Tellurium dioxide

α-TeO2, paratellurite

Names
Other names

Tellurium(IV) oxide

Identifiers

CAS Number

* 7446-07-3 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 56390 Y

PubChem CID

* 62638

UNII |

* 397E9RKE83 Y

InChI

* InChI=1S/O2Te/c1-3-2 Y

Key: LAJZODKXOMJMPK-UHFFFAOYSA-N Y

* InChI=1/O2Te/c1-3-2

Key: LAJZODKXOMJMPK-UHFFFAOYAO

SMILES

* O=[Te]=O

Properties

Chemical formula

| TeO2
Molar mass | 159.60 g/mol
Appearance  | white solid
Density | 5.670 g/cm3(orthorhombic)
6.04 g/cm3 (tetragonal) [1]
Melting point |  732 °C (1,350 °F; 1,005 K)
Boiling point |  1,245 °C (2,273 °F; 1,518 K)

Solubility in water

| negligible
Solubility | soluble in acid and alkali

Refractive index (nD)

| 2.24
Hazards
Flash point | Non-flammable
Related compounds

Other cations

| Sulfur dioxide
Selenium dioxide

Related tellurium oxides

| Tellurium trioxide
Tellurium monoxide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is YN ?)
Infobox references

Tellurium dioxide (TeO2) is a solid oxide of tellurium. It is encountered in two different forms, the yellow orthorhombic mineral tellurite, β-TeO2, and the synthetic, colourless tetragonal (paratellurite), α-TeO2.[2] Most of the information regarding reaction chemistry has been obtained in studies involving paratellurite, α-TeO2.[3]

## Contents

* 1 Preparation
* 2 Physical properties
* 3 Chemical properties
* 4 Structure
* 5 Uses
* 6 Safety
* 7 References
* 8 External links

## Preparation

Paratellurite, α-TeO2, is produced by reacting tellurium with O2:[2]

Te + O2 → TeO2

An alternative preparation is to dehydrate tellurous acid, H2TeO3, or to thermally decompose basic tellurium nitrate, Te2O4·HNO3, above 400 °C.[2]

## Physical properties

The longitudinal speed of sound in Tellurium dioxide is 4,260 metres per second (14,000 ft/s) at around room temperature.[4]

## Chemical properties

TeO2 is barely soluble in water and soluble in strong acids and alkali metal hydroxides.[5] It is an amphoteric substance and therefore can act both as an acid or as a base depending on the solution it is in.[6] It reacts with acids to make tellurium salts and bases to make tellurites. It can be oxidized to telluric acid or tellurates.

The tellurite ion is kinetically inert, but TeO2 equivalents will oxidize thioates in acid to the diacyl disulfide.[7]

## Structure

Paratellurite, α-TeO2, converts at high pressure into the β-, tellurite form.[8] Both the α-, (paratellurite) and β- (tellurite forms) contain four coordinate Te with the oxygen atoms at four of the corners of a trigonal bipyramid. In paratellurite all vertices are shared to give a rutile-like structure, where the O-Te-O bond angle are 140°. α-TeO2 In tellurite pairs of trigonal pyramidal, TeO4 units, sharing an edge, share vertices to then form a layer.[8] The shortest Te-Te distance in tellurite is 317 pm, compared to 374 pm in paratellurite.[8] Similar Te2O6 units are found in the mineral denningite.[8]

TeO2 melts at 732.6 °C, forming a red liquid.[9] The structure of the liquid, as well as the glass which can be formed from it with sufficiently rapid cooling, are also based on approximately four coordinate Te. However, compared to the crystalline forms, the liquid and glass appear to incorporate short-range disorder (a variety of coordination geometries) which marks TeO2 glass as distinct from the canonical single-oxide glass-formers such as SiO2, which share the same short-range order with their parent liquids.[10]

## Uses

It is used as an acousto-optic material.[4]

Tellurium dioxide is also a reluctant glass former, it will form a glass under suitable cooling conditions,[11] or with additions of a small molar fraction of a second compound such as an oxide or halide. TeO2 glasses have high refractive indices and transmit into the mid-infrared part of the electromagnetic spectrum, therefore they are of technological interest for optical waveguides. Tellurite glasses have also been shown to exhibit Raman gain up to 30 times that of silica, useful in optical fibre amplification.[12]

## Safety

TeO2 is a possible teratogen.[13]

Exposure to tellurium compounds produces a garlic-like odour on the breath, caused by the formation of diethyl telluride.[14]

## References

1. ↑ Pradyot Patnaik (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.
2. ↑ 2.0 2.1 2.2 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 911. ISBN 978-0-08-022057-4. https://books.google.com/books?id=OezvAAAAMAAJ&q=0-08-022057-6&dq=0-08-022057-6&source=bl&ots=m4tIRxdwSk&sig=XQTTjw5EN9n5z62JB3d0vaUEn0Y&hl=en&sa=X&ei=UoAWUN7-EM6ziQfyxIDoCQ&ved=0CD8Q6AEwBA.
3. ↑ W.R.McWhinnie (1995) Tellurium - Inorganic chemistry Encyclopedia of Inorganic Chemistry Ed. R. Bruce King (1994) John Wiley & Sons ISBN 978-0-471-93620-6
4. ↑ 4.0 4.1 "MODEL ATM SERIES ACOUSTO-OPTIC MODULATOR". https://intraaction.com/wp-content/themes/Divi/pdf/ATMModSeries08991.pdf.
5. ↑ Mary Eagleson (1994). Concise Encyclopedia Chemistry. Berlin: Walter de Gruyter. pp. 1081. ISBN 3-11-011451-8. https://archive.org/details/conciseencyclope00eagl.
6. ↑ K. W. Bagnall (1966). The Chemistry of Selenium, Tellurium and Polonium. London: Elsevier. pp. 59–60. ISBN 0-08-018855-9. https://archive.org/details/chemistryofsulph0000unse/page/59.
7. ↑ Subrahmanyan, T.; Aravamudan, G.; Rout, G. C.; Seshasayee, M. (1984). "Synthesis, properties, and molecular structure of bis(thiobenzoato-S)tellurium(II), C14H10O2S2Te(II)". Journal of Crystallographic and Spectroscopic Research (Plenum) 14 (3): 242–243. doi:10.1007/BF01161161. Bibcode: 1984JCCry..14..239S.
8. ↑ 8.0 8.1 8.2 8.3 Wells, A. F. (1984), Structural Inorganic Chemistry (5th ed.), Oxford: Clarendon Press, ISBN 0-19-855370-6
9. ↑ Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic chemistry. Academic Press. pp. 592–593. ISBN 0-12-352651-5.
10. ↑ Alderman, Oliver; Benmore, Chris; Feller, Steve; Kamitsos, Efstratios; Simandiras, Emmanuel; Liakos, Dimitrios; Jesuit, Martha; Boyd, Makyla et al. (2020). "Short-Range Disorder in TeO2 Melt and Glass". J. Phys. Chem. Lett. 11 (2): 427–431. doi:10.1021/acs.jpclett.9b03231. PMID 31867975.
11. ↑ Tagiara, N. S.; Palles, D.; Simandiras, E.; Psycharis, V.; Kyritsis, A.; Kamitsos, E. I. (2017). "Synthesis, thermal and structural properties of pure TeO2 glass and zinc-tellurite glasses". Journal of Non-Crystalline Solids 457: 116–125. doi:10.1016/j.jnoncrysol.2016.11.033.
12. ↑ "Tellurite glasses with peak absolute Raman gain coefficients up to 30 times that of fused silica". Optics Letters 28 (13): 1126–8. 2003. doi:10.1364/OL.28.001126. PMID 12879929. Bibcode: 2003OptL...28.1126S.
13. ↑ "Maternal toxicity and teratogenicity of tellurium dioxide in the Wistar rat: relationship to pair-feeding". Reprod. Toxicol. 2 (1): 55–61. 1988. doi:10.1016/S0890-6238(88)80009-1. PMID 2980402. Bibcode: 1988RepTx...2...55P.
14. ↑ Atta-ur-Rahman (2008). Studies in Natural Products Chemistry, Volume 35. Elsevier. p. 905. ISBN 978-0-444-53181-0. https://books.google.com/books?id=8Ugmrew2EqEC.

## External links

* TeO2 properties at Moltech Berlin
* Safety data for TeO2

* v
* t
* e

Tellurium compounds

* Te2Br
* TeBr4
* Te3Cl2
* TeCl4
* TeF4
* TeF6
* TeI4
* TeO
* TeO2
* TeO3
* TeN

* v
* t
* e

Oxides

Mixed oxidation states|

* Antimony tetroxide (Sb2O4)
* Cobalt(II,III) oxide (Co3O4)
* Europium(II,III) oxide (Eu3O4)
* Iron(II,III) oxide (Fe<sub>3O4)
* Lead(II,IV) oxide (Pb3O4)
* Manganese(II,III) oxide (Mn3O4)
* Silver(I,III) oxide (Ag2O2)
* Triuranium octoxide (U3O8)
* Carbon suboxide (C3O2)
* Mellitic anhydride (C12O9)
* [[Chemistry:Praseodymium(III,IV) Praseodymium(III,IV) oxide]] (Pr6O11)
* Terbium(III,IV) oxide (Tb4O7)

+1 oxidation state|

* Copper(I) oxide (Cu<sub>2O)
* Caesium oxide (Cs2O)
* Dicarbon monoxide (C2O)
* Dichlorine monoxide (Cl2O)
* Gallium(I) oxide (Ga2O)
* Lithium oxide (Li2O)
* Potassium oxide (K2O)
* Rubidium oxide (Rb2O)
* Silver oxide (Ag2O)
* Thallium(I) oxide (Tl2O)
* Sodium oxide (Na2O)
* Water (hydrogen oxide) (H2O)

+2 oxidation state|

* Aluminium(II) oxide (AlO)
* Barium oxide (BaO)
* Beryllium oxide (BeO)
* Cadmium oxide (CdO)
* Calcium oxide (CaO)
* Carbon monoxide (CO)
* Chromium(II) oxide (CrO)
* Cobalt(II) oxide (CoO)
* Copper(II) oxide (CuO)
* Europium(II) oxide (EuO)
* Germanium monoxide (GeO))
* Iron(II) oxide (FeO)
* Lead(II) oxide (PbO)
* Magnesium oxide (MgO)
* Manganese(II) oxide (MnO)
* Mercury(II) oxide (HgO)
* Nickel(II) oxide (NiO)
* Nitric oxide (NO)
* Palladium(II) oxide (PdO)
* Silicon monoxide (SiO)
* Strontium oxide (SrO)
* Sulfur monoxide (SO)
* Disulfur dioxide (S2O2)
* Thorium monoxide (ThO)
* Tin(II) oxide (SnO)
* Titanium(II) oxide (TiO)
* Vanadium(II) oxide (VO)
* Zinc oxide (ZnO)

+3 oxidation state|

* Aluminium oxide (Al<sub>2O3)
* Antimony trioxide (Sb2O3)
* Arsenic trioxide (As2O3)
* Bismuth(III) oxide (Bi2O3)
* Boron trioxide (B2O3)
* Cerium(III) oxide (Ce2O3)
* Dibromine trioxide (Br2O3)
* Chromium(III) oxide (Cr2O3)
* Dinitrogen trioxide (N2O3)
* Dysprosium(III) oxide (Dy2O3)
* Erbium(III) oxide (Er2O3)
* Europium(III) oxide (Eu2O3)
* Gadolinium(III) oxide (Gd2O3)
* Gallium(III) oxide (Ga2O3)
* Holmium(III) oxide (Ho2O3)
* Indium(III) oxide (In<sub>2O3)
* Iron(III) oxide (Fe2O3)
* Lanthanum oxide (La2O3)
* Lutetium(III) oxide (Lu2O3)
* Manganese(III) oxide (Mn2O3)
* Neodymium(III) oxide (Nd2O3)
* Nickel(III) oxide (Ni2O3)
* Phosphorus trioxide (P4O6)
* Praseodymium(III) oxide (Pr2O3)
* Promethium(III) oxide (Pm2O3)
* Rhodium(III) oxide (Rh2O3)
* [[Chemistry:Samarium(III) Samarium(III) oxide]] (Sm2O3)
* Scandium oxide (Sc2O3)
* Terbium(III) oxide (Tb2O3)
* Thallium(III) oxide (Tl2O3)
* Thulium(III) oxide (Tm2O3)
* Titanium(III) oxide (Ti2O3)
* Tungsten(III) oxide (W2O3)
* Vanadium(III) oxide (V2O3)
* Ytterbium(III) oxide (Yb2O3)
* Yttrium(III) oxide (Y2O3)

+4 oxidation state|

* Americium dioxide (AmO2)
* Carbon dioxide (CO2)
* Carbon trioxide (CO3)
* Cerium(IV) oxide (CeO2)
* Chlorine dioxide (ClO2)
* Chromium(IV) oxide (CrO<sub>2)
* Dinitrogen tetroxide (N2O4)
* Germanium dioxide (GeO<sub>2)
* [[Chemistry:Hafnium(IV) Hafnium(IV) oxide]] (HfO2)
* Lead dioxide (PbO2)
* Manganese dioxide (MnO2)
* Neptunium(IV) oxide (NpO2)
* Nitrogen dioxide (NO2)
* Osmium dioxide (OsO2)
* Plutonium(IV) oxide (PuO2)
* Praseodymium(IV) oxide (PrO2)
* Protactinium(IV) oxide (PaO2)
* Rhodium(IV) oxide (RhO2)
* Ruthenium(IV) oxide (RuO<sub>2)
* Selenium dioxide (SeO2)
* Silicon dioxide (SiO2)
* Sulfur dioxide (SO2)
* Tellurium dioxide (TeO<sub>2)
* [[Chemistry:Terbium(IV) Terbium(IV) oxide]] (TbO2)
* Thorium dioxide (ThO2)
* Tin dioxide (SnO2)
* Titanium dioxide (TiO<sub>2)
* Tungsten(IV) oxide (WO2)
* Uranium dioxide (UO2)
* Vanadium(IV) oxide (VO2)
* Zirconium dioxide (ZrO2)

+5 oxidation state|

* Antimony pentoxide (Sb2O5)
* Arsenic pentoxide (As2O5)
* Dinitrogen pentoxide (N2O5)
* Niobium pentoxide (Nb2O5)
* Phosphorus pentoxide (P2O5)
* Protactinium(V) oxide (Pa2O5)
* Tantalum pentoxide (Ta2O5)
* Vanadium(V) oxide (V2O5)

+6 oxidation state|

* Chromium trioxide (CrO3)
* Molybdenum trioxide (MoO3)
* Rhenium trioxide (ReO3)
* Selenium trioxide (SeO3)
* Sulfur trioxide (SO3)
* Tellurium trioxide (TeO3)
* Tungsten trioxide (WO3)
* Uranium trioxide (UO3)
* Xenon trioxide (XeO3)
* Iridium trioxide (IrO3)

+7 oxidation state|

* Dichlorine heptoxide (Cl2O7)
* Manganese heptoxide (Mn2O7)
* [[Chemistry:Rhenium(VII) Rhenium(VII) oxide]] (Re2O7)
* Technetium(VII) oxide (Tc2O7)

+8 oxidation state|

* Osmium tetroxide (OsO4)
* Ruthenium tetroxide (RuO4)
* Xenon tetroxide (XeO4)
* Iridium tetroxide (IrO4)
* Hassium tetroxide (HsO4)

Related|

* Oxocarbon
* Suboxide
* Oxyanion
* Ozonide
* Peroxide
* Superoxide

Oxides are sorted by oxidation state. Category:Oxides

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