Nickel(II) carbonate

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Nickel(II) carbonate
Nickel(II) carbonate
Names
IUPAC name
Nickel(II) carbonate
Other names
Nickelous carbonate
Identifiers
3333-67-3 N
29863-10-3 (Ni4CO3(OH)6(H2O)4) N
ChemSpider 17701 YesY
EC Number 222-068-2
Jmol 3D model Interactive image
PubChem 18746
RTECS number QR6200000
UN number 3288
  • InChI=1S/CH2O3.Ni/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 YesY
    Key: ZULUUIKRFGGGTL-UHFFFAOYSA-L YesY
  • InChI=1/CH2O3.Ni/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
    Key: ZULUUIKRFGGGTL-NUQVWONBAN
  • [Ni+2].[O-]C([O-])=O
Properties
NiCO3
Appearance light green powder
Density 4.39 g/cm3
Melting point 205 °C (401 °F; 478 K)
decomposes[1]
0.0093 g/100ml
6.6·10−9
Structure
rhombohedral
Vapor pressure {{{value}}}
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
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.[2]

Reactions

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:[3]

Ni + O + CO2 + 6 H2O → NiCO3(H2O)4

Uses

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

Safety

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

References

  1. ↑ https://www.conncoll.edu/media/website-media/offices/ehs/envhealthdocs/Nickel_Carbonate.pdf
  2. ↑ 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
  3. ↑ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. p. 1557.
Carbonates
H2CO3 He
Li2CO3 BeCO3 B C (NH4)2CO3,
NH4HCO3		 O F Ne
Na2CO3,
NaHCO3,
Na3H(CO3)2		 MgCO3,
Mg(HCO3)2		 Al2(CO3)3 Si P S Cl Ar
K2CO3,
KHCO3		 CaCO3,
Ca(HCO3)2		 Sc Ti V Cr MnCO3 FeCO3 CoCO3 NiCO3 CuCO3 ZnCO3 Ga Ge As Se Br Kr
Rb2CO3 SrCO3 Y Zr Nb Mo Tc Ru Rh Pd Ag2CO3 CdCO3 In Sn Sb Te I Xe
Cs2CO3,
CsHCO3		 BaCO3   Hf Ta W Re Os Ir Pt Au Hg Tl2CO3 PbCO3 (BiO)2CO3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
↓
La2(CO3)3 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2CO3 Np Pu Am Cm Bk Cf Es Fm Md No Lr
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