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(Top) 1 Synthesis 2 Properties 3 See also 4 References

Hydrogen telluride

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Hydrogen telluride
Names
Liquid hydrogen telluride in a test tube

Tellurium, Te Hydrogen, H
IUPAC name hydrogen telluride
Other names hydrotelluric acid tellane tellurium hydride dihydrogen telluride tellurane
Identifiers
CAS Number	7783-09-7^Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:30452^N
ChemSpider	20455^N
ECHA InfoCard	100.029.073
EC Number	236-813-4
PubChem CID	21765
UNII	7F4735942K^N
CompTox Dashboard (EPA)	DTXSID20228446
InChI InChI=1S/H2Te/h1H2^N Key: VTLHPSMQDDEFRU-UHFFFAOYSA-N^N
SMILES [TeH2]
Properties
Chemical formula	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)
Solubility in water	0.70 g/100 mL
Acidity (pK_a)	2.6
Conjugate acid	Telluronium
Conjugate base	Telluride
Structure
Molecular shape	bent
Thermochemistry
Std enthalpy of formation (Δ_fH^⦵₂₉₈)	0.7684 kJ/g
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	toxic
NFPA 704 (fire diamond)	4 4 1
Related compounds
Other anions	H₂O H₂S H₂Se H₂Po
Other cations	Na₂Te Ag₂Te K₂Te Rb₂Te Cs₂Te
Related compounds	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). N verify (what is ^YN ?) Infobox references

Hydrogen telluride is the inorganic compound with the formula H₂Te. A hydrogen chalcogenide and the simplest hydride of tellurium, it is a colorless gas. Although unstable in ambient air, the gas can exist long enough to be readily detected by the odour of rotting garlic at extremely low concentrations; or by the revolting odour of rotting leeks at somewhat higher concentrations. Most compounds with Te–H bonds (tellurols) are unstable with respect to loss of H₂. H₂Te is chemically and structurally similar to hydrogen selenide, both are acidic. The H–Te–H angle is about 90°. Volatile tellurium compounds often have unpleasant odours, reminiscent of decayed leeks or garlic.^[2]

Synthesis[edit]

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[edit]

H
₂Te is an endothermic compound, degrading to the elements at room temperature:

H
₂Te → H
₂ + Te

Light accelerates the decomposition. It is unstable in air, being oxidized to water and elemental tellurium:^[6]

2H
₂Te + O
₂ → 2 H
₂O + 2 Te

It is almost as acidic as phosphoric acid (K_a = 8.1×10⁻³), having a K_a value of about 2.3×10⁻³.^[6] It reacts with many metals to form tellurides.^[7]

References[edit]

^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.

^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. 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.

^ ^a ^b Nicola Petragnani; Hélio A. Stefani (2007). Tellurium in organic synthesis. Best synthetic methods (2nd ed.). Academic Press. p. 6. ISBN 978-0-08-045310-1.

^ ^a ^b Egon Wiberg; Arnold Frederick Holleman (2001). Nils Wiberg (ed.). Inorganic chemistry. Translated by Mary Eagleson. Academic Press. p. 589. ISBN 0-12-352651-5.

^ Henry Enfield Roscoe; Carl Schorlemmer (1878). A treatise on chemistry. Vol. 1. Appleton. pp. 367–368.