Cadmium acetate
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| Names | |
|---|---|
| IUPAC name Cadmium acetate | |
| Other names Cadmium diacetate | |
| Identifiers | |
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3D model (JSmol) |
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| ChemSpider |
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| ECHA InfoCard | 100.008.049  |
| EC Number |
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PubChem CID |
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| UNII |
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| UN number | 2570 |
CompTox Dashboard (EPA) |
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InChI
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| Properties | |
Chemical formula | Cd(CH3COO)2 (anhydrous) Cd(CH3COO)2·2H2O (dihydrate) |
| Molar mass | 230.500 g/mol (anhydrous) 266.529 g/mol (dihydrate) |
| Appearance | colorless crystals (anhydrous) white crystals (dihydrate) |
| Odor | acetic acid |
| Density | 2.341 g/cm3 (anhydrous) 2.01 g/cm3 (dihydrate) |
| Melting point | 255 °C (491 °F; 528 K) (anhydrous) dihydrate decomposes at 130°C [1] |
Solubility in water | soluble (anhydrous), very soluble (dihydrate) |
| Solubility | soluble in methanol, ethanol (anhydrous) soluble in ethanol (dihydrate) |
| -83.7·10−6 cm3/mol | |
| Structure | |
| monoclinic | |
| Hazards | |
| GHS labelling: | |
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| Warning | |
| H302, H312, H332, H410 | |
| P261, P264, P270, P271, P273, P280, P301+P312, P302+P352, P304+P312, P304+P340, P312, P322, P330, P363, P391, P501 | |
| NFPA 704 (fire diamond) |  3 1 0 |
| NIOSH (US health exposure limits): | |
PEL (Permissible) | [1910.1027] TWA 0.005 mg/m3 (as Cd)[2] |
REL (Recommended) | Ca[2] |
IDLH (Immediate danger) | Ca [9 mg/m3 (as Cd)][2] |
| Related compounds | |
Other anions | Cadmium fluoride Cadmium chloride Cadmium bromide Cadmium iodide |
Other cations | Zinc acetate Mercury(II) acetate Silver acetate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).  N verify (what is  Y N ?) Infobox references | |
Chemical compound
Cadmium acetate is the chemical compound with the formula Cd(O2CCH3)2(H2O)2. The compound is marketed both as the anhydrous form and as a dihydrate, both of which are white or colorless. Only the dihydrate has been verified by X-ray crystallography.
Preparation, reactions, and uses
It forms by treating cadmium oxide with acetic acid:[3][4]
- CdO + 2 CH3CO2H + H2O → Cd(O2CCH3)2(H2O)2
It can also be prepared by treating cadmium nitrate with acetic anhydride.[5]
Cadmium acetate has few applications. By reaction with trioctylphosphine selenide, it has often been used as a precursor to cadmium selenide and related semiconductors.[6]
Structure of the dihydrate
Unlike the coordination geometry of zinc in zinc diacetate dihydrate, cadmium is seven coordinate in Cd(O2CCH3)2(H2O)2.[7] It is a coordination polymer, featuring acetate ligands interconnecting cadmium centers.
Safety
Cadmium compounds are considered Group 1 carcinogens by the IARC.
References
- ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. p. 447. ISBN 0-8493-0594-2.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH).
- ^ Gangolli, S. (1999). The Dictionary of Substances and Their Effects. London: Royal Society of Chemistry. pp. 12–13. ISBN 9780854048137. Retrieved 2009-03-29.
- ^ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill Professional. pp. 143–144. ISBN 0-07-049439-8. Retrieved 2009-03-29.
- ^ F. Wagenknecht; R. Juza (1963). "Cadmium acetate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1105.
- ^ García-Rodríguez, Raúl; Hendricks, Mark P.; Cossairt, Brandi M.; Liu, Haitao; Owen, Jonathan S. (2013). "Conversion Reactions of Cadmium Chalcogenide Nanocrystal Precursors". Chemistry of Materials. 25 (8): 1233–1249. doi:10.1021/cm3035642.
- ^ Harrison, W.; Trotter, J. (1972). "Crystal and molecular structure of cadmium diacetate dihydrate". Journal of the Chemical Society, Dalton Transactions (8–9): 956. doi:10.1039/dt9720000956.
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- Cd2(AlCl4)2
