Chemistry:Cadmium acetate
From HandWiki
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| Names | |
|---|---|
| IUPAC name
Cadmium acetate
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| Other names
Cadmium diacetate
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| EC Number |
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PubChem CID
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| RTECS number |
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| UNII |
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| UN number | 2570 |
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| Properties | |
| 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] |
| 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 pictograms |   
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| GHS Signal word | Warning |
| H302, H312, H332, H410 | |
| P261, P264, P270, P271, P273, P280, P301+312, P302+352, P304+312, P304+340, P312, P322, P330, P363, P391, P501 | |
| NFPA 704 (fire diamond) | |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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[1910.1027] TWA 0.005 mg/m3 (as Cd)[2] |
REL (Recommended)
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Ca[2] |
IDLH (Immediate danger)
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Ca [9 mg/m3 (as Cd)][2] |
| Related compounds | |
Other anions
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Cadmium fluoride Cadmium chloride Cadmium bromide Cadmium iodide |
Other cations
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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). | |
 verify (what is   ?)
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| Infobox references | |
Cadmium acetate is the chemical compound with the formula Cd(O
2CCH
3)
2(H
2O)
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 CH
3CO
2H + H
2O → Cd(O
2CCH
3)
2(H
2O)
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(O
2CCH
3)
2(H
2O)
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. pp. 447. ISBN 0-8493-0594-2.
- ↑ 2.0 2.1 2.2 NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0087.html.
- ↑ Gangolli, S. (1999). The Dictionary of Substances and Their Effects. London: Royal Society of Chemistry. pp. 12–13. ISBN 9780854048137. https://books.google.com/books?id=s4YittJrOsAC&dq=%22Cadmium+acetate%22&pg=PA12. Retrieved 2009-03-29.
- ↑ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill Professional. pp. 143–144. ISBN 0-07-049439-8. https://books.google.com/books?id=Xqj-TTzkvTEC&dq=%22Cobalt+hydroxide%22+OR+%22Cobalt(II)+hydroxide%22&pg=PA243. Retrieved 2009-03-29.
- ↑ F. Wagenknecht; R. Juza (1963). "Cadmium acetate". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 2. NY, NY: Academic Press. pp. 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.
Acetyl halides and salts of the acetate ion
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|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| AcOH | He | ||||||||||||||||||
| LiOAc | Be(OAc)2 BeAcOH |
B(OAc)3 | AcOAc ROAc |
NH4OAc | AcOOH | FAc | Ne | ||||||||||||
| NaOAc | Mg(OAc)2 | Al(OAc)3 ALSOL Al(OAc)2OH Al2SO4(OAc)4 |
Si | P | S | ClAc | Ar | ||||||||||||
| KOAc | Ca(OAc)2 | Sc(OAc)3 | Ti(OAc)4 | VO(OAc)3 | Cr(OAc)2 Cr(OAc)3 |
Mn(OAc)2 Mn(OAc)3 |
Fe(OAc)2 Fe(OAc)3 |
Co(OAc)2, Co(OAc)3 |
Ni(OAc)2 | Cu(OAc)2 | Zn(OAc)2 | Ga(OAc)3 | Ge | As(OAc)3 | Se | BrAc | Kr | ||
| RbOAc | Sr(OAc)2 | Y(OAc)3 | Zr(OAc)4 | Nb | Mo(OAc)2 | Tc | Ru(OAc)2 Ru(OAc)3 Ru(OAc)4 |
Rh2(OAc)4 | Pd(OAc)2 | AgOAc | Cd(OAc)2 | In | Sn(OAc)2 Sn(OAc)4 |
Sb(OAc)3 | Te | IAc | Xe | ||
| CsOAc | Ba(OAc)2 | Hf | Ta | W | Re | Os | Ir | Pt(OAc)2 | Au | Hg2(OAc)2, Hg(OAc)2 |
TlOAc Tl(OAc)3 |
Pb(OAc)2 Pb(OAc)4 |
Bi(OAc)3 | Po | At | Rn | |||
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La(OAc)3 | Ce(OAc)x | Pr | Nd | Pm | Sm(OAc)3 | Eu(OAc)3 | Gd(OAc)3 | Tb | Dy(OAc)3 | Ho(OAc)3 | Er | Tm | Yb(OAc)3 | Lu(OAc)3 | |||||
| Ac | Th | Pa | UO2(OAc)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
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