Zinc carbonate

Zinc carbonate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.020.435 Edit this at Wikidata
EC Number
  • 222-477-6
  • basic: 226-076-7
UNII
UN number 9157
  • InChI=1S/CH2O3.Zn/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
    Key: FMRLDPWIRHBCCC-UHFFFAOYSA-L
  • C(=O)([O-])[O-].[Zn+2]
Properties
ZnCO3
Molar mass 125.4
Appearance white solid
Density 4.434 g/cm3[1]
Melting point 140 °C (284 °F; 413 K)[1] (decomposes)
0.91 mg/L[1]
1.46×10−10[2]
-34×10−6 cm3/mol[3]
n1=1.621, n2=1.848[4]
Structure[5]
Calcite, hR30, No. 167
R3c
a = 4.6528 Å, c = 15.025 Å
6
Hazards
GHS labelling:
GHS09: Environmental hazard
Warning
H319, H410, H411
P264, P273, P280, P302+P352, P305+P351+P338, P321, P332+P313, P337+P313, P362, P391, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Zinc carbonate is the inorganic compound with the formula ZnCO3. It is a white solid that is insoluble in water. It exists in nature as the mineral smithsonite. It is prepared by treating cold solutions of zinc sulfate with potassium bicarbonate. Upon warming, it converts to basic zinc carbonate (Zn5(CO3)2(OH)6).[6]

Zinc carbonate adopts the same structure as calcium carbonate (calcite).[7] Zinc is octahedral and each carbonate is bonded to six Zn centers such that oxygen atoms are three-coordinate.

  1. ^ a b c Haynes, p. 4.95
  2. ^ Haynes, p. 5.178
  3. ^ Haynes, p. 4.131
  4. ^ Haynes, p. 4.137
  5. ^ Haynes, p. 4.144
  6. ^ Wagenknecht, F.; Juza, R. (1963). "Zinc carbonate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1086.
  7. ^ Effenberger, H.; Mereiter, K.; Zemann, J. (1981). "Crystal structure refinements of magnesite, calcite, rhodochrosite, siderite, smithonite, and dolomite, with discussion of some aspects of the stereochemistry of calcite type carbonates". Zeitschrift für Kristallographie - Crystalline Materials. 156 (3–4): 233–243. Bibcode:1981ZK....156..233E. doi:10.1524/zkri.1981.156.3-4.233.