| |
| Identifiers | |
|---|---|
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.033.271 |
| EC Number |
|
PubChem CID
|
|
CompTox Dashboard (EPA)
|
|
| |
| |
| 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 labelling:[4] | |
| |
| Danger | |
| H314 | |
| P260, P264, P264+P265, P280, P301+P330+P331, P302+P361+P354, P304+P340, P305+P354+P338, P316, P317, P321, P363, P405, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
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]
- GeO2 + 4 HI → GeI4 + 2 H2O
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 GeI4 + 15 Fe2(CO)9 → Ge12[Fe(CO)3]8I4 + 22 FeI2 + 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
- ^ a b c A. W. Laubengayer, P. L. Brandt (Feb 1932). "The Preparation of Germanium Tetrabromide and Germanium Tetraiodide". Journal of the American Chemical Society. 54 (2): 621–623. doi:10.1021/ja01341a502. ISSN 0002-7863. Archived from the original on 2021-10-20. Retrieved 2021-01-12.
- ^ a b L. M. Dennis, F. E. Hance (Dec 1922). "GERMANIUM. IV. GERMANIUM TETRA-IODIDE1". Journal of the American Chemical Society. 44 (12): 2854–2860. doi:10.1021/ja01433a020. ISSN 0002-7863. Retrieved 2021-01-12.
- ^ a b Schenk, P.W. (1963). "12. Silicon and Germanium". In Brauer, Georg (ed.). 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.
- ^ "Germanium tetraiodide". pubchem.ncbi.nlm.nih.gov.
- ^ 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". Journal of Non-Crystalline Solids. 411: 40–44. Bibcode:2015JNCS..411...40V. doi:10.1016/j.jnoncrysol.2014.09.018. Retrieved 2021-01-12.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ 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". Chemical Communications. 54 (10): 1217–1220. doi:10.1039/C7CC08091C. ISSN 1359-7345. PMID 29336437. Retrieved 2021-01-12.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ 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.
This page was last edited on 26 October 2023, at 08:15