Indium(III) hydroxide
Names
IUPAC name
Indium(III) hydroxide
Other names
Indium hydroxide, indium trihydroxide
Identifiers
3D model (JSmol)
ECHA InfoCard 100.039.937 Edit this at Wikidata
EC Number
  • 243-947-7
UNII
  • InChI=1S/In.3H2O/h;3*1H2/q+3;;;/p-3
    Key: IGUXCTSQIGAGSV-UHFFFAOYSA-K
  • [OH-].[OH-].[OH-].[In+3]
Properties
In(OH)3
Molar mass 165.8404 g/mol
Appearance White solid
Density 4.38 g/cm3
Melting point 150 °C (302 °F; 423 K) (decomposes)
insoluble
1.725
Structure
cubic
Im3
octahedral
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
0
1
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Indium(III) hydroxide is the chemical compound with the formula In(OH)3. Its prime use is as a precursor to indium(III) oxide, In2O3.[1] It is sometimes found as the rare mineral dzhalindite.

Structure

Indium(III) hydroxide has a cubic structure, space group Im3, a distorted ReO3 structure.[2][3]

Preparation and reactions

Neutralizing a solution containing an In3+ salt such as indium nitrate (In(NO3)3) or a solution of indium trichloride (InCl3) gives a white precipitate that on aging forms indium(III) hydroxide.[4][5] A thermal decomposition of freshly prepared In(OH)3 shows the first step is the conversion of In(OH)3·xH2O to cubic indium(III) hydroxide.[4] The precipitation of indium hydroxide was a step in the separation of indium from zincblende ore by Reich and Richter, the discoverers of indium.[6]

Indium(III) hydroxide is amphoteric, like gallium(III) hydroxide (Ga(OH)3) and aluminium hydroxide (Al(OH)3), but is much less acidic than gallium hydroxide (Ga(OH)3),[5] having a lower solubility in alkaline solutions than in acid solutions.[7] It is for all intents and purposes a basic hydroxide.[8]

Dissolving indium(III) hydroxide in strong alkali gives solutions that probably contain either four coordinate [In(OH)4]− or [In(OH)4(H2O)]−.[8]

Reaction with acetic acid or carboxylic acids is likely to give the basic acetate or carboxylate salt, e.g. (CH3COO)2In(OH).[7]

At 10 MPa pressure and 250-400 °C, indium(III) hydroxide converts to indium oxide hydroxide (InO(OH)), which has a distorted rutile structure.[5]

Rapid decompression of samples of indium(III) hydroxide compressed at 34 GPa causes decomposition, yielding some indium metal.[9]

Laser ablation of indium(III) hydroxide gives indium(I) hydroxide (InOH), a bent molecule with an In-O-H angle of around 132° and an In-O bond length of 201.7 pm.[10]

References

  1. ^ Simon Aldridge, Anthony J. Downs (2011). The Group 13 Metals Aluminium, Gallium, Indium and Thallium: Chemical Patterns and Peculiarities. Wiley. ISBN 978-0-470-68191-6.
  2. ^ A Norlund Christensen, N.C. Broch (1967). "Hydrothermal Investigation of the systems In2O3-H2O-Na2O and In2O3-D2O-Na2O. The crystal structure of rhombohedral In2O3 and In(OH)3". Acta Chemica Scandinavica. 21: 1046–1056. doi:10.3891/acta.chem.scand.21-1046.
  3. ^ Wells A.F. (1984). Structural Inorganic Chemistry (5th ed.). Oxford Science Publications. ISBN 0-19-855370-6.
  4. ^ a b Sato, T. (2005). "Preparation and thermal decomposition of indium hydroxide". Journal of Thermal Analysis and Calorimetry. 82 (3): 775–782. doi:10.1007/s10973-005-0963-4. ISSN 1388-6150. S2CID 195329927.
  5. ^ a b c Egon Wiberg, Arnold Frederick Holleman (2001). Inorganic Chemistry. Elsevier. ISBN 0123526515.
  6. ^ Advanced Inorganic Chemistry. Vol. I (31st ed.). Krishna Prakashan Media. 2008. ISBN 9788187224037.
  7. ^ a b George K. Schweitzer, Lester L. Pesterfield (2009). The Aqueous Chemistry of the Elements. Oxford University Press. ISBN 978-0195393354.
  8. ^ a b Anthony John Downs (1993). Chemistry of aluminium, gallium, indium, and thallium. Springer. ISBN 0-7514-0103-X.
  9. ^ Gurlo, Aleksander; Dzivenko, Dmytro; Andrade, Miria; Riedel, Ralf; Lauterbach, Stefan; Kleebe, Hans-Joachim (2010). "Pressure-Induced Decomposition of Indium Hydroxide". Journal of the American Chemical Society. 132 (36): 12674–12678. doi:10.1021/ja104278p. ISSN 0002-7863. PMID 20731389.
  10. ^ Lakin, Nicholas M.; Varberg, Thomas D.; Brown, John M. (1997). "The Detection of Lines in the Microwave Spectrum of Indium Hydroxide, InOH, and Its Isotopomers". Journal of Molecular Spectroscopy. 183 (1): 34–41. Bibcode:1997JMoSp.183...34L. doi:10.1006/jmsp.1996.7237. ISSN 0022-2852.
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