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Germanium dichloride
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| Names | |
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| Preferred IUPAC name
Germanium dichloride | |
| Systematic IUPAC name
Dichlorogermanylidene | |
| Other names
Dichlorogermylene Germanium(II) chloride | |
| Identifiers | |
3D model (JSmol) |
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| ChemSpider | |
| ECHA InfoCard | 100.030.162 |
| EC Number |
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PubChem CID |
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| UNII | |
CompTox Dashboard (EPA) |
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| Properties | |
| GeCl2 | |
| Molar mass | 143.546 g/mol |
| Appearance | white-pale yellow solid |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Germanium dichloride is a chemical compound of germanium and chlorine with the formula GeCl2. It is a yellow solid. Germanium dichloride is an example of a compound featuring germanium in the +2 oxidation state.
Preparation
Solid germanium dichloride can be produced by comproportionation by passing germanium tetrachloride, GeCl4, over germanium metal at 300 °C and reduced pressure (0.1 mmHg).[1]
- 2 GeCl2"}},"i":0}}]}' id="mwGw"/>GeCl4 + Ge → 2 GeCl2
Germanium dichloride is also formed from the decomposition of trichlorogermane, GeHCl3, at 70 °C. Trichlorogermane is generated when germanium reacts with hydrogen chloride.[1] This reaction involves dehydrohalogenation.
- GeCl2 + HCl"}},"i":0}}]}' id="mwKA"/>GeHCl3 → GeCl2 + HCl
Another route to germanium dichloride is the reduction of germanium tetrachloride with hydrogen at 800 °C.[1]
- GeCl2 + 2HCl"}},"i":0}}]}' id="mwNA"/>GeCl4 + H2 → GeCl2 + 2HCl
Reactions
GeCl2 is hydrolysed to give yellow germanium(II) hydroxide, which on warming gives brown germanium monoxide:[1]
- GeCl2 + 2 H2O ⇌ Ge(OH)2(s) + 2 HCl
- GeO + H2O"}},"i":0}}]}' id="mwRA"/>Ge(OH)2 → GeO + H2O
Alkalizing a solution containing germanium(II) ions:
- Ge2+ + 2 OH− → Ge(OH)2
Germanium oxides and hydroxides are amphoteric. Solutions of GeCl2 in HCl are strongly reducing.[2] With chloride ion, ionic compounds containing the pyramidal GeCl−3 ion have been characterised, for example [3] With rubidium and caesium chloride compounds, e.g. RbGeCl3 are produced; these have distorted perovskite structures.[1]
Germanium dichloride reacts with tetraethylammonium chloride to give the trichlorogermanate:[4]
- Et4NGeCl3"}},"i":0}}]}' id="mwaA"/>GeCl2 + Et4NCl → Et4NGeCl3
Dichlorogermylene
Molecular GeCl2 is often called dichlorogermylene, highlighting its resemblance to a carbene. The structure of gas-phase molecular GeCl2 shows that it is a bent molecule, as predicted by VSEPR theory.[5] The dioxane complex, GeCl2·dioxane, has been used as a source of molecular GeCl2 for reaction syntheses, as has the in situ reaction of GeCl4 and Ge metal. GeCl2 is quite reactive and inserts into many types of chemical bonds.[6] Usually, germanium dichloride is generated from germanium dichloride dioxane.
References
- 1 2 3 4 5 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 376. doi:10.1016/C2009-0-30414-6. ISBN 978-0-08-037941-8.
- ↑ Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
- ↑ Kociok-Köhn, G.; Winter, J. G.; Filippou, A. C. (1999). "Trimethylphosphonium trichlorogermanate(II)". Acta Crystallogr. C. 55 (3): 351–353. Bibcode:1999AcCrC..55..351K. doi:10.1107/S010827019801169X.
- ↑ Parshall, G. W. (1974). Tetraethylammonium Trichlorogermanate(l-) and Trichlorostannate(l-). Inorganic Syntheses. Vol. 15. pp. 222–225. doi:10.1002/9780470132463.ch48. ISBN 9780470132463.
- ↑ 2</sub>. Equilibrium structure and anharmonic force field"},"last2":{"wt":"Honjou"},"first2":{"wt":"Hiroaki"},"last3":{"wt":"Tanaka"},"first3":{"wt":"Keiichi"},"last4":{"wt":"Tanaka"},"first4":{"wt":"Takehiko"},"last1":{"wt":"Tsuchiya"},"first1":{"wt":"Masaki J."},"journal":{"wt":"Journal of Molecular Structure"},"volume":{"wt":"352–353"},"year":{"wt":"1995"},"pages":{"wt":"407–415"},"doi":{"wt":"10.1016/0022-2860(95)08830-O"},"bibcode":{"wt":"1995JMoSt.352..407T"}},"i":0}}]}' id="mwyg"/>Tsuchiya, Masaki J.; Honjou, Hiroaki; Tanaka, Keiichi; Tanaka, Takehiko (1995). "Millimeter-wave spectrum of germanium dichloride GeCl2. Equilibrium structure and anharmonic force field". Journal of Molecular Structure. 352–353: 407–415. Bibcode:1995JMoSt.352..407T. doi:10.1016/0022-2860(95)08830-O.
- ↑ Egorov, M.P.; Gaspar, P. (1994). "Germanium: Organometallic chemistry". Encyclopedia of Inorganic chemistry. John Wiley & Sons. ISBN 0-471-93620-0.