Nickel(II) carbonate
| Nickel(II) carbonate | |
|---|---|
 | |
| IUPAC name Nickel(II) carbonate | |
| Other names Nickelous carbonate | |
| Identifiers | |
| CAS number | (for Ni4CO3(OH)6(H2O)4 29863-10-3) 3333-67-3 (for Ni4CO3(OH)6(H2O)4 29863-10-3)  |
| PubChem | 18746 |
| ChemSpider | 17701 |
| EC number | 222-068-2 |
| UN number | 3288 |
| RTECS number | QR6200000 |
| Jmol-3D images | {{#if:[Ni+2].[O-]C([O-])=O|Image 1 |
| |
| |
| Properties | |
| Molecular formula | NiCO3 |
| Molar mass | 118.702 g/mol |
| Appearance | light green powder |
| Density | 4.39 g/cm3 |
| Melting point | decomposes before melting |
| Solubility in water | 0.0093 g/100 mL |
| Structure | |
| Crystal structure | rhombohedral |
| Hazards | |
| MSDS | ICSC 0927 |
| EU Index | 028-010-00-0 |
| EU classification | Carc. Cat. 1 Muta. Cat. 3 Repr. Cat. 2 Toxic (T) Harmful (Xn) Irritant (Xi) Dangerous for the environment (N) |
| R-phrases | R49, R61, R20/22, R38, R42/43, R48/23, R68, R50/53 |
| S-phrases | S53, S45, S60, S61 |
| NFPA 704 |
 0
2
0
|
| LD50 | 840 mg/kg |
(verify) (what is: / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
| Infobox references | |
Nickel(II) carbonate describes one or a mixture of inorganic compounds containing nickel and carbonate. From the industrial perspective, the most important nickel carbonate is basic nickel carbonate with the formula Ni4CO3(OH)6(H2O)4. Simpler carbonates, ones more likely encountered in the laboratory, are NiCO3 and its hexahydrate. All are paramagnetic green solid containing Ni2+ cations. The basic carbonate is an intermediate in the hydrometallurgical purification of nickel from its ores and is used in electroplating of nickel.[1] Nickel carbonates are used in some ceramic applications and as precursors to catalysts.
Nickel carbonates are hydrolyzed upon contact with aqueous acids to give solutions containing the ion [Ni(H2O)6]2+, liberating water and carbon dioxide in the process. Calcining (heating to drive off CO2 and water) of these carbonates gives nickel oxide:
- NiCO3 → NiO + CO2
The nature of the resulting oxide depends on the nature of the precursor. The oxide obtained from the basic carbonate is often most useful for catalysis.
Basic nickel carbonate can be made by treating solutions of nickel sulfate with sodium carbonate, shown here for the basic carbonate:
- 4 Ni2+ + CO32- + 6 OH- + 4 H2O → Ni4CO3(OH)6(H2O)4
The hydrated carbonate has been prepared by electrolytic oxidation of nickel in the presence of carbon dioxide:[2]
- Ni + O + CO2 + 6 H2O → NiCO3(H2O)4
References
- ↑ Keith Lascelles, Lindsay G. Morgan, David Nicholls, Detmar Beyersmann, "Nickel Compounds" in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a17_235.pub2
- ↑ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. p. 1557.
| |||||||||||