Aluminium carbonate
| Names | |
|---|---|
| IUPAC name
Dialuminium Tricarbonate | |
| Identifiers | |
3D model (JSmol) |
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| ChemSpider | |
| ECHA InfoCard | 100.034.930 |
PubChem CID |
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| UNII | |
CompTox Dashboard (EPA) |
|
| |
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| Properties | |
| Al2(CO3)3 | |
| Molar mass | 233.99 g/mol |
| Appearance | white powder, unstable |
| Density | 3.14 g/cm3 |
| reacts | |
| Structure[1] | |
| orthorhombic | |
| Fdd2 | |
a = 21.989 Å, b = 10.176 Å, c = 4.4230 Å | |
Lattice volume (V) |
989.7 |
Formula units (Z) |
8 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Aluminium carbonate (Al2(CO3)3), is a carbonate of aluminium.[2] The neutral carbonate is relatively unknown compared to its related compounds, such as the basic sodium aluminium carbonate mineral dawsonite (NaAlCO3(OH)2) and hydrated basic aluminium carbonate minerals scarbroite (Al5(CO3)(OH)13•5(H2O)) and hydroscarbroite (Al14(CO3)3(OH)36•nH2O).[3][4][5]
Preparation
[edit]For many years there was no evidence for the existence of a simple aluminium carbonate, Al2(CO3)3, as the combination of Al3+ and carbonates are sufficiently alkaline to precipitate aluminium hydroxide and produce carbon dioxide:[6]
![{\displaystyle {2\,[\mathrm {Al} (\mathrm {H} {\vphantom {A}}_{\smash[{t}]{2}}\mathrm {O} ){\vphantom {A}}_{\smash[{t}]{6}}]{\vphantom {A}}^{3+}{\mskip {2mu}}(\mathrm {aq} ){}+{}3\,\mathrm {CO} {\vphantom {A}}_{\smash[{t}]{3}}{\vphantom {A}}^{2-}{\mskip {2mu}}(\mathrm {aq} ){}\mathrel {\longrightarrow } {}2\,\mathrm {Al} (\mathrm {OH} ){\vphantom {A}}_{\smash[{t}]{3}}{\mskip {2mu}}(\mathrm {s} ){}+{}3\,\mathrm {CO} {\vphantom {A}}_{\smash[{t}]{2}}{\mskip {2mu}}(\mathrm {g} ){}+{}9\,\mathrm {H} {\vphantom {A}}_{\smash[{t}]{2}}\mathrm {O} {\mskip {2mu}}(\mathrm {l} )}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/27e6891912209f89743b0ae468dbd3a1d54ce4d3)
However, in 2023, Al2(CO3)3 was produced by heating aluminium oxide at 2300 °C under 24 GPa of carbon dioxide. The resulting solid is stable in air and at room temperature.[7]
Some minerals contain both aluminium and carbonate. Dawsonite has the formula NaAlCO3(OH)2. Hydrotalcites, both synthetic and natural, are layered metal hydroxides comprised in part of aluminium and carbonate.[8]
Surface carbonate species readily form upon exposure of aluminium oxide to CO2.[9]
References
[edit]- ↑ Bayarjargal, Lkhamsuren; Spahr, Dominik; Milman, Victor; Marquardt, Julien; Giordano, Nico; Winkler, Björn (2023). CCDC 2259169: Experimental Crystal Structure Determination (Report). Cambridge Crystallographic Data Centre. doi:10.5517/ccdc.csd.cc2ftvfk.
- ↑ Anthony John Downs, (1993), Chemistry of Aluminium, Gallium, Indium, and Thallium, Springer, ISBN 978-0-7514-0103-5
- ↑ "Scarbroite". www.mindat.org.
- ↑ "Hydroscarbroite". www.mindat.org.
- ↑ "Dawsonite". www.mindat.org. Retrieved 2020-12-14.
- ↑ Moody, Bernard (2013). Comparative Inorganic Chemistry. Elsevier. p. 311. ISBN 9781483280080.
- ↑ Bayarjargal, Lkhamsuren; Spahr, Dominik; Milman, Victor; Marquardt, Julien; Giordano, Nico; Winkler, Björn (28 August 2023). "Anhydrous Aluminum Carbonates and Isostructural Compounds". Inorganic Chemistry. 62 (34): 13910–13918. doi:10.1021/acs.inorgchem.3c01832. PMID 37579301. S2CID 260898136.
- ↑ Costantino, Umberto; Marmottini, Fabio; Nocchetti, Morena; Vivani, Riccardo (1998). "New Synthetic Routes to Hydrotalcite-Like Compounds − Characterisation and Properties of the Obtained Materials". European Journal of Inorganic Chemistry. 1998 (10): 1439–1446. doi:10.1002/(SICI)1099-0682(199810)1998:10<1439::AID-EJIC1439>3.0.CO;2-1.
- ↑ Parkyns, N. D. (1969-01-01). "The surface properties of metal oxides. Part II. An infrared study of the adsorption of carbon dioxide on γ-alumina". Journal of the Chemical Society A: Inorganic, Physical, Theoretical: 410–417. doi:10.1039/J19690000410. ISSN 0022-4944.
