“Nickel(II) carbonate”的意思、由来-开放百科全书

词条

Nickel(II) carbonate

释义

Structure and reactions
Uses
Natural occurrence
Safety
References

{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 476999002
| Name = Nickel(II) carbonate
| ImageFile1 = Nickel carbonate basic.jpg
| ImageSize1 =
| ImageName1 = Nickel(II) carbonate
| ImageFile2 = Calcium-carbonate-xtal-3D-SF.png
| IUPACName = Nickel(II) carbonate
| OtherNames = Nickelous carbonate
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 17701
| InChI = 1/CH2O3.Ni/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
| InChIKey = ZULUUIKRFGGGTL-NUQVWONBAN
| SMILES = [Ni+2].[O-]C([O-])=O
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/CH2O3.Ni/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = ZULUUIKRFGGGTL-UHFFFAOYSA-L
| CASNo = 3333-67-3
| CASNo_Ref = {{cascite|changed|??}}
| CASNo2_Ref = {{cascite|changed|??}}
| CASNo2 = 29863-10-3
| CASNo2_Comment = (Ni₄CO₃(OH)₆(H₂O)₄)
| PubChem = 18746
| EINECS = 222-068-2
| UNNumber = 3288
| RTECS = QR6200000
|Section2={{Chembox Properties
| Formula = NiCO₃
| MolarMass = 118.7
| Appearance = light green powder
| Density = 4.39 g/cm³
| MeltingPtC = 205
| MeltingPt_notes =
decomposes^[1]
| Solubility = 0.0093 g/100ml
| SolubilityProduct = 6.6·10⁻⁹
|Section3={{Chembox Structure
| CrystalStruct = rhombohedral
|Section7={{Chembox Hazards
| ExternalSDS = ICSC 0927
| GHSPictograms = {{GHS07}}{{GHS08}}^[2]
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|302|312|332|315|317|319|334|335|350}}^[2]
| PPhrases = {{P-phrases|201|261|280|305+351+338|308+313}}^[2]
| NFPA-H = 2
| NFPA-R = 0
| NFPA-F = 0
| LD50 = 840 mg/kg
|Section8={{Chembox Related
| OtherAnions =
| OtherCations =
| OtherCompounds =
}}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]

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, 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:^[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. ^¹²{{Sigma-Aldrich|id=339776|name=Nickel(II) carbonate hydroxide tetrahydrate|accessdate=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. ^{{cite journal|title=Structures of hydrothermally synthesized cobalt(II) carbonate and nickel(II) carbonate|author=Pertlik, F.|journal=Acta Crystallographica Section C|year=1986|volume=42|pages=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

3 : Carbonates|Nickel compounds|IARC Group 1 carcinogens

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