Nickel(II) carbonate

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 solids 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.[3]

Nickel(II) carbonate

Names
IUPAC name Nickel(II) carbonate
Other names Nickelous carbonate
Identifiers
CAS Number	3333-67-3^N 29863-10-3 (Ni4CO3(OH)6(H2O)4)^N
3D model (JSmol)	Interactive image
ChemSpider	17701^Y
ECHA InfoCard	100.020.063
EC Number	222-068-2
PubChem CID	18746
RTECS number	QR6200000
UN number	3288
CompTox Dashboard (EPA)	DTXSID3025708
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
SMILES [Ni+2].[O-]C([O-])=O
Properties
Chemical formula	NiCO3
Molar mass	118.7
Appearance	light green powder
Density	4.39 g/cm^3
Melting point	205 °C (401 °F; 478 K) decomposes[1]
Solubility in water	0.0093 g/100ml
Solubility product (Ksp)	6.6·10^−9
Structure
Crystal structure	rhombohedral
Hazards
Safety data sheet	ICSC 0927
GHS pictograms	[2]
GHS Signal word	Danger
GHS hazard statements	H302, H312, H332, H315, H317, H319, H334, H335, H350[2]
GHS precautionary statements	P201, P261, P280, P305+351+338, P308+313[2]
NFPA 704 (fire diamond)	0 2 0
Lethal dose or concentration (LD, LC):
LD50 (median dose)	840 mg/kg
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is ^YN ?)
Infobox references

Structure and reactions

NiCO₃ adopts a structure like calcite, consisting of nickel in an octahedral coordination geometry.[4]

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:

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:[5]

Ni + O + CO₂ + 6 H₂O → NiCO₃(H₂O)₄

Uses

Nickel carbonates are used in some ceramic applications and as precursors to catalysts.

Natural occurrence

The natural nickel carbonate is known as gaspéite - a rare mineral. Basic Ni carbonates also have some natural representatives.[6]

Safety

It is moderately toxic and causes low irritation. Avoid prolonged contact.

References

1. https://www.conncoll.edu/media/website-media/offices/ehs/envhealthdocs/Nickel_Carbonate.pdf
2. Sigma-Aldrich Co., Nickel(II) carbonate hydroxide tetrahydrate. Retrieved on 2014-05-06.
3. 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
4. Pertlik, F. (1986). "Structures of hydrothermally synthesized cobalt(II) carbonate and nickel(II) carbonate". Acta Crystallographica Section C. 42: 4–5. doi:10.1107/S0108270186097524.
5. Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. p. 1557.
6. https://www.mindat.org/min-1657.html