13494-80-9 Usage
Chemical Properties
Different sources of media describe the Chemical Properties of 13494-80-9 differently. You can refer to the following data:
1. Tellurium is a heavy metal, which is processed as a grey powder. It has hexagonal, rhombohedral structure, a low water solubility and high relative density. The particle size ranges from 52.36 to 112.98 μm.
Tellurium is a silvery white metal in group 16 of the periodic table. It shares chemical and clinical properties with selenium(Amdur, 1947, 1958; Schroeder et al., 1967; Shie andDeeds, 1920). Telluriumis a semiconductor and may have multiple electron states (-2, 0, +2, +4, +6). It can react with hydrogen to form hydrogen telluride and with halogens. Tellurite (+2) and teleurate (+4) compounds are water soluble. Elemental tellurium burns, producing a blue flame and tellurium dioxide.
2. Tellurium is a grayish or silvery white, lustrous, crystalline, semimetallic element. It may exist in a hexagonal crystalline form or an amorphous powder.Soluble in sulfuric acid, nitric acid, potassium hydroxide, and potassium cyanide solutions; insoluble in water. Imparts garlic-like odor to breath, can be depilatory. It is a ptype semiconductor and its conductivity is sensitive to light exposure. It is found in sulfide ores and is produced as a by-product of copper or bismuth refining.
History
Different sources of media describe the History of 13494-80-9 differently. You can refer to the following data:
1. The element was discovered by Muller von Reichenstein in 1782 while investigating a bluish-white ore of gold. The element was isolated from this ore by Klaproth in 1798, who suggested the name “tellurium” after the Latin word tellus, meaning earth. Tellurium occurs in nature only in minute quantities. It is found in small amounts in many sulfide deposits. One of the more common tellurium minerals is calaverite, AuTe2 , in which the metal is combined with gold. Some other tellurium minerals are altaite, PbTe; sylvanite, (Ag,Au)Te2; rickardite, Cu4Te3; tetradymite, Bi2Te2S; petzite, Ag3AuTe2 and coloradoite, HgTe. The metal is found in the native state and also in the form of its dioxide, tellurite, TeO2. The abundance of tellurium in the earth’s crust is estimated to be about 1 μg/kg.
2. Discovered by Muller von Reichenstein in 1782; named
by Klaproth, who isolated it in 1798. Tellurium is occasionally
found native, but is more often found as the telluride of
gold (calaverite), and combined with other metals. It is recovered
commercially from the anode muds produced during
the electrolytic refining of blister copper. The U.S., Canada,
Peru, and Japan are the largest producers of the element.
Crystalline tellurium has a silvery-white appearance, and
when pure exhibits a metallic luster. It is brittle and easily pulverized.
Amorphous tellurium is formed by precipitating tellurium
from a solution of telluric or tellurous acid. Whether
this form is truly amorphous, or made of minute crystals, is
open to question. Tellurium is a p-type semiconductor, and
shows greater conductivity in certain directions, depending
on alignment of the atoms. Its conductivity increases slightly
with exposure to light. It can be doped with silver, copper,
gold, tin, or other elements. In air, tellurium burns with a
greenish-blue flame, forming the dioxide. Molten tellurium
corrodes iron, copper, and stainless steel. Tellurium and its
compounds are probably toxic and should be handled with
care. Workmen exposed to as little as 0.01 mg/m3 of air, or
less, develop “tellurium breath,” which has a garlic-like odor.
Forty-two isotopes and isomers of tellurium are known, with
atomic masses ranging from 106 to 138. Natural tellurium
consists of eight isotopes, two of which are radioactive with
very long half-lives. Tellurium improves the machinability of
copper and stainless steel, and its addition to lead decreases
the corrosive action of sulfuric acid on lead and improves its
strength and hardness. Tellurium catalysts are used in the oxidation
of organic compounds and are used in hydrogenation
and halogenation reactions. Tellurium is also used in electronic
and semiconductor devices. It is also used as a basic
ingredient in blasting caps, and is added to cast iron for chill
control. Tellurium is used in ceramics. Bismuth telluride has
been used in thermoelectric devices. Tellurium costs about
50￠/g, with a purity of about 99.5%. The metal with a purity
of 99.9999% costs about $5/g.
Uses
Different sources of media describe the Uses of 13494-80-9 differently. You can refer to the following data:
1. Small amounts of tellurium are added to stainless steel and copper to improve their machinability. It enhances the strength and hardness of lead and protects lead from the corrosive action of sulfuric acid. Tellurium also is a strong chilling agent in iron castings. It controls the chill and imparts a tough abrasion resistance to the surface.
Tellurium is a curing agent for natural and synthetic rubber. It improves mechanical properties of the rubber imparting resistance to heat and abrasion. Tellurium is a coloring agent in glass, ceramics, and enamels. Traces of tellurium incorporated into platinum catalysts make the catalytic hydrogenation of nitric oxide favorable to forming hydroxylamine. A major application of tellurium is in semiconductor research. Tellurides of lead and bismuth are used in thermoelectric devices for power generation and refrigeration.
2. Tellurium is a common constituent of ores that contain silver, gold, lead, antimony, and bismuth, and it is often present in small amounts in coal. Tellurium is widely used in metallurgy because it improves the properties of copper, tin, lead-based alloys, steel, and cast iron. It is used in rubber manufacturing to increase heat resistance and to retard the aging of rubber hoses and cable coatings. Small amounts are used in the electronics industry for lasers and photoreceptors. Tellurium is not an essential micronutrient; therefore, it is not found in nutritional supplements.
As coloring agent in chinaware, porcelains, enamels, glass; reagent in producing black finish on silverware; in manufacture of special alloys of marked electrical resistance; in semiconductor research.
3. Tellurium’s major use is as an alloy with copper and stainless steel. It makes these metalseasier to machine and mill (cut on a lathe). It is also used as a vulcanizing agent in the productionof rubber, as a coloring agent for glass and ceramics, and for thermoelectrical devices.Along with lithium, it is used to make special batteries for spacecraft and infrared lamps.Tellurium can be used as a p-type semiconductor, but more efficient elements can do a betterjob. It is also used as a depilatory, which removes hair from skin.Although tellurium forms many compounds, most of them have little commercial value.
4. The metal is used in vulcanizing rubber, instorage batteries, and as a coloring agent inceramics. It is also used as an additive toiron, steel, and copper. Many tellurium saltsfind application on semiconductors.
Production Methods
Different sources of media describe the Production Methods of 13494-80-9 differently. You can refer to the following data:
1. Tellurium is recovered from the anode slimes produced in electrolytic refining of copper. Other metals present in these slimes are gold, silver, and selenium, which are all recovered as by-products in the extraction of tellurium. Tellurium is leached with caustic soda solution and the leachate upon neutralization precipitates tellurium dioxide, TeO2, in crude and impure form. A part of tellurium remaining in the slimes can be recovered during extraction of gold and silver. In this gold and silver recovery process, tellurium incorporates into the soda slag obtained from roasting the slimes in a furnace. Soda slag is produced when leached with a solution of caustic soda. The liquor is neutralized to form a crude precipitate of tellurium dioxide.
Crude tellurium dioxide is dissolved in a strong solution of caustic soda to form sodium tellurite. Electrolysis of sodium tellurite solution deposits tellurium metal on the stainless steel cathode.
Also, the tellurium metal can be prepared by thermal reduction of dioxide. However, prior to reduction crude dioxide is refined by successive caustic leaching and neutralization steps mentioned above.
Refined tellurium contains traces of lead, copper, iron, selenium, and other impurities. Highly pure tellurium can be obtained either by distilling refined tellurium in vacuum or by the zone melting process. The last traces of selenium can be removed as hydride by treating molten tellurium with hydrogen.
2. Elemental tellurium (Te) has some metallic properties,
although it is classed as a nonmetal or metalloid. The
name is derived from the Latin word for earth, tellus.
Tellurium is occasionally found naturally, more often as
telluride of gold, calaverite. The elemental form has a bright
luster, is brittle, readily powders, and burns slowly in air.
Tellurium exists in two allotropic forms, in the form of
powder and hexagonal crystalline (isomorphous) with gray
selenium. The concentration in the earth’s crust is about
0.002 ppm. It is recovered from anode muds during the
refining of blister copper. It is also found in various sulfide
ores along with selenium and is produced as a by-product of
metal refineries. The United States, Canada, Peru, and Japan
are the largest producers.
Tellurium’s industrial applications include its use as a
metallurgical additive to improve the characteristics of alloys
of copper, steel, lead, and bronze. Increased ductility results
from its use in steel and copper alloys. Addition of tellurium
to cast iron is used for chill control, and it is a basic part of
blasting caps. It is used in some chemical processes as a
catalyst for synthetic fiber production, and as a vulcanizing
agent and accelerator in the processing of rubber.
Description
Tellurium is one of the rarest elements on earth similar to
selenium, and was discovered in Transylvania in 1782 by
Franz-Joseph Muller von Reichenstein. The name derived from
the Latin word for earth. Tellurium is occasionally found
naturally, more often as telluride of gold, calaverite.
Physical properties
Tellurium is a silver-white, brittle crystal with a metallic luster and has semiconductorcharacteristics. It is a metalloid that shares properties with both metals and nonmetals, andit has some properties similar to selenium and sulfur, located just above it in group 16 of theperiodic table.There are two allotropic forms of tellurium: (1) the crystalline form that has a silvery metallicappearance and a density of 6.24 g/cm3, a melting point of 499.51°C, and a boiling point of988°C; and (2) the amorphous allotrope that is brown in color and has a density of 6.015g/cm3and ranges for the melting and boiling point temperatures similar to the crystalline form.
Isotopes
There are a total of 48 isotopes of tellurium. Eight of these are consideredstable. Three of the stable ones are actually radioactive but have such long half-livesthat they still contribute to the natural abundance of tellurium in the crust of the Earth.The isotope Te-123 (half-life of 6×10+14 years) contributes 0.89% of the total telluriumfound on Earth, Te-128 (half-life of 7.7×10+24 years) contributes 31.74% to the naturalabundance, and Te-130 (half-life of 0.79×10+21 years) contributes 34.08% to the telluriumin the Earth’s crust. The other five stable isotopes and the percentage of theirnatural abundance are as follows: Te-120 = 0.09%, Te-122 = 2.55%, Te-124 = 4.74%,Te-125 = 7.07%, and Te-126 = 18.84%. The other 40 isotopes are all radioactive withshort half-lives.
Origin of Name
The name “tellurium” is derived from the Latin word for Earth, tellus.
Occurrence
Tellurium is the 71st most abundant element on Earth. It makes up a small portion ofigneous rocks and is sometimes found as a free element, but is more often recovered fromseveral ores. Its major ores are sylvanite (AgAuTe4), also known as graphic tellurium, calaverite,sylvanite, and krennerite, all with the same general formula (AuTe2). Other minor ores arenagyagite, black tellurium, hessite, altaite, and coloradoite. In addition, it is recovered fromgold telluride (AuTe2). Significant quantities are also recovered from the anode “slime” of theelectrolytic refining process of copper production.
Characteristics
The pure form of tellurium burns with a blue flame and forms tellurium dioxide (TeO2).It is brittle and is a poor conductor of electricity. It reacts with the halogens of group 17, butnot with many metals. When it reacts with gold, it forms gold telluride. Tellurium is insolublein water but readily reacts with nitric acid to produce tellurous acid. If inhaled, it produces agarlic-like odor on one’s breath.
Definition
Different sources of media describe the Definition of 13494-80-9 differently. You can refer to the following data:
1. A nonmetallic element with
many properties similar to selenium and sulfur.
Atomic number 52; group VIA of the period table;
aw 127.60; valences of 2, 4, 6; eight stable isotopes.
2. tellurium: Symbol Te. A silvery metalloidelement belonging to group16 (formerly VIB) of the periodictable; a.n. 52; r.a.m. 127.60; r.d. 6.24(crystalline); m.p. 449.5°C; b.p.989.8°C. It occurs mainly as telluridesin ores of gold, silver, copper,and nickel and it is obtained as a byproductin copper refining. There areeight natural isotopes and nine radioactiveisotopes. The element is usedin semiconductors and smallamounts are added to certain steels.Tellurium is also added in smallquantities to lead. Its chemistry issimilar to that of sulphur. It was discoveredby Franz Müller (1740–1825)in 1782.
General Description
Grayish-white, lustrous, brittle, crystalline solid; dark-gray to brown, amorphous powder with metallic characteristics. Used as a coloring agent in chinaware, porcelains, enamels, glass; producing black finish on silverware; semiconductor devices and research; manufacturing special alloys of marked electrical resistance. Improves mechanical properties of lead; powerful carbide stabilizer in cast iron, Tellurium vapor in "daylight" lamps, vulcanization of rubber. Blasting caps. Semiconductor research.
Reactivity Profile
Tellurium is attacked by chlorine fluoride with incandescence. When Tellurium and potassium are warmed in an atmosphere of hydrogen, combination occurs with incandescence [Mellor 11:40. 1946-47]. Burning Tellurium produces toxic Tellurium oxide gas. Avoid solid sodium, halogens, interhalogens, metals, hexalithium disilicide. Reacts with nitric acid; reacts with concentrated sulfuric acid forming a red solution. Dissolves in potassium hydroxide in the presence of air with formation of deep red solution; combines with halogens. Avoid antimony and chlorine trifluoride; chlorine trifluoride reacts vigorously with Tellurium producing flame. Fluorine and Tellurium react with incandescence. Lithium silicide attacks Tellurium with incandescence. Reaction with zinc is accompanied by incandescence (same potential with cadmium, only hazard is less). A vigorous reaction results when liquid Tellurium is poured over solid sodium [EPA, 1998].
Hazard
All forms of tellurium are toxic in gas form. The vapors of all the compounds of the dustand powder forms of the element should not be inhaled or ingested. When a person is poisonedwith tellurium, even in small amounts, the breath will smell like garlic.
Health Hazard
Although tellurium in elemental form haslow toxicity, ingestion can produce nausea,vomiting, tremors, convulsions, and centralnervous system depression. In addition,exposure to the metal or to its compoundscan generate garlic-like odor in breath, sweat,and urine. Such odor is imparted by dimethyltelluride that is formed in the body. Oralintake of large doses of the metal or itscompounds can be lethal. Clinical symptomsare similar for most tellurium salts,which include headache, drowsiness, lossof appetite, nausea, tremors, and convulsions.High exposure can produce metallictaste, dry throat, chill and other symptoms.Inhalation of dust or fume of the metalcan cause irritation of the respiratory tract.Chronic exposure can produce bronchitis andpneumonia.
Fire Hazard
A finely divided suspension of elemental Tellurium in air will explode. Insoluble in water. Burning Tellurium produces toxic Tellurium oxide gas. Avoid solid sodium, halogens, interhalogens, metals, hexalithium disilicide. Reacts with nitric acid; reacts with concentrated sulfuric acid forming a red solution. Dissolves in potassium hydroxide in the presence of air with formation of deep red solution; combines with halogens. Avoid antimony and chlorine trifluoride; chlorine trifluoride reacts vigorously with Tellurium producing flame. Fluorine and Tellurium react with incandescence. Lithium silicide attacks Tellurium with incandescence. Reaction with zinc is accompanied by incandescence (same potential with cadmium, only hazard is less). A vigorous reaction results when liquid Tellurium is poured over solid sodium.
Flammability and Explosibility
Nonflammable
Safety Profile
Poison by ingestion and intratracheal routes. An experimental teratogen. Exposure causes nausea, vomiting, tremors, convulsions, respiratory arrest, central nervous system depression, and garlic odor to breath. Aerosols of tellurium, tellurium dioxide, and hydrogen telluride cause irritation of the respiratory system and may lead to the development of bronchitis and pneumonia. Experimental reproductive effects. Under the proper conditions it undergoes hazardous reactions with halogens (e.g., chlorine, fluorine), interhalogens (e.g., bromine pentafluoride, chlorine fluoride, chlorine trifluoride), metals (e.g., cadmium, potassium, sodium, platinum, tin, zinc), hexalithium disilicide, silver bromate, silver iodate. When heated to decomposition it emits toxic fumes of Te. See also TELLURIUM COMPOUNDS.
Potential Exposure
The primary use of tellurium is in the vulcanization of rubber and as an additive in ferritic steel production. It is also used as a carbide stabilizer in cast iron, a chemical catalyst; a coloring agent in glazes and glass; a thermocoupling material in refrigerating equipment; as an additive to selenium rectifiers; in alloys of lead, copper, steel, and tin for increased resistance to corrosion and stress, workability, machinability, and creep strength; and in certain culture media in bacteriology. Since tellurium is present in silver, copper, lead, and bismuth ores, exposure may occur during purification of these ores.
Environmental Fate
Metals are recalcitrant to degradation; therefore, no biodegradation studies have been performed on tellurium. No aquatic bioaccumulation data exist for tellurium; however, based on its density and low water solubility, it is unlikely to present a concern for bioaccumulation in the water column. No environmental monitoring data are available on the levels of tellurium in sediment or sediment-dwelling organisms. Therefore, it is unclear whether tellurium has the potential to bioaccumulate in this compartment. In humans, tellurium accumulates in the bones. Based on this, it may be assumed that tellurium has the potential to bioaccumulate in vertebrates.
Purification Methods
Purify it by zone refining and repeated sublimation to an impurity of less than 1 part in 108 (except for surface contamination by TeO2). [Machol & Westrum J Am Chem Soc 80 2950 1958.] Tellurium is volatile at 500o/0.2mm. It has also been purified by electrode deposition [Mathers & Turner Trans Amer Electrochem Soc 54 293 1928].
Toxicity evaluation
Tellurium has a low toxicity in its elemental form, but dimethyltelluride
is formed in the body. Tellurium caused a highly
synchronous primary demyelination of peripheral nerves,
related to the inhibition of squalene epoxidase, which blocks
cholesterol synthesis. The sequence of metabolic events in
sciatic nerve following tellurium treatment initially involves
inhibition of the conversion of squalene to 2,3-epoxysqualene,
and this block in the cholesterol biosynthesis pathway results,
either directly or indirectly, in the inhibition of the synthesis of
myelin components and the breakdown of myelin. The efficacy
of garlic as a lipid-lowering agent has been recognized, but the
biochemical mechanisms underlying this action are currently
unknown. It is possible that organic tellurium compounds,
which are found in high concentration in fresh garlic buds, may
contribute to this action by inhibiting squalene epoxidase, the
penultimate enzyme in the synthetic pathway of cholesterol.
Weanling rats fed a diet rich in tellurium develop a demyelinating
polyneuropathy because of inhibition of this enzyme in
peripheral nerves. Chronic exposure to small amounts of
tellurium found in garlic might reduce endogenous cholesterol production through inhibition of hepatic squalene epoxidase
and so reduce cholesterol levels. Tellurium may also contribute
to the characteristic odor of garlic.
Incompatibilities
Finely divided powder or dust may be flammable and explosive. Violent reaction with halogens, interhalogens, zinc and lithium silicide; with incandescence. Incompatible with oxidizers, cadmium; strong bases; chemically active metals; silver bromate; nitric acid.
Check Digit Verification of cas no
The CAS Registry Mumber 13494-80-9 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,3,4,9 and 4 respectively; the second part has 2 digits, 8 and 0 respectively.
Calculate Digit Verification of CAS Registry Number 13494-80:
(7*1)+(6*3)+(5*4)+(4*9)+(3*4)+(2*8)+(1*0)=109
109 % 10 = 9
So 13494-80-9 is a valid CAS Registry Number.
InChI:InChI=1/Te
13494-80-9Relevant articles and documents
Efficient quenching of TGA-capped CdTe quantum dot emission by a surface-coordinated europium(III) cyclen complex
Gallagher, Shane A.,Comby, Steve,Wojdyla, Michal,Gunnlaugsson, Thorfinnur,Kelly, John M.,Gun'Ko, Yurii K.,Clark, Ian P.,Greetham, Gregory M.,Towrie, Michael,Quinn, Susan J.
, p. 4133 - 4135 (2013)
Extremely efficient quenching of the excited state of aqueous CdTe quantum dots (QDs) by photoinduced electron transfer to a europium cyclen complex is facilitated by surface coordination to the thioglycolic acid capping ligand. The quenching dynamics are elucidated using steady-state emission and picosecond transient absorption.
Electron energy loss spectroscopy (EELS) of H2O, H2S, H2Se and H2Te
Pradeep, T.,Hegde, M. S.
, p. 883 - 888 (1988)
Electronic excitation in H2O, H2S, H2Se and H2Te molecules has been studied by the EELS technique.Spectra of H2S and H2Se are remarkably similar with the 1b1-nd transition most intense.The intensity of the first transition 1b1-nsa1 decreases through H2O to H2Se and this transition is absent in H2Te.Transitions observed by EELS have been compared with optical absorption studies.A correlation diagram of the occupied and the excited states has been provided for these four molecules by making use of UVPES and EELS.
Synthesis and structures of new ternary aluminum chalcogenides: LiAlSe2, α-LiAlTe2, and β-LiAlTe2
Kim, Joonyeong,Hughbanks, Timothy
, p. 3092 - 3097 (2000)
The synthesis and crystal structures of new ternary aluminum chalcogenides, LiAlSe2, α-LiAlTe2, and β-LiAlTe2, are reported. These compounds are synthesized by solid-state reaction at 800 °C. The single-crystal X-ray structures of these compounds have been determined. LiAlSe2: a = 6.8228(9) A, b = 8.266(1) A, c = 6.5236(7) A, Pna21 (No. 33, Z = 4). α-LiAlTe2: a = 6.5317(4) A, c = 11.6904(9) A, I42d (No. 122, Z = 4). β-LiAlTe2: a = 4.4810(6) A, c = 7.096(1) A, P3m1 (No. 156, Z = 1). These ternary compounds are formed by fusion of AlQ4 (Q = Se, Te) tetrahedra. LiAlSe2 shows β-NaFeO2 structure type, which can be viewed as a wurtzite superstructure. α-LiAlTe2 adopts chalcopyrite structure type. In LiAlSe2 and α-LiAlTe2, AlQ4 (Q = Se, Te) tetrahedra share four corners to build three-dimensional structures and Li atoms are located in the tetrahedral sites between the chalcogen layers. β-LiAlTe2 has polar layers formed by three-corner shared AlTe4 tetrahedra, and Li cations are in the distorted antiprisms between the layers. 7Li MAS NMR studies show that chemical shifts of Li in these ternary chalcogenides are nearly identical regardless of different chemical environments.
Spectroscopic behavior of cationic metallophthalocyanines in the presence of anionic quantum dots
Idowu, Mopelola,Nyokong, Tebello
, p. 411 - 416 (2010)
The interactions and spectroscopic properties between cationic zinc phthalocyanine derivatives (peripherally and non-peripherally tetrasubstituted and peripherally octa substituted with 2-diethylmethylaminoethylsulfanyl (βTZnPc, αTZnPc and βOZnPc)) and CdTe core quantum dots (QDs) capped with mercaptopropionic acid or thioglycolic acid (represented as CdTe@MPA and CdTe@TGA, respectively) have been studied in methanol:water mixture. Strong coupling of MPcs was deduced from the interaction since the UV-vis spectroscopic studies of the ground state complex formed on mixing both components showed loss of the phthalocyanine monomeric band with the formation of a dimeric band (spectrum of aggregated species). The dimerization constants were of the order of 104 M-1.
Matrix isolation study of D2Te and H2Te molecules in solid argon
Montano, P. A.,Nagarathna, H. M.,Newlin, D.,Stewart, G. W.
, p. 5558 - 5560 (1981)
A careful synthesis of H2Te and D2Te and their isolation in solid argon are reported.Rare gas metrix isolated molecules of H2Te and D2Te were studied using Moessbauer spectroscopy.The gaseous species were identified using mass spectrometry.Moessbauer parameters were analyzed using extended Hueckel calculations.A good agreement between the experimental and the calculated value of the quadrupole splitting requires a smaller quadrupole moment for the excited state of 125Te then that reported in the literature.A 10percent increase in the QS for D2Te is explained as due to the enhancement of 3> caused by a slight contraction of the D-Te bond.
NiTe2 Nanowire Outperforms Pt/C in High-Rate Hydrogen Evolution at Extreme pH Conditions
Anantharaj, Sengeni,Karthick, Kannimuthu,Kundu, Subrata
, p. 3082 - 3096 (2018)
Better hydrogen generation with nonprecious electrocatalysts over Pt is highly anticipated in water splitting. Such an outperforming nonprecious electrocatalyst, nickel telluride (NiTe2), has been fabricated on Ni foam for electrocatalytic hydrogen evolution in extreme pH conditions, viz., 0 and 14. The morphological outcome of the fabricated NiTe2 was directed by the choice of the Te precursor. Nanoflakes (NFs) were obtained when NaHTe was used, and nanowires (NWs) were obtained when Te metal powder with hydrazine hydrate was used. Both NiTe2 NWs and NiTe2 NFs were comparatively screened for hydrogen evolution reaction (HER) in extreme pH conditions, viz., 0 and 14. NiTe2 NWs delivered current densities of 10, 100, and 500 mA cm-2 at the overpotentials of 125 ± 10, 195 ± 4, and 275 ± 7 mV in 0.5 M H2SO4. Similarly, in 1 M KOH, overpotentials of 113 ± 5, 247 ± 5, and 436 ± 8 mV were required for the same current densities, respectively. On the other hand, NiTe2 NFs showed relatively poorer HER activity than NiTe2 NWs, which required overpotentials of 193 ± 7, 289 ± 5, and 494 ± 8 mV in 0.5 M H2SO4 for the current densities of 10 and 100 mA cm-2 and 157 ± 5 and 335 ± 6 mV in 1 M KOH for the current densities of 10 and 100 mA cm-2, respectively. Notably, NiTe2 NWs outperformed the state-of-the-art Pt/C 20 wt % loaded Ni foam electrode of comparable mass loading. The Pt/C 20 wt % loaded Ni foam electrode reached 500 mA cm-2 at 332 ± 5 mV, whereas NiTe2 NWs drove the same current density with 57 mV less. These encouraging findings emphasize that a NiTe2 NW could be an alternative to noble and expensive Pt as a nonprecious and high-performance HER electrode for proton-exchange membrane and alkaline water electrolyzers.
Reactivity of uranium(iii) with H2E (E = S, Se, Te): Synthesis of a series of mononuclear and dinuclear uranium(iv) hydrochalcogenido complexes
Franke, Sebastian M.,Rosenzweig, Michael W.,Heinemann, Frank W.,Meyer, Karsten
, p. 275 - 282 (2015)
We report the syntheses, electronic properties, and molecular structures of a series of mono- and dinuclear uranium(iv) hydrochalcogenido complexes supported by the sterically demanding but very flexible, single N-anchored tris(aryloxide) ligand (AdArO)3N)3-. The mononuclear complexes [((AdArO)3N)U(DME)(EH)] (E = S, Se, Te) can be obtained from the reaction of the uranium(iii) starting material [((AdArO)3N)UIII(DME)] in DME via reduction of H2E and the elimination of 0.5 equivalents of H2. The dinuclear complexes [{((AdArO)3N)U}2(μ-EH)2] can be obtained by dissolving their mononuclear counterparts in non-coordinating solvents such as benzene. In order to facilitate the work with the highly toxic gases, we created concentrated THF solutions that can be handled using simple glovebox techniques and can be stored at -35 °C for several weeks. This journal is
Heavy hydrides: H2Te ultraviolet photochemistry
Underwood,Chastaing,Lee,Wittig
, (2005)
The room-temperature ultraviolet absorption spectrum of H2 Te has been recorded. Unlike other group-6 hydrides, it displays a long-wavelength tail that extends to 400 nm. Dissociation dynamics have been examined at photolysis wavelengths of 266 nm (which lies in the main absorption feature) and 355 nm (which lies in the long-wavelength tail) by using high- n Rydberg time-of-flight spectroscopy to obtain center-of-mass translational energy distributions for the channels that yield H atoms. Photodissociation at 355 nm yields TeH (Π 12 2) selectively relative to the TeH (Π 32 2) ground state. This is attributed to the role of the 3 A′ state, which has a shallow well at large RH-TeH and correlates to H+TeH (Π 12 2). Note that the Π 12 2 state is analogous to the P 12 2 spin-orbit excited state of atomic iodine, which is isoelectronic with TeH. The 3 A′ state is crossed at large R only by 2 A″, with which it does not interact. The character of 3 A′ at large R is influenced by a strong spin-orbit interaction in the TeH product. Namely, Π 12 2 has a higher degree of spherical symmetry than does Π 32 2 (recall that I (P 12 2) is spherically symmetric), and consequently Π 12 2 is not inclined to form either strongly bonding or antibonding orbitals with the H atom. The 3 A′ ←X transition dipole moment dominates in the long-wavelength region and increases with R. Structure observed in the absorption spectrum in the 380-400 nm region is attributed to vibrations on 3 A′. The main absorption feature that is peaked at ～240 nm might arise from several excited surfaces. On the basis of the high degree of laboratory system spatial anisotropy of the fragments from 266 nm photolysis, as well as high-level theoretical studies, the main contribution is believed to be due to the 4 A″ surface. The 4 A″ ←X transition dipole moment dominates in the Franck-Condon region, and its polarization is in accord with the experimental observations. An extensive secondary photolysis (i.e., of nascent TeH) is observed at 266 and 355 nm, and the corresponding spectral features are assigned. Analyses of the c.m. translational energy distributions yield bond dissociation energies D0. For H2 Te and TeH, these are 65.0±0.1 and 63.8±0.4 kcalmol, respectively, in good agreement with predictions that use high-level relativistic theory.
Dynamic distribution of growth rates within the ensembles of colloidal II-VI and III-V semiconductor nanocrystals as a factor governing their photoluminescence efficiency
Talapin, Dmitri V.,Rogach, Andrey L.,Shevchenko, Elena V.,Kornowski, Andreas,Haase, Markus,Weller, Horst
, p. 5782 - 5790 (2002)
The distribution of properties within ensembles of colloidally grown II-VI and III-V semiconductor nanocrystals was studied. A drastic difference in the photoluminescence efficiencies of size-selected fractions was observed for both organometallically prepared CdSe and InAs colloids and for CdTe nanocrystals synthesized in aqueous medium, indicating a general character of the phenomenon observed. The difference in the photoluminescence efficiencies is attributed to different averaged surface disorder of the nanocrystals originating from the Ostwald ripening growth mechanism when larger particles in the ensemble grow at the expense of dissolving smaller particles. At any stage of growth, only a fraction of particles within the ensemble of growing colloidal nanocrystals has the most perfect surface and, thus, shows the most efficient photoluminescence. This is explained by a theoretical model describing the evolution of an ensemble of nanocrystals in a colloidal solution. In an ensemble of growing nanocrystals, the fraction of particles with the highest photoluminescence corresponds to the particle size having nearly zero average growth rate. The small average growth rate leads to the lowest possible degree of surface disorder at any given reaction conditions.
