Chemistry:Germanium(II) iodide
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3D model (JSmol)
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PubChem CID
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| Properties | |
| GeI2 | |
| Molar mass | 326.439 g·mol−1 |
| Appearance | yellow solid[1] |
| Density | 5.37 g·cm−3 (25 °C)[2] |
| Melting point | 428 °C[3] |
| Boiling point | 550 °C (decomposes)[3] |
| Structure | |
| P3m1 (No. 164)[4] | |
| Related compounds | |
Other anions
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germanium(II) fluoride germanium(II) chloride germanium(II) bromide |
Other cations
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tin(II) iodide lead(II) iodide |
Related compounds
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germanium(IV) iodide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Germanium(II) iodide is an iodide of germanium, with the chemical formula of GeI2.
Preparation
Germanium(II) iodide can be produced by reacting germanium(IV) iodide with hydriodic acid and hypophosphorous acid and water:[1]
- GeI
4 + H
2O + H
3PO
2 → GeI
2 + H
3PO
3 + 2 HI
It can also be formed by the reaction of germanium monosulfide or germanium monoxide and hydrogen iodide.[1]
- GeO + 2 HI → GeI
2 + H
2O
- GeS + 2 HI → GeI
2 + H
2S}
It can also be produced from the direct reaction of germanium and iodine at 200 – 400 °C:[1]
- Ge + I
2 → GeI
2
Germanium(II) iodide can also be formed from the decomposition of HGeI3, which can be prepared by reacting HGeCl3 with hydroiodic acid:[5]
- HGeCl
3 + 3 HI → HGeI
3 + HCl
- HGeI
3 → GeI
2 + HI
Properties
Germanium(II) iodide is a yellow crystal that slowly hydrolyzes into germanium(II) hydroxide in the presence of moisture. It is insoluble in hydrocarbons and slightly soluble in chloroform and carbon tetrachloride. It has a cadmium iodide structure with lattice parameters a = 413 pm and c = 679 pm.[1] It disproportionates to germanium and germanium tetraiodide at 550 °C.[6]
Applications
Germanium(II) iodide can react with carbene to form stable compounds.[2] It is also used in the electronics industry to produce germanium layers epitaxially through disproportionation reactions.[7]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 Georg Brauer (Hrsg.), unter Mitarbeit von Marianne Baudler u. a.: Handbuch der Präparativen Anorganischen Chemie. 3., umgearbeitete Auflage. Band I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6, S. 727.
- ↑ 2.0 2.1 Sigma-Aldrich Co., product no. {{{id}}}.
- ↑ 3.0 3.1 William M. Haynes (2012), CRC Handbook of Chemistry and Physics, 93rd Edition, CRC Press, pp. 4–65, ISBN 978-143988049-4, https://books.google.com/books?id=-BzP7Rkl7WkC&pg=PA4-65
- ↑ Jean d’Ans, Ellen Lax, Roger Blachnik (1998), Taschenbuch für Chemiker und Physiker, Springer DE, pp. 472, ISBN 364258842-5, https://books.google.com/books?id=ssy59etLaksC&pg=PA472
- ↑ Wolfgang Kirmse (2013), Carbene Chemistry 2e, Elsevier, pp. 540, ISBN 978-032316145-9, https://books.google.com/books?id=T3dnOIFjwWwC&pg=PA540
- ↑ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils, ed., Inorganic Chemistry, San Diego/Berlin: Academic Press/De Gruyter, p. 959, ISBN 0-12-352651-5
- ↑ A.G. Milnes (1972), Heterojunctions and Metal Semiconductor Junctions, Elsevier, pp. 104, ISBN 032314136-6, https://books.google.com/books?id=Ox3JhIg40hcC&pg=PA104
| 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 | |||
 |  |
