Hydrogen telluride

Liquid hydrogen telluride in a test tube

Tellurium, Te

Hydrogen, H

Names
IUPAC name

hydrogen telluride

Other names

hydrotelluric acid
tellane
tellurium hydride
dihydrogen telluride

Identifiers

CAS Number

* 7783-09-7 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:30452 N

ChemSpider |

* 20455 N

EC Number |

* 236-813-4

PubChem CID

* 21765

UNII |

* 7F4735942K N

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 (pKa)  | 2.6
Conjugate acid | Telluronium
Conjugate base | Telluride
Structure

Molecular shape

| bent
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| 0.7684 kJ/g
Hazards
Main hazards | Highly toxic and flammable
NFPA 704 (fire diamond)  |

Related compounds

Other anions

| H2O
H2S
H2Se
H2Po

Other cations

| Li2Te
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

Tracking categories (test):

* SizeSet

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 its rotting garlic-like odour at extremely low concentrations, or by the revolting odour of rotting leeks that it has 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, and 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]

## Contents

* 1 Synthesis
* 2 Properties
* 3 See also
* 4 References

## 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 NaBH4.[5]

Hydrogen telluride cannot be efficiently prepared from its constituent elements, in contrast to H2Se.[3]

## Properties

H2Te is an endothermic compound, degrading to the elements at room temperature:

H2Te → H2 \+ Te

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

2 H2Te \+ O2 → 2 H2O \+ 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

* Dimethyl telluride

## References

1. ↑ Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
2. ↑ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
3. ↑ 3.0 3.1 F. Fehér, "Hydrogen Telluride" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. pp. 438.
4. ↑ Shriver, Atkins. Inorganic Chemistry, Fifth Edition. W. H. Freeman and Company, New York, 2010; pp 407.
5. ↑ 5.0 5.1 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.
6. ↑ 6.0 6.1 Egon Wiberg; Arnold Frederick Holleman (2001). Nils Wiberg. ed. Inorganic chemistry. Academic Press. p. 589. ISBN 0-12-352651-5.
7. ↑ Henry Enfield Roscoe; Carl Schorlemmer (1878). A treatise on chemistry. 1. Appleton. pp. 367–368.

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Hydrogen compounds

* H3AsO3
* H3AsO4
* HArF
* HAt
* HSO3F
* HBF4
* HBr
* HBrO
* HBrO2
* HBrO3
* HBrO4
* HCl
* HClO
* HClO2
* HClO3
* HClO4
* HCN
* HCNO
* H2CrO4/H2Cr2O7
* H2CO3
* H2CS3
* HF
* HFΟ
* HI
* HIO
* HIO2
* HIO3
* HIO4
* HMnO4
* H2MoO4
* HNC
* NaHCO3
* HNCO
* HNO
* HNO2
* HNO3
* H2N2O2
* HNO5S
* H3NSO3
* H2O
* H2O2
* H2O3
* H3PO2
* H3PO3
* H3PO4
* H4P2O7
* H5P3O10
* H2PtCl6
* H2S
* H2S2
* H2Se
* H2SeO3
* H2SeO4
* H4SiO4
* H2SiF6
* HSCN
* HNSC
* H2SO3
* H2SO4
* H2SO5
* H2S2O3
* H2S2O6
* H2S2O7
* H2S2O8
* CF3SO3H
* H2Te
* H2TeO3
* H6TeO6
* H4TiO4
* H2Po
* HCo(CO)4

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Binary compounds of hydrogen

Alkali metal (Group 1) hydrides|

* LiH
* NaH
* KH
* RbH
* CsH

Lithium hydride, LiH
ionic metal hydride

Beryllium hydride
Left (gas phase): BeH2
covalent metal hydride
Right: (BeH2)n (solid phase)
polymeric metal hydride

Borane and diborane
Left: BH3 (special conditions), covalent metalloid hydride
Right: B2H6 (standard conditions), dimeric metalloid hydride

Methane, CH4
covalent nonmetal hydride

Ammonia, NH3
covalent nonmetal hydride

Water, H2O
covalent nonmetal hydride

Hydrogen fluoride, HF
covalent nonmetal hydride

Alkaline (Group 2) earth hydrides|

| Monohydrides|

* BeH
* MgH
* CaH
* SrH
* BaH

|

Dihydrides|

* BeH2
* MgH2
* CaH2
* SrH2
* BaH2

|

Group 13 hydrides|

| Boranes|

* BH3
* B2H6
* B2H2
* B2H4
* B4H10
* B5H9
* B5H11
* B6H10
* B6H12
* B10H14
* B18H22

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Alanes|

* AlH3
* Al2H6

|

Gallanes|

* GaH3
* Ga2H6

|

Indiganes|

* InH3
* In2H6

|

Thallanes|

* TlH3
* Tl2H6

|

Group 14 hydrides|

| Linear alkanes|

* CH4
* C2H6
* C3H8
* C4H10
* C5H12
* C6H14
* C7H16
* C8H18
* C9H20
* C10H22
* more...

|

Linear alkenes|

* C2H4
* C3H6
* C4H8
* C5H10
* C6H12
* C7H14
* C8H16
* C9H18
* C10H20
* more...

|

Linear alkynes|

* C2H2
* C3H4
* C4H6
* C5H8
* C6H10
* C7H12
* C8H14
* C9H16
* C10H18
* more...

|

Silanes|

* SiH4
* Si2H6
* Si3H8
* Si4H10
* Si5H12
* Si6H14
* Si7H16
* Si8H18
* Si9H20
* Si10H22
* more...

|

Silenes|

* Si2H4

|

Silynes|

* Si2H2
* SiH

|

Germanes|

* GeH4
* Ge2H6
* Ge3H8
* Ge4H10
* Ge5H12

|

Stannanes|

* SnH4
* Sn2H6

|

Plumbanes|

* PbH4

|

* CH
* CH2
* CH3
* C2H
* Cycloalkanes
* Cycloalkenes
* Annulenes
* Many more

Pnictogen (Group 15) hydrides|

| Azanes|

* NH3
* N2H4
* N3H5
* N4H6
* N5H7
* N6H8
* N7H9
* N8H10
* N9H11
* N10H12
* more...

|

Azenes|

* N2H2
* N3H3
* N4H4

|

Phosphanes|

* PH3
* P2H4
* P3H5
* P4H6
* P5H7
* P6H8
* P7H9
* P8H10
* P9H11
* P10H12
* more...

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Phosphenes|

* P2H2
* P3H3
* P4H4

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Arsanes|

* AsH3
* As2H4

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Stibanes|

* SbH3

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Bismuthanes|

* BiH3

|

* HN3
* NH
* radical

Hydrogen chalcogenides (Group 16 hydrides)|

| Polyoxidanes|

* H2O
* H2O2
* H2O3
* H2O4
* H2O5
* H2O6
* H2O7
* H2O8
* H2O9
* H2O10
* more...

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Polysulfanes|

* H2S
* H2S2
* H2S3
* H2S4
* H2S5
* H2S6
* H2S7
* H2S8
* H2S9
* H2S10
* more...

|

Selanes|

* H2Se
* H2Se2

|

Tellanes|

* H2Te
* H2Te2

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Polanes|

* PoH2

|

* HO
* HO2
* HO3
* H2O+–O–
* H2S=S
* (HS)2S+–S–
* HS
* HDO
* D2O
* T2O

Hydrogen halides (Group 17 hydrides)|

* HF
* HCl
* HBr
* HI
* HAt

Transition metal hydrides|

* ScH2
* YH2
* YH3
* TiH2
* ZrH2
* HfH2
* VH
* VH2
* NbH
* NbH2
* TaH
* CrH
* CrH2
* CrHx
* NiH
* PdHx (x < 1)
* FeH
* FeH2
* FeH5
* CuH
* ZnH2
* CdH2
* HgH2

Lanthanide hydrides|

* LaH2
* LaH3
* LaH10
* CeH2
* CeH3
* PrH2
* PrH3
* NdH2
* NdH3
* SmH2
* SmH3
* EuH2
* GdH2
* GdH3
* TbH2
* TbH3
* DyH2
* DyH3
* HoH2
* HoH3
* ErH2
* ErH3
* TmH2
* TmH3
* YbH2
* YbH2.5
* LuH2
* LuH3

Actinide hydrides|

* AcH2
* ThH2
* Th4H15
* PaH3
* UH3
* NpH2
* NpH3
* PuH2
* PuH3
* AmH2
* AmH3
* CmH2

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Tellurides

| H2Te |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  | He

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Li2Te | BeTe |  |  |  |  |  |  |  |  |  |  | B  | CTe2
(CH3)2Te | (NH4)2Te | O  | F  | Ne
Na2Te | MgTe |  |  |  |  |  |  |  |  |  |  | Al2Te | Si  | P2Te5 | S  | Cl  | Ar
K2Te | CaTe | Sc2Te3 | Ti  | VTe2 | CrTe
Cr2Te3 | MnTe
MnTe2 | FeTe | CoTe | NiTe | CuTe | ZnTe | GaTe
Ga2Te3 | GeTe | As2Te3
As4Te3 | Se  | Br  | Kr
Rb2Te | SrTe | Y2Te3 | Zr  | NbTe2 | MoTe2 | Tc  | Ru  | Rh  | Pd  | Ag2Te | CdTe | In2Te3 | SnTe
SnTe2 | Sb2Te3 | Te2- | I  | Xe
Cs2Te | BaTe | *  | Hf  | TaTe2 | WTe2
WTe3 | ReTe2 | Os  | Ir  | Pt  | AuxTey | HgTe | Tl2Te | PbTe | Bi2Te3 | Po  | At  | Rn
Fr  | Ra  | **  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og  |  |  |  |  |  |  |  |
|  | ↓ |  |  |  |  |  |  |  |  |  |  |  |  |  |  |
| * | La2Te3 | Ce2Te3 | Pr2Te3 | Nd2Te3 | Pm  | Sm2Te3 | Eu2Te3 | Gd  | Tb  | Dy  | Ho  | Er2Te3 | Tm2Te3 | Yb  | Lu  |
| ** | Ac  | ThTe2 | Pa  | UTe2 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr  |

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