Rubidium germanium iodide

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Rubidium germanium iodide
Identifiers
3D model (JSmol)
  • InChI=1S/Ge.3HI.Rb/h;3*1H;/q+2;;;;+1/p-3
    Key: BMENQWFJSMYCLV-UHFFFAOYSA-K
  • [Ge+2].[I-].[I-].[I-].[Rb+]
Properties
GeI3Rb
Molar mass 538.811 g·mol−1
Melting point 61 °C (decomposes)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Rubidium germanium iodide is a ternary halide of rubidium and germanium, with the chemical formula RbGeI3. It is being considered as a potential counterpart to the toxic CH3NH3PbI3 for photovoltaic applications. [1]

Contents

Preparation

Rubidium germanium iodide can be prepared by reacting germanium(II) hydroxide and rubidium iodide in hydroiodic acid: [2]

Ge(OH)2 + RbI + 2 HI → GeRbI3 + 2 H2O

Properties

Rubidium germanium iodide is polymorphic with various distorted perovskite-like structures, reflecting the influence of the "non-bonding" pair of electrons on the centre of Ge2+. [3]

At room temperature, rubidium germanium iodide has a black, cubic perovskite form; between -29 °C and -52 °C a black rhombohedral form; a bordeaux-red orthrhombic perovskite form between -52 °C and -92 °C; and a lemon-yellow orthorhombic form below -92 °C. [4]

Related Research Articles

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<span class="mw-page-title-main">Thallium triiodide</span> Chemical compound

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3.

<span class="mw-page-title-main">Tin(II) iodide</span> Chemical compound

Tin(II) iodide, also known as stannous iodide, is an ionic tin salt of iodine with the formula SnI2. It has a formula weight of 372.519 g/mol. It is a red to red-orange solid. Its melting point is 320 °C, and its boiling point is 714 °C.

Germanium iodides are inorganic compound with the formula GeIx. Two such compounds exist: germanium(II) iodide, GeI2, and germanium(IV) iodide GeI4.

<span class="mw-page-title-main">Bismuth(III) iodide</span> Chemical compound

Bismuth(III) iodide is the inorganic compound with the formula BiI3. This gray-black salt is the product of the reaction of bismuth and iodine, which once was of interest in qualitative inorganic analysis.

<span class="mw-page-title-main">Germanium monoxide</span> Chemical compound

Germanium monoxide (chemical formula GeO) is a chemical compound of germanium and oxygen. It can be prepared as a yellow sublimate at 1000 °C by reacting GeO2 with Ge metal. The yellow sublimate turns brown on heating at 650 °C. GeO is not well characterised. It is amphoteric dissolving in acids to form germanium(II) salts and in alkali to form "trihydroxogermanates" or "germanites" containing the Ge(OH)3− ion.

<span class="mw-page-title-main">Germanium dichloride</span> Chemical compound

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<span class="mw-page-title-main">Germanium tetrafluoride</span> Chemical compound

Germanium tetrafluoride (GeF4) is a chemical compound of germanium and fluorine. It is a colorless gas.

<span class="mw-page-title-main">Germanium nitride</span> Chemical compound

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<span class="mw-page-title-main">Iodite</span> Ion

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<span class="mw-page-title-main">Rhodium(III) iodide</span> Chemical compound

Rhodium(III) iodide is an inorganic compound with the formula RhI3. It is a black solid.

Europium(III) iodide is an inorganic compound containing europium and iodine with the chemical formula EuI3.

Ruthenium(III) iodide is a chemical compound containing ruthenium and iodine with the formula RuI3. It is a black solid.

<span class="mw-page-title-main">Hafnium(III) iodide</span> Chemical compound

Hafnium(III) iodide is an inorganic compound of hafnium and iodine with the formula Hf I3. It is a black solid.

References

  1. ↑ Deepthi Jayan, K.; Sebastian, Varkey (2021-09-01). "Ab initio DFT determination of structural, mechanical, optoelectronic, thermoelectric and thermodynamic properties of RbGeI3 inorganic perovskite for different exchange-correlation functionals". Materials Today Communications. 28: 102650. doi:10.1016/j.mtcomm.2021.102650. ISSN   2352-4928.
  2. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 377. ISBN   978-0-08-037941-8.
  3. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 376. ISBN   978-0-08-037941-8.
  4. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 376–377. ISBN   978-0-08-037941-8.
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