Chemistry:Germanium(IV) iodide
| |
| Identifiers | |
|---|---|
3D model (JSmol)
|
|
| ChemSpider | |
| EC Number |
|
PubChem CID
|
|
| |
| |
| Properties | |
| GeI4 | |
| Molar mass | 580.248 g·mol−1 |
| Appearance | red crystals[1] (For colors at different temperatures, see this document)[2] |
| Density | 4.32 g·cm−3 |
| Melting point | 146 °C (419 K)[1] |
| Solubility | Soluble in non-polar solvents such as carbon disulfide, chloroform and benzene[3] |
| Hazards | |
| GHS pictograms | 
|
| GHS Signal word | Danger |
| H314 | |
| P260, P264, P264+265Script error: No such module "Preview warning".Category:GHS errors, P280, P301+330+331, P302+361+354Script error: No such module "Preview warning".Category:GHS errors, P304+340, P305+354+338Script error: No such module "Preview warning".Category:GHS errors, P316Script error: No such module "Preview warning".Category:GHS errors, P317Script error: No such module "Preview warning".Category:GHS errors, P321, P363, P405, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Germanium(IV) iodide is an inorganic compound with the chemical formula GeI4.
Preparation
Germanium(IV) iodide can be obtained by the reaction of germanium and iodine[2] or the reaction of germanium dioxide and 57% hydriodic acid:[1]
- GeO
2 + 4 HI → GeI
4 + 2 H
2O
Chemical properties
Germanium(IV) iodide reacts with tetraalkyl tin at 250 °C to form R2SnI2 and R2GeI2 (R= Et, Bu, Ph).[5] It reacts with germanium and sulfur at high temperatures to produce red GeSI2 and orange Ge2S3I2.[6] It reacts with diiron nonacarbonyl in an ionic liquid ([BMIm]Cl/AlCl3) at 130 °C to obtain Ge12[Fe(CO)3]8I4.[7]
- 12 GeI
4 + 15 Fe
2(CO)
9 → Ge
12[Fe(CO)
3]
8I
4 + 22 FeI
2 + 111 CO↑
Physical properties
Germanium(IV) iodide is an orange-red crystalline solid that hydrolyzes in water. It is soluble in carbon disulfide and benzene, but less soluble in carbon tetrachloride and chloroform.[3] It begins to decompose into germanium(II) iodide and iodine above its melting point.[8] Germanium(IV) iodide crystallizes in the cubic crystal system, space group Pa3 (space group no. 205), with the lattice parameter a = 11.89 Å. The crystal structure consists of tetrahedral GeI4 molecules.
References
- ↑ 1.0 1.1 1.2 A. W. Laubengayer, P. L. Brandt (Feb 1932). "The Preparation of Germanium Tetrabromide and Germanium Tetraiodide" (in en). Journal of the American Chemical Society 54 (2): 621–623. doi:10.1021/ja01341a502. ISSN 0002-7863. https://pubs.acs.org/doi/abs/10.1021/ja01341a502. Retrieved 2021-01-12.
- ↑ 2.0 2.1 L. M. Dennis, F. E. Hance (Dec 1922). "GERMANIUM. IV. GERMANIUM TETRA-IODIDE1" (in en). Journal of the American Chemical Society 44 (12): 2854–2860. doi:10.1021/ja01433a020. ISSN 0002-7863. https://pubs.acs.org/doi/abs/10.1021/ja01433a020. Retrieved 2021-01-12.
- ↑ 3.0 3.1 Schenk, P.W. (1963). "12. Silicon and Germanium". in Brauer, Georg. Handbook of preparative inorganic chemistry (Second ed.). Academic Press. p. 719. doi:10.1016/B978-0-12-395590-6.50020-X. ISBN 978-0-12-395590-6. https://archive.org/details/handbookpreparat00brau.
- ↑ "Germanium tetraiodide" (in en). https://pubchem.ncbi.nlm.nih.gov/compound/83479#section=Safety-and-Hazards.
- ↑ Kocheshkov, K. A.; Fomina, N. V.; Sheverdina, N. I.; Zemlyanskii, N. N.; Chernoplekova, V. A. Reaction of tetraalkyltin with germanium tetrahalides. Izvestiya Akademii Nauk SSSR, Seriya Khimicheskaya, 1973. 3: 711. ISSN: 0002-3353.
- ↑ A.P. Velmuzhov, M.V. Sukhanov, A.D. Plekhovich, A.I. Suchkov, V.S. Shiryaev (Mar 2015). "Thermal decomposition study of GeSI2 and Ge2S3I2 glassy alloys" (in en). Journal of Non-Crystalline Solids 411: 40–44. doi:10.1016/j.jnoncrysol.2014.09.018. Bibcode: 2015JNCS..411...40V. https://linkinghub.elsevier.com/retrieve/pii/S0022309314004736. Retrieved 2021-01-12.
- ↑ Silke Wolf, Wim Klopper, Claus Feldmann (2018). "Ge 12 {Fe(CO) 3 } 8 (μ-I) 4 : a germanium–iron cluster with Ge 4 , Ge 2 and Ge units" (in en). Chemical Communications 54 (10): 1217–1220. doi:10.1039/C7CC08091C. ISSN 1359-7345. PMID 29336437. http://xlink.rsc.org/?DOI=C7CC08091C. Retrieved 2021-01-12.
- ↑ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1995). Lehrbuch der anorganischen Chemie (101., verb. und stark erw. Aufl ed.). Berlin: de Gruyter. ISBN 978-3-11-012641-9.
| HI | He | ||||||||||||||||
| LiI | BeI2 | BI3 | CI4 | NI3 | I2O4, I2O5, I4O9 |
IF, IF3, IF5, IF7 |
Ne | ||||||||||
| NaI | MgI2 | AlI3 | SiI4 | PI3, P2I4 |
S | ICl, ICl3 |
Ar | ||||||||||
| KI | CaI2 | Sc | TiI4 | VI3 | CrI3 | MnI2 | FeI2 | CoI2 | NiI2 | CuI | ZnI2 | Ga2I6 | GeI2, GeI4 |
AsI3 | Se | IBr | Kr |
| RbI | SrI2 | YI3 | ZrI4 | NbI5 | Mo | Tc | Ru | Rh | Pd | AgI | CdI2 | InI3 | SnI4, SnI2 |
SbI3 | TeI4 | I | Xe |
| CsI | BaI2 | HfI4 | TaI5 | W | Re | Os | Ir | Pt | AuI | Hg2I2, HgI2 |
TlI | PbI2 | BiI3 | Po | AtI | Rn | |
| Fr | RaI2 | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La | Ce | Pr | Nd | Pm | SmI2 | Eu | Gd | TbI3 | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | ThI4 | Pa | UI3, UI4 |
Np | Pu | Am | Cm | Bk | Cf | EsI3 | Fm | Md | No | Lr | |||
 |  |
