatase, illmenite, and titanite. The chief mined ore, ilmenite, occurs
as vast deposits of sand in Western Australia, Norway, Canada and
Ukraine. Large deposits of rutile in North America and South Africa also
contribute significantly to the world supply of titanium. World
production of the metal is about 90.000 tonnes per year, and that of
titanium dioxide is 4.3 million tonnes per year.
The
titanium dioxide, TiO2, is commonly found in a black or brownish form
known as rutile. The natural forms that are less frequently found in
nature are the anatasite and the brooquite. Both the pure rutile and the
pure anatasite are white. The black basic oxide, FeTiO3, is
found in the natural form as the natural mineral called ilmenite; this
is the main commercial source of titanium.
Health
effects of titanium
There is no known biological role for titanium. There is a detectable
amount of titanium in the human body and it has been hestimated that we
take in about 0.8 mg/day, but most passes through us without being
adsorbed. It is not a poisoun metal and the human body can tolerate
titanium in large dosis.
Elemental titanium
and titanium dioxide is of a low order of toxicity. Laboratory animals (rats) exposed to titanium
dioxide via inhalation have developed small-localized areas of
dark-colored dust deposits in the lungs. Excessive exposure in humans
may result in slight changes in the lungs.
Effects of
overexposure to titanium powder: Dust inhalation may cause tightness and pain in chest,
coughing, and difficulty in breathing. Contact with skin or eyes may
cause irritation. Routes of entry: Inhalation, skin contact, eye
contact.
Carcinogenicity: The International Agency for Research on
Cancer (IARC) has listed titanium dioxide within Group 3 (The
agent is not classifiable as to its carcinogenicity to humans.)
Environmental effects of titanium
Low toxicity.
When in a metallic powdered form, titanium metal poses a significant
fire hazard and, when heated in air, an explosion hazard.
No environmental effects have been reported.
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