Hydrogen telluride
Liquid hydrogen telluride in a test tube
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Tellurium, Te Hydrogen, H | |
Names | |
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IUPAC name
hydrogen telluride
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Other names
hydrotelluric acid
tellane tellurium hydride dihydrogen telluride tellurane | |
Identifiers | |
3D model (
JSmol ) |
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ChEBI | |
ChemSpider | |
ECHA InfoCard
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100.029.073 |
EC Number |
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PubChem CID
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
H2Te | |
Molar mass | 129.6158 g mol−1 |
Appearance | colourless gas |
Odor | Pungent, resembles rotting garlic or leeks |
Density | 3.310 g/L, gas 2.57 g/cm3 (−20 °C, liquid) |
Melting point | −49 °C (−56 °F; 224 K)[1] |
Boiling point | −2.2 °C (28.0 °F; 270.9 K) (unstable above −2 °C) |
0.70 g/100 mL | |
Acidity (pKa) | 2.6 |
Conjugate acid
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Telluronium |
Conjugate base
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Telluride |
Structure | |
bent | |
Thermochemistry | |
Std enthalpy of (ΔfH⦵298)formation |
0.7684 kJ/g |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
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toxic |
NFPA 704 (fire diamond) | |
Related compounds | |
Other anions
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H2Po
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Other cations
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Related compounds
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telluric acid tellurous acid stibine |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hydrogen telluride is the
Synthesis
Electrolytic methods have been developed.[3]
H2Te can also be prepared by hydrolysis of the telluride derivatives of electropositive metals.[4] The typical hydrolysis is that of aluminium telluride:
- Al2Te3 + 6 H2O → 2 Al(OH)3 + 3 H2Te
Other salts of Te2− such as MgTe and sodium telluride can also be used. Na2Te can be made by the reaction of Na and Te in anhydrous ammonia.[5] The intermediate in the hydrolysis, HTe−
, can be isolated as salts as well. NaHTe can be made by reducing tellurium with NaBH
4.[5]
Hydrogen telluride cannot be efficiently prepared from its constituent elements, in contrast to H2Se.[3]
Properties
H
2Te is an
- H
2Te → H
2 + Te
Light accelerates the decomposition. It is unstable in air, being oxidized to water and elemental tellurium:[6]
- 2 H
2Te + O
2 → 2 H
2O + 2 Te
It is almost as acidic as phosphoric acid (Ka = 8.1×10−3), having a Ka value of about 2.3×10−3.[6] It reacts with many metals to form tellurides.[7]
See also
References
- ISBN 0-8493-0487-3.
- ISBN 0-7506-3365-4.
- ^ a b F. Fehér, "Hydrogen Telluride" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. pp. 438.
- ^ Shriver, Atkins. Inorganic Chemistry, Fifth Edition. W. H. Freeman and Company, New York, 2010; pp 407.
- ^ ISBN 978-0-08-045310-1.
- ^ ISBN 0-12-352651-5.
- ^ Henry Enfield Roscoe; Carl Schorlemmer (1878). A treatise on chemistry. Vol. 1. Appleton. pp. 367–368.