| Hydrogen telluride | |
|---|---|
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| IUPAC name |
hydrogen telluride
|
| Other names | hydrotelluric acid tellane tellurium hydride |
| Identifiers | |
| CAS number | 7783-09-7 |
| PubChem | 21765 |
| Properties | |
| Molecular formula | H2Te |
| Molar mass | 129.6158 g mol−1 |
| Appearance | colourless gas |
| Density | 3.310 g/cm3, gas 2.57 g/cm3 (-20 °C, liquid) |
| Melting point |
−49 °C [1] |
| Boiling point |
−2.2 °C (unstable above -2 °C) |
| Solubility in water | 0.70 g/100 mL |
| Acidity (pKa) | 2.6 |
| Structure | |
| Molecular shape | bent |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
0.7684 kJ/g |
| Hazards | |
| Main hazards | toxic |
| Related compounds | |
| Other anions | H2O H2S H2Se H2Po |
| Other cations | Na2Te Ag2Te |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
| Infobox references | |
Hydrogen telluride is the inorganic compound with the formula H2Te. The simplest hydride of tellurium, it is rarely encountered because of its tendency to decompose to the constituent elements. Most compounds with Te-H bonds are unstable with respect to loss of H2. H2Te is chemically and structurally similar to hydrogen selenide, both are acidic species with H-X-H angles approaching 90°.[2]
Contents |
Synthesis
H2Te is prepared by the acidification of salts of Te2−, such as Al2Te3 and Na2Te. Na2Te can be generated by the reaction of Na and Te in anhydrous ammonia. The intermediate in the acidification, HTe− is a stable anion.
Properties
H2Te is an endothermic compound, and is unstable in air, rapidly decomposing into water and elemental tellurium:[3]
- 2 H2Te + O2 → 2 H2O + 2 Te
It is almost as acidic as phosphoric acid (pKa=8.1×10−3), having a pKa value of about 2.3×10−3.[3] It reacts with many metals to form tellurides.[4]
See also
References
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
- ^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
- ^ a b Egon Wiberg; Arnold Frederick Holleman (2001). Nils Wiberg. ed. Inorganic chemistry. Academic Press. p. 589. ISBN 0123526515.
- ^ Henry Enfield Roscoe; Carl Schorlemmer (1878). A treatise on chemistry. 1. Appleton. pp. 367-368.
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