Tellurium tetrachloride

Tellurium tetrachloride  Tellurium tetrachloride

Names
IUPAC names

Tellurium(IV) chloride
Tetratellurium hexadecachloride

Other names

Tellurium chloride

Identifiers

CAS Number

* 10026-07-0 N

3D model (JSmol)

* monomer: Interactive image
* tetramer: Interactive image

ChemSpider |

* 55367 Y

ECHA InfoCard | 100.030.038

PubChem CID

* 61443

UNII |

* DNY2R5498H N

CompTox Dashboard (EPA)

* DTXSID1064904

InChI

* InChI=1S/Cl4Te/c1-5(2,3)4 Y

Key: SWLJJEFSPJCUBD-UHFFFAOYSA-N Y

* InChI=1/Cl4Te/c1-5(2,3)4

Key: SWLJJEFSPJCUBD-UHFFFAOYAL

SMILES

* monomer: Cl[Te](Cl)(Cl)Cl

* tetramer: [Cl+2]12[Te-2](Cl)(Cl)(Cl)3[Cl+2]4[Te-2](Cl)(Cl)(Cl)1[Cl+2]5[Te-2](Cl)(Cl)(Cl)2[Cl+2]3[Te-2]45(Cl)(Cl)(Cl)

Properties

Chemical formula

| TeCl4
Molar mass | 269.41 g/mol
Appearance  | hygroscopic pale yellow solid
(if fused, maroon liquid)
Density | 3.26 g/cm3, solid
Melting point | 224 °C (435 °F; 497 K)
Boiling point | 380 °C (716 °F; 653 K)

Solubility in water

| hot sulfur chloride[1]
Structure

Crystal structure

| Monoclinic, mS80

Space group

| C12/c1, No. 15

Coordination geometry

| Distorted octahedral (Te)

Molecular shape

| Seesaw (gas phase)

Dipole moment

| 2.59 D (gas phase)
Hazards
Occupational safety and health (OHS/OSH):

Main hazards

| Toxic, corrosive,
respiratory irritant
Related compounds

Other anions

| Tellurium tetrafluoride
Tellurium tetrabromide
Tellurium tetraiodide

Other cations

| Selenium tetrachloride
Polonium tetrachloride

Related compounds

| Tellurium dichloride

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

Chemical compound

Tellurium tetrachloride is the inorganic compound with the empirical formula TeCl4. The compound is volatile, subliming at 200 °C at 0.1 mmHg.[2] Molten TeCl4 is ionic, dissociating into TeCl3+ and Te2Cl102−.[2]

## Structure

[edit]

TeCl4 is monomeric in the gas phase, with a structure similar to that of SF4.[3] In the solid state, it is a tetrameric cubane-type cluster, consisting of a Te4Cl4 core and three terminal chloride ligands for each Te. Alternatively, this tetrameric structure can be considered as a Te4 tetrahedron with face-capping chlorines and three terminal chlorines per tellurium atom, giving each tellurium atom a distorted octahedral environment

## Synthesis

[edit]

TeCl4 is prepared by chlorination of tellurium powder:

Te + 2 Cl2 → TeCl4

The reaction is initiated with heat. The product is isolated by distillation.[4] Crude TeCl4 can be purified by distillation under an atmosphere of chlorine.[1]

Alternatively TeCl4 can be prepared using sulfuryl chloride (SO₂Cl₂) as a chlorine source.[1] Yet another method involves the reaction of tellurium with sulfur monochloride (S2Cl2) at room temperature. This exothermic reaction rapidly forms white needle-like crystals of TeCl4.[5]

## Reactions

[edit]

Tellurium tetrachloride is the gateway compound for high valent organotellurium compounds. Arylation gives, depending on conditions, Te(C6H4R)2Cl2, [Te(C6H4R)5]−, [Te(C6H4R)6]2−.[6]

TeCl4 has few applications in organic synthesis. Its equivalent weight is high, and the toxicity of organotellurium compounds is problematic. Possible applications of tellurium tetrachloride to organic synthesis have been reported.[7] It adds to alkenes to give Cl-C-C-TeCl3 derivatives, wherein the Te can be subsequently removed with sodium sulfide. Electron-rich arenes react to give aryl Te compounds. Thus, anisole gives TeCl2(C6H4OMe)2, which can be reduced to the diaryl telluride. TeCl4 is a precursor to tellurium-containing heterocycles like tellurophenes.[1]

Heating a mixture of TeCl4 and metallic tellurium gives tellurium dichloride (TeCl2).[8]

In moist air, TeCl4 forms tellurium oxychloride (TeOCl2), which further decomposes with excess water to form tellurous acid (H2TeO3).[8]

## Safety considerations

[edit]

As is the case for other tellurium compounds, TeCl4 is toxic. It also releases HCl upon hydrolysis.[1]

## References

[edit]

1. ^ a b c d e Petragnani, Nicola; Mendes, Samuel R.; Silveira, Claudio C. (2008-04-07). "Tellurium Tetrachloride: an improved method of preparation". Tetrahedron Letters. 49 (15): 2371–2372\. doi:10.1016/j.tetlet.2008.02.085. ISSN 0040-4039.
2. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
3. ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5
4. ^ Suttle, J. F.; Smith, C. R. F. (1950). Audrieth, Ludwig F. (ed.). Inorganic Syntheses. Vol. 3\. pp. 140–2\. doi:10.1002/9780470132340. ISBN 978-0-470-13162-6. `{{cite book}}`: ISBN / Date incompatibility (help)CS1 maint: multiple names: authors list (link)
5. ^ Lenher, Victor. "Tellurium Tetrachloride". Journal of the American Chemical Society. 24. doi:10.1021/ja02016a007.
6. ^ Miyasato, Masataka; Sagami, Takao; Minoura, Mao; Yamamoto, Yohsuke; Akiba, Kin-ya (2004). "Syntheses and Reactions of Hexavalent Organotellurium Compounds Bearing Five or Six Tellurium-Carbon Bonds". Chemistry – A European Journal. 10 (10): 2590–2600\. doi:10.1002/chem.200305260. PMID 15146530.
7. ^ Petragnani, N.; Comasseto, J. V. (1991). "Tellurium Reagents in Organic Synthesis; Recent Advances. Part 1". Synthesis. 1991 (10): 793–817\. doi:10.1055/s-1991-26577. S2CID 260335920. and Petragnani, N.; Comasseto, J. V. (1991). "Tellurium Reagents in Organic Synthesis; Recent Advances. Part 2". Synthesis. 1991 (11): 897–919\. doi:10.1055/s-1991-26605. S2CID 196716602.
8. ^ a b Simons, J. H. (1930-09-01). "The Properties of Tellurium Tetrachloride". Journal of the American Chemical Society. 52 (9): 3488–3493\. doi:10.1021/ja01372a003. ISSN 0002-7863.

* v
* t
* e

Tellurium compounds

* Te2Br
* TeBr4
* Te3Cl2
* TeCl2
* TeCl4
* TeF4
* TeF6
* TeI
* TeI4
* TeO
* TeO2
* TeO3
* Te(OH)6
* HOTeF5
* TeN
* TeO2−
4+TeO2−

* v
* t
* e

Salts and covalent derivatives of the chloride ion

| HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | B4Cl4
B12Cl12
BCl3
B2Cl4
+BO3 | C2Cl2
C2Cl4
C2Cl6
CCl4

+CO3 | NCl3
ClN3

+NO3 | ClxOy
Cl2O
Cl2O2
ClO
ClO2
Cl2O4
Cl2O6
Cl2O7
ClO4
+O | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | Si5Cl12
Si2Cl6
SiCl4 | P2Cl4
PCl3
PCl5
+P | S2Cl2
SCl2
SCl4
+SO4 | Cl2 | Ar
KCl | CaCl
CaCl2 |  | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2
MnCl3 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5
+As | Se2Cl2
SeCl2
SeCl4 | BrCl | Kr
RbCl | SrCl2 |  | YCl3 | ZrCl2
ZrCl3
ZrCl4 | NbCl3
NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl3
TcCl4 | RuCl2
RuCl3
RuCl4 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
XeCl4
CsCl | BaCl2 | *  | LuCl3 | HfCl4 | TaCl3
TaCl4
TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | ReCl3
ReCl4
ReCl5
ReCl6 | OsCl2
OsCl3
OsCl4
OsCl5 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
(Au[AuCl4])2
AuCl3 | Hg2Cl2
HgCl2 | TlCl
TlCl3 | PbCl2
PbCl4 | BiCl3 | PoCl2
PoCl4 | AtCl | Rn
FrCl | RaCl2 | **  | LrCl3 | RfCl4 | DbCl5 | SgO2Cl2 | BhO3Cl | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og

*  | LaCl3 | CeCl3 | PrCl3 | NdCl2
NdCl3 | PmCl3 | SmCl2
SmCl3 | EuCl2
EuCl3 | GdCl3 | TbCl3 | DyCl2
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3
**  | AcCl3 | ThCl3
ThCl4 | PaCl4
PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl3
NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3
CfCl2 | EsCl2
EsCl3 | FmCl2 | MdCl2 | NoCl2
*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
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