Cannabis Ruderalis

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Tellurium, 52Te
Tellurium
Pronunciation/tɛˈljʊəriəm/ ​(te-LURE-ee-əm)
Appearancesilvery lustrous gray (crystalline),
brown-black powder (amorphous)
Standard atomic weight Ar°(Te)
Tellurium in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
Se
↑
Te
↓
Po
antimony ← tellurium → iodine
Atomic number (Z)52
Groupgroup 16 (chalcogens)
Periodperiod 5
Block  p-block
Electron configuration[Kr] 4d10 5s2 5p4
Electrons per shell2, 8, 18, 18, 6
Physical properties
Phase at STPsolid
Melting point722.66 K ​(449.51 °C, ​841.12 °F)
Boiling point1261 K ​(988 °C, ​1810 °F)
Density (at 20° C)6.237 g/cm3[3]
when liquid (at m.p.)5.70 g/cm3
Heat of fusion17.49 kJ/mol
Heat of vaporization114.1 kJ/mol
Molar heat capacity25.73 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K)   (775) (888) 1042 1266
Atomic properties
Oxidation states−2, −1, 0, +1, +2, +3, +4, +5, +6 (a mildly acidic oxide)
ElectronegativityPauling scale: 2.1
Ionization energies
  • 1st: 869.3 kJ/mol
  • 2nd: 1790 kJ/mol
  • 3rd: 2698 kJ/mol
Atomic radiusempirical: 140 pm
Covalent radius138±4 pm
Van der Waals radius206 pm
Color lines in a spectral range
Spectral lines of tellurium
Other properties
Natural occurrenceprimordial
Crystal structure ​hexagonal[4] (hP3)
Lattice constants
Hexagonal crystal structure for tellurium
a = 445.59 pm
c = 592.75 pm (at 20 °C)[3]
Thermal expansion19.0×10−6/K (at 20 °C)[a]
Thermal conductivity1.97–3.38 W/(m⋅K)
Magnetic orderingdiamagnetic[5]
Molar magnetic susceptibility−39.5×10−6 cm3/mol (298 K)[6]
Young's modulus43 GPa
Shear modulus16 GPa
Bulk modulus65 GPa
Speed of sound thin rod2610 m/s (at 20 °C)
Mohs hardness2.25
Brinell hardness180–270 MPa
CAS Number13494-80-9
History
Namingafter Roman Tellus, deity of the Earth
DiscoveryFranz-Joseph Müller von Reichenstein (1782)
First isolationMartin Heinrich Klaproth
Isotopes of tellurium
Main isotopes[7] Decay
abun­dance half-life (t1/2) mode pro­duct
120Te 0.09% stable
121Te synth 16.78 d ε 121Sb
122Te 2.55% stable
123Te 0.89% stable[8]
124Te 4.74% stable
125Te 7.07% stable
126Te 18.8% stable
127Te synth 9.35 h β− 127I
128Te 31.7% 2.2×1024 y β−β− 128Xe
129Te synth 69.6 min β− 129I
130Te 34.1% 8.2×1020 y β−β− 130Xe
 Category: Tellurium
| references

Tellurium (Template:Pron-en te-LOOR-ee-əm) is a chemical element that has the symbol Te and atomic number 52. A brittle, mildly toxic, silver-white metalloid which looks similar to tin, tellurium is chemically related to selenium and sulfur. Tellurium was discovered in 1782 by Franz-Joseph Müller von Reichenstein in a mineral containing gold and tellurium. Martin Heinrich Klaproth named the new element in 1798 after the Latin word for "earth", tellus. Although several gold deposits contain tellurium minerals, the main commercial source for tellurium is as a by-product of copper and lead production. Tellurium is primarily used in alloys, foremost in steel and copper to improve machinability. Applications in solar panels and as a semiconductor material also consume a considerable fraction of tellurium production.

Tellurium has no biological function, although fungi can incorporate it in place of sulfur and selenium into amino acids such as telluro-cysteine and telluro-methionine. In humans, tellurium is partly metabolized into dimethyl telluride, (CH3)2Te, a gas with a garlic-like odor which is exhaled in the breath of victims of tellurium toxicity or exposure.

History

Oval black and white engraving of a man looking left with a scarf and a coat with large buttons.
Klaproth named the new element and credited von Reichenstein with its discovery

Tellurium (Latin tellus meaning "earth") was discovered in the 18th century in a gold ore from the mines in Zlatna, near what is now Sibiu, Transylvania. This ore was known as "Faczebajer weißes blättriges Golderz" (white leafy gold ore from Faczebaja) or antimonalischer Goldkies (antimonic gold pyrite), and, according to Anton von Rupprecht, was Spießglaskönig (argent molybdique), containing native antimony.[9] In 1782 Franz-Joseph Müller von Reichenstein, who was then serving as the Hungarian chief inspector of mines in Transylvania, concluded that the ore did not contain antimony, but that it was bismuth sulfide.[10] The following year, he reported that this was erroneous and that the ore contained mostly gold and an unknown metal very similar to antimony. After a thorough investigation which lasted for three years and consisted of more than fifty tests, Müller determined the specific gravity of the mineral and noted the radish-like odor of the white smoke which passed off when the new metal was heated, the red color which the metal imparts to sulfuric acid, and the black precipitate which this solution gives when diluted with water. Nevertheless, he was not able to identify this metal and gave it the names aurum paradoxium and metallum problematicum, as it did not show the properties predicted for the expected antimony.[11][12][13]

In 1789, another Hungarian scientist, Pál Kitaibel, also discovered the element independently in an ore from Deutsch-Pilsen which had been regarded as argentiferous molybdenite, but later he gave the credit to Müller. In 1798, it was named by Martin Heinrich Klaproth who earlier isolated it from the mineral calaverite.[12][13][14]

Tellurium was used as a chemical bonder in the making of the outer shell of the first atomic bomb. The 1960s brought growth in thermoelectric applications for tellurium, as well as its use in free-machining steel, which became the dominant use.

Characteristics

Physical

When crystalline, tellurium is silvery-white and when it is in pure state it has a metallic luster. It is a brittle and easily pulverized metalloid. Amorphous tellurium is found by precipitating it from a solution of tellurous or telluric acid (Te(OH)6).[15] Tellurium is a p-type semiconductor that shows a greater electrical conductivity in certain directions which depends on atomic alignment; the conductivity increases slightly when exposed to light (photoconductivity).[16] When in its molten state, tellurium is corrosive to copper, iron and stainless steel.

Isotopes

Main article: isotopes of tellurium

Naturally occurring tellurium has eight isotopes. Four of those isotopes, 122Te, 124Te, 125Te and 126Te, are stable. The other four, 120Te, 123Te, 128Te and 130Te, have been observed to be radioactive.[17][18] The stable isotopes make up only 33.2 % of the naturally occurring tellurium; this is possible due to the long half-lives of the unstable isotopes. They are in the range from 1013 to 2.2 1024 years. This makes 128Te the isotope with the longest half life among all radioisotopes.[19]

There are 38 known nuclear isomers of tellurium with atomic masses that range from 105 to 142. Tellurium is the lightest element known to undergo alpha decay, with isotopes 106Te to 110Te being able to undergo this mode of decay.[17] The atomic mass of tellurium (127.60 g·mol−1) exceeds that of the following element iodine (126.90 g·mol−1).[20]

Occurrence

See also: Category:Telluride minerals
A dark mass, approximately 2 millimetres in diameter, on a rose-coloured crystal substrate
Tellurium on quartz (Moctezuma, Sonora, Mexico)

With an abundance in the Earth's crust comparable to that of platinum, tellurium is one of the rarest stable solid element in the Earth's crust. Its abundance is about 1 µg/kg.[21] In comparison, even the rarest of the lanthanides have crustal abundances of 500 µg/kg (see Abundance of the chemical elements).[22]

The extreme rarity of tellurium in the Earth's crust is not a reflection of its cosmic abundance, which is in fact greater than that of rubidium, even though rubidium is ten thousand times more abundant in the Earth's crust. The extraordinarily low abundance of tellurium on Earth is rather thought to be due to conditions in the Earth's formation, when the stable form of certain elements, in the absence of oxygen and water, was controlled by the reductive power of free hydrogen. Under this scenario, certain elements such as tellurium which form volatile hydrides were severely depleted during the formation of the Earth's crust, through evaporation of these hydrides. Tellurium and selenium are the heavy elements most depleted in the Earth's crust by this process.[citation needed]

Tellurium is sometimes found in its native (elemental) form, but is more often found as the tellurides of gold (calaverite, krennerite, petzite, sylvanite and others). Tellurium compounds are the most common chemical compounds of gold found in nature (rare non-tellurides such as gold aurostibite and bismuthide are known). Tellurium is also found combined with elements other than gold, in salts of other metals. In contrast to selenium, tellurium is not able to replace sulfur in its minerals. This is due to the large difference in ion radius of sulfur and tellurium. In consequence, many sulfide minerals contain considerable amounts of selenium, but only traces of tellurium.[23]

In the gold rush of 1893, diggers in Kalgoorlie discarded a pyritic material which got in their way as they searched for pure gold. The Kalgoorlie waste was thus used to fill in potholes or as part of sidewalks. Three years passed before it was realized that this waste was calaverite, a telluride of gold that had not been recognized. This led to a second gold rush on 29 May 1896.[24]

Compounds and chemistry

See also: Category:Tellurium compounds

Tellurium belongs to the same chemical family as oxygen, sulfur, selenium and polonium: the chalcogen family. It forms similar compounds to sulfur and selenium. It exhibits the oxidation states −2, +2, +4 and +6, with the +4 state being most common.[15]

Tellurides

The −2 oxidation state is exhibited in binary compounds with many metals, such as zinc telluride, ZnTe, formed by heating tellurium with zinc.[25] Decomposition of ZnTe with hydrochloric acid yields hydrogen telluride, H
2Te, the tellurium analogue of the other chalcogen hydrides, H
2O, H
2S and H
2Se:

ZnTe + 2 HCl → ZnCl
2 + H
2Te

H
2Te reacts with many metals to form tellurides, containing the Te2−
 anion.[25] Gold and silver tellurides are considered good ores.

Halides

The +2 oxidation state is exhibited by the monoxide, TeO, and the dihalides, TeCl
2, TeBr
2 and TeI
2. The dihalides have not been obtained in pure form,[26]: 274  although they are known decomposition products of the tetrahalides in organic solvents, and their derived tetrahalotellurates are well-characterized:

Te + X
2 + 2 X−
 → TeX2−
4

where X is Cl, Br, or I. These anions are square planar in geometry.[26]: 281  Polynuclear anionic species also exist, such as the dark brown Te
2I2−
6,[26]: 283  and the black Te
4I2−
14.[26]: 285 

Fluorine forms two halides with tellurium: the mixed-valence Te
2F
4 and TeF
6. In the +6 oxidation state, the –OTeF
5 structural group occurs in a number of compounds such as HOTeF
5, B(OTeF
5)
3, Xe(OTeF
5)
2, Te(OTeF
5)
4 and Te(OTeF
5)
6.[27] The square antiprismatic anion TeF2−
8 is also attested.[28] The other halogens do not form halides with tellurium in the +6 oxidation state, but only tetrahalides (TeCl
4, TeBr
4 and TeI
4) in the +4 state, and other lower halides (Te
3Cl
2, Te
2Cl
2, Te
2Br
2, Te
2I and two forms of TeI). In the +4 oxidation state, halotellurate anions are known, such as TeCl2−
6 and Te
2Cl2−
10. Halotellurium cations are also attested, including TeI+
3, found in TeI
3AsF
6.[29]

Oxocompounds
A sample of pale yellow powder
A sample of tellurium dioxide powder

Tellurium monoxide was first reported in 1883 as a black amorphous solid formed by the heat decomposition of TeSO
3 in vacuum, disproportionating into tellurium dioxide, TeO
2 and elemental tellurium upon heating.[30][31] Since then, however, some doubt has been cast on its existence in the solid phase, although it is known as a vapor phase fragment; the black solid may be merely an equimolar mixture of elemental tellurium and tellurium dioxide.[32]

Tellurium dioxide is formed by heating tellurium in air, causing it to burn with a blue flame.[25] Tellurium trioxide, β-TeO
3, is obtained by thermal decomposition of Te(OH)
6. The other two forms of trioxide reported in the literature, the α- and γ- forms, were found not to be true oxides of tellurium in the +6 oxidation state, but a mixture of Te4+
, OH−
 and O−
2.[33] Tellurium also exhibits mixed-valence oxides, Te
2O
5 and Te
4O
9.[33]

The tellurium oxides and hydrated oxides form a series of acids, including tellurous acid (H
2TeO
3), orthotelluric acid (Te(OH)
6) and metatelluric acid ((H
2TeO
4)
n).[32] The two forms of telluric acid form tellurate salts containing the TeO2–
4 and TeO6−
6 anions, respectively. Tellurous acid forms tellurite salts containing the anion TeO2−
3. Other tellurium cations include TeF2+
8, which consists of two fused tellurium rings and the polymeric TeF2+
7.

Zintl cations

When tellurium is treated with concentrated sulfuric acid, it forms red solutions containing the Zintl ion, Te2+
4. The oxidation of tellurium by AsF
5 in liquid SO
2 also produces this square planar cation, as well as with the trigonal prismatic, yellow-orange Te4+
6:[28]

4 Te + 3 AsF
5 → Te2+
4(AsF−
6)
2 + AsF
3
6 Te + 6 AsF
5 → Te4+
6(AsF−
6)
4 + 2 AsF
3

Other tellurium Zintl cations include the polymeric Te2+
7 and the blue-black Te2+
8, which consists of two fused 5-membered tellurium rings. The latter cation is formed by the reaction of tellurium with tungsten hexachloride:[28]

8 Te + 2 WCl
6 → Te2+
8(WCl−
6)
2

Interchalcogen cations also exist, such as Te
2Se2+
6 (distorted cubic geometry) and Te
2Se2+
8. These are formed by oxidizing mixtures of tellurium and selenium with AsF
5 or SbF
5.[28]

Organotellurium compounds
Main article: Organotellurium chemistry

In organic chemistry, tellurium forms analogues of alcohols and thiols, which have the functional group –TeH and are called tellurols. The –TeH functional group is also attributed to using the prefix tellanyl-.[34]

Production

The principal source of tellurium is from anode sludges produced during the electrolytic refining of blister copper. It is a component of dusts from blast furnace refining of lead. Treatment of 500 tons of copper ore typically yields one pound (0.45 kg) of tellurium. Tellurium is produced mainly in the United States, Canada, Peru and Japan.[35] For the year 2006 the British Geological Survey gives the following numbers: Canada 11 t, United States 50 t, Peru 37 t and Japan 24 t.[36]

Grey and white world map with four countries colored to show the percentage of world wide tellurium production. US to produce 40%; Peru to produce 30%; Japan to produce 20%;and Canada to produce 10%
Tellurium production 2006

The anode sludges contain the selenides and tellurides of the noble metals in compounds with the formula M2Se or M2Te (M = Cu, Ag, Au). At temperatures of 500 °C the anode sludges are roasted with sodium carbonate under air. The metals are reduced to the metals, while the tellurium is converted to sodium tellurite.[28]

M2Te + O2 + Na2CO3 → Na2TeO3 + 2 M + CO2

Tellurites can be leached from the mixture with water and are normally present as hydrotellurites HTeO3- in solution. Selenates are also formed during this process, but they can be separated by adding sulfuric acid. The hydrotellurites are converted into the insoluble tellurium dioxide while the selenites stay in solution.[28]

HTeO3- + OH- + H2SO4 → TeO2 + 2 SO42− + 2 H2O

The reduction to the metal is done either by electrolysis or by reacting the tellurium dioxide with sulfur dioxide in sulfuric acid.[28]

TeO2 + 2 SO2 + 2H2O → Te + SO42− + 4 H+

Commercial-grade tellurium is usually marketed as minus 200-mesh powder but is also available as slabs, ingots, sticks, or lumps. The year-end price for tellurium in 2000 was US$14 per pound. In recent years, the tellurium price was driven up by increased demand and limited supply, reaching as high as US$100 per pound in 2006.[37][38]

Applications

Metallurgy

The largest consumer of tellurium is metallurgy, where it is used in iron, copper and lead alloys. When added to stainless steel and copper it makes these metals more machinable. It is alloyed into cast iron for promoting chill for spectroscopic purposes, as the presence of electrically conductive free graphite tends to deleteriously effect spark emission testing results. In lead it improves strength and durability and decreases the corrosive action of sulfuric acid.[39]

Semiconductor and electronic industry uses

Solar panels, angled at about 30 degrees, reflect the blue sky from above a grassy field.
A CdTe photovoltaic array

Tellurium is used in cadmium telluride (CdTe) solar panels. National Renewable Energy Laboratory lab tests using this material achieved some of the highest efficiencies for solar cell electric power generation. Massive commercial production of CdTe solar panels by First Solar in recent years has significantly increased tellurium demand.[40][41] If some of the cadmium in CdTe is replaced by zinc then CdZnTe is formed which is used in solid-state x-ray detectors.[42]

Alloyed with both cadmium and mercury, to form mercury cadmium telluride, an infrared sensitive semiconductor material is formed.[43] Organotellurium compounds such as dimethyl telluride, diethyl telluride, diisopropyl telluride, diallyl telluride and methyl allyl telluride are used as precursors for Metalorganic vapor phase epitaxy growth of II-VI compound semiconductors. Diisopropyl telluride (DIPTe) is employed as the preferred precursor for achieving the low-temperature growth of CdHgTe by MOVPE.[44] For these process high purity metalorganics of both selenium and tellurium are used. The compounds for semiconductor industry and are prepared by adduct purification.[45][46]

Tellurium as a tellurium suboxide is used in the media layer of several types of rewritable optical discs, including ReWritable Compact Discs (CD-RW), ReWritable Digital Video Discs (DVD-RW) and ReWritable Blu-ray Discs.[47][48]

Tellurium is used in the new phase change memory chips[49] developed by Intel.[50] Bismuth telluride (Bi2Te3) is used in thermoelectric devices.

Other uses

Biological role

Tellurium has no biological function, although fungi can incorporate it in place of sulfur and selenium into amino acids such as telluro-cysteine and telluro-methionine. Organisms have show a highly variable tollernace on tellurium compounds. Most organisms metabolize tellurium partly to form dimethyl telluride although also dimethyle ditelluride is formed by some species. Dimethyl telluride has been observed in hot springs at very low concentrations.[57][58][59]

Precautions

Tellurium and tellurium compounds are considered to be mildly toxic and need to be handled with care, although acute poisoning is rare.[60] Tellurium is not reported to be carcinogenic.[60]

Humans exposed to as little as 0.01 mg/m3 or less in air develop "tellurium breath", which has a garlic-like odor.[51] The garlic odor that is associated with human intake of tellurium compounds is caused from the tellurium being metabolized by the body. When the body metabolizes tellurium in any oxidation state, the tellurium gets converted into dimethyl telluride, (CH3)2Te, which is volatile and is the cause of the garlic-like smell. Even though the metabolic pathways of tellurium are not known, it is generally assumed that they resemble those of the more extensively studied selenium, because the final methylated metabolic products of the two elements are similar.[61][62][63]

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