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) Y
PubChem	18746
ChemSpider	17701 Y
EC number	222-068-2
UN number	3288
RTECS number	QR6200000
Jmol-3D images	Image 1
SMILES [Ni+2].[O-]C([O-])=O
InChI InChI=1S/CH2O3.Ni/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 Y Key: ZULUUIKRFGGGTL-UHFFFAOYSA-L Y InChI=1/CH2O3.Ni/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 Key: ZULUUIKRFGGGTL-NUQVWONBAN
Properties
Molecular formula	NiCO3
Molar mass	118.702 g/mol
Appearance	light green powder
Density	2.6 g/cm3
Melting point	decomposes before melting
Solubility in water	0.093 g/L
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
Y carbonate (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 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 consisting of Ni²⁺ cations. The basic carbonate is an intermediate in the hydrometallurgical purification of nickel from its ores and is used in electroplating of Ni.^[1] Nickel carbonates are used in some ceramic applications and as precursors to catalysts.

Nickel carbonates are hydrolyzed upon contact with by 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 NiO, shown here with anhydrous nickel carbonate:

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⁺ + Na₂CO₃ + 6 OH^- + 4 H₂O → Ni₄CO₃(OH)₆(H₂O)₄ + 2 Na⁺

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

1. ^ 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
2. ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. p. 1557.