cobalt(II) perchlorate
{{Chembox
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| Name =
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| PIN =
| SystematicName = Cobalt(II) diperchlorate
| OtherNames = {{Unbulleted list
| Cobaltous perchlorate
| Cobalt diperchlorate
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| ImageFile = Cobalt perchlorate hexahydrate.jpg
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| ImageCaption = Hexahydrate
| Section1 = {{Chembox Identifiers
| index1_label = hexahydrate
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| CASNo = 13455-31-7
| ChEBI =
| ChemSpiderID = 24278
| EINECS =
| EC_number = 236-653-5
| Gmelin =
| StdInChI = 1S/2ClHO4.Co/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2
| StdInChIKey = BSUSEPIPTZNHMN-UHFFFAOYSA-L
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| MeSHName =
| PubChem = 26064
| RTECS =
| InChI1=1S/2ClHO4.Co.6H2O/c2*2-1(3,4)5;;;;;;;/h2*(H,2,3,4,5);;6*1H2/q;;+2;;;;;;/p-2
| InChIKey1=KPOBHNYTWJSVKF-UHFFFAOYSA-
| SMILES = [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Co+2]
| SMILES1 = [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Co+2].O.O.O.O.O.O
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| Section2 = {{Chembox Properties
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| Appearance = Pink solid (anhydrous)
Dark-red crystals (hexahydrate)
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| Density = 3.33 g/cm3
| Formula = Co(ClO4)2
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| MolarMass = 257.83 g/mol
| MeltingPt =
| MeltingPtC = 170
| MeltingPt_notes= (decomposition, hexahydrate)
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| Solubility = 113 g/100 mL (25 °C)
| SolubleOther = Insoluble in ethanol and acetone
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| Section3 = {{Chembox Structure
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| Section7 = {{Chembox Hazards
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| NFPA-H = 2
| NFPA-F = 0
| NFPA-I = 1
| NFPA-S = OX
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| ExternalSDS = [https://www.fishersci.com/store/msds?partNumber=AA4432009&productDescription=CBLT+II+PERCHLRAT+H+99.999+10G&vendorId=VN00024248&countryCode=US&language=en Fisher SDS]
| GHSPictograms = {{GHS03}}{{GHS07}}{{GHS08}}
| GHSSignalWord = Danger
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| Section9 = {{Chembox Related
| OtherAnions =
| OtherCations = Iron(II) perchlorate
Nickel(II) perchlorate
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Cobalt(II) perchlorate is an inorganic chemical compound with the formula Co(ClO4)2·nH2O (n = 0,6). The pink anhydrous and red hexahydrate forms are both hygroscopic solids.
Preparation and reactions
Cobalt(II) perchlorate hexahydrate is produced by reacting cobalt metal or cobalt(II) carbonate with perchloric acid, followed by the evaporation of the solution:
:CoCO3 + 2 HClO4 → Co(ClO4)2 + H2O + CO2
The anhydrous form cannot be produced from the hexahydrate by heating, as it instead decomposes to cobalt(II,III) oxide at 170 °C. Instead, anhydrous cobalt(II) perchlorate is produced from the reaction of dichlorine hexoxide and cobalt(II) chloride, followed by heating in a vacuum at 75 °C.{{cite journal |author1=Jean-Louis Pascal |author2=Jacqueline Potier |author3=Cheng Shan Zhang |title=Chlorine trioxide, Cl2O6, a most efficient perchlorating reagent in new syntheses of anhydrous metal perchlorates, chloryl and nitryl perchloratometalates of cobalt(II), nickel(II), and copper(II). Reactivity of chlorine trioxide with anhydrous or hydrated chlorides and nitrates |journal=Journal of the Chemical Society, Dalton Transactions |date=1985 |volume=2 |issue=2 |pages=297–305 |doi=10.1039/DT9850000297 |language=en}}
Structure
The anhydrous form consists of octahedral Co(ClO4)6 centers, with tridentate perchlorate ligands.{{cite journal |author1=J. L. Pascal |author2=J. Potier |author3=D. J. Jones |author4=J. Roziere |author5=A. Michalowicz |title=Structural approach to the behavior of perchlorate as a ligand in transition-metal complexes using EXAFS, IR, and Raman spectroscopy. 2. Crystal structure of M(ClO4)2 (M = Co, Ni). A novel mode of perchlorate coordination |journal=Inorganic Chemistry |date=1985 |volume=24 |issue=2 |pages=238–241 |doi=10.1021/ic00196a026 |language=en}} On the other hand, the orthorhombic hexahydrate consists of isolated [Co(H2O)6]2+ octahedrons and perchlorate anions with lattice constants a = 7.76 Å, b = 13.44 Å and c = 5.20 Å. The hexahydrate undergoes phase transitions at low temperatures.{{cite journal |author1=M.B. Patel |author2=Sushama Patel |author3=D.P. Khandelwal |author4=H.D. Bist |title=Vibrational studies and phase transitions in Co(ClO4)2·6H2O and Mn(ClO4)2·6H2O |journal=Chemical Physics Letters |date=1983 |volume=101 |issue=1 |pages=93–99 |doi=10.1016/0009-2614(83)80311-X |language=en}}{{cite journal |author1=A. K. Jain |author2=G. C. Upreti |title=On the anomalous paramagnetism of Co(II) perchlorate hexahydrate at low temperatures |journal=Journal of Physics C: Solid State Physics |date=1975 |volume=8 |issue=12 |pages=1884–1888 |doi=10.1088/0022-3719/8/12/013 |bibcode=1975JPhC....8.1884C |language=en}}
References
{{reflist}}
{{Cobalt compounds}}
{{Perchlorates}}