Germanium dichloride

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Germanium dichloride
Germanium dichloride.png
Names
Preferred IUPAC name
Germanium dichloride
Systematic IUPAC name
Dichlorogermanylidene
Other names
Dichlorogermylene

Germanium(II) chloride

Germanous chloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.162 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 233-192-1
PubChem CID
UNII
  • InChI=1S/Cl2Ge/c1-3-2
    Key: QHGIKMVOLGCZIP-UHFFFAOYSA-N
  • Cl[Ge]Cl
Properties
GeCl2
Molar mass 143.546 g/mol
Appearancewhite-pale yellow solid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

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.

Contents

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]

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.

GeHCl3 → GeCl2 + HCl

Another route to germanium dichloride is the reduction of germanium tetrachloride with hydrogen at 800 °C. [1]

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
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]

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.

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Germanium dichloride dioxane is a chemical compound with the formula GeCl2(C4H8O2), where C4H8O2 is 1,4-dioxane. It is a white solid. The compound is notable as a source of Ge(II), which contrasts with the pervasiveness of Ge(IV) compounds. This dioxane complex represents a well-behaved form of germanium dichloride.

References

  1. 1 2 3 4 5 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 376. ISBN   978-0-08-037941-8.
  2. ↑ Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN   0-12-352651-5
  3. ↑ Kociok-Köhn, G.; Winter, J. G.; Filippou, A. C. (1999). "Trimethylphosphonium trichlorogermanate(II)". Acta Crystallogr. C. 55 (3): 351–353. doi: 10.1107/S010827019801169X .
  4. ↑ Parshall, G. W. (1974). "Tetraethylammonium Trichlorogermanate(l-) and Trichlorostannate(l-)". Inorganic Syntheses. 15: 222–225. doi:10.1002/9780470132463.ch48. ISBN   9780470132463.
  5. ↑ 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.
  6. ↑ Egorov, M.P.; Gaspar, P. (1994). "Germanium: Organometallic chemistry". Encyclopedia of Inorganic chemistry. John Wiley & Sons. ISBN   0-471-93620-0.
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