:Cobalt(II) iodide
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| verifiedrevid = 455355332
| ImageFile = Cobalt(II)-iodide-xtal-packing-3D-bs-17.png
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| IUPACName = Cobalt(II) iodide
| OtherNames = cobaltous iodide, cobalt diiodide
|Section1={{Chembox Identifiers
| Abbreviations =
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo1_Ref = {{cascite|correct|CAS}}
| CASNo1 = 15238-00-3
| CASNo1_Comment = (HCl)
| CASNo2_Ref = {{cascite|changed|??}}
| CASNo2 = 52595-03-6
| CASNo2_Comment = (hexahydrate)
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = RTJ1W9DF34
| EINECS = 239-283-2
| PubChem = 419951
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID = 76542
| SMILES = [Co+2].[I-].[I-]
| InChI = 1/Co.2HI/h;2*1H/q+2;;/p-2
| InChIKey = AVWLPUQJODERGA-NUQVWONBAD
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChI = 1S/Co.2HI/h;2*1H/q+2;;/p-2
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = AVWLPUQJODERGA-UHFFFAOYSA-L
| RTECS =
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| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI =
| KEGG_Ref = {{keggcite|correct|kegg}}
| KEGG =
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|Section2={{Chembox Properties
| Formula = CoI2
| MolarMass = 312.7421 g/mol (anhydrous)
420.83 g/mol (hexahydrate)
| Appearance = α-form: black hexagonal crystal
β-form: yellow powder
| Density = α-form: 5.584 g/cm3
β-form: 5.45 g/cm3
hexahydrate: 2.79 g/cm3
| MeltingPt = α-form: 515-520 °C under vacuum
β-form: converts to α-form at 400 °C
| BoilingPtC = 570
{{Citation
| last1 = Perry
| first1 = Dale L.
| author-link =
| last2 = Phillips
| first2 = Sidney L.
| author2-link =
| publication-date =
| year = 1995
| title = Handbook of Inorganic Compounds
| edition =
| volume =
| series =
| location = San Diego
| place =
| publisher = CRC Press
| id =
| isbn = 0-8493-8671-3
| doi =
| oclc =
| pages = 127–8
| url = https://books.google.com/books?id=0fT4wfhF1AsC&q=%22Cobalt(II)+iodide%22&pg=PA128
| access-date = 2008-06-03
}}
| SolubleOther =
| Solvent =
| pKa =
| pKb =
| MagSus = +10,760·10−6 cm3/mol}}
|Section7={{Chembox Hazards
| ExternalSDS =
| GHSPictograms = {{GHS07}}{{GHS08}}
| GHSSignalWord = Warning
| HPhrases = {{H-phrases|302|312|315|319|332|335}}
| PPhrases = {{P-phrases|}}
| MainHazards =
| NFPA-H = 3
| NFPA-F = 0
| NFPA-R = 1
| NFPA-S =
| FlashPt =
| AutoignitionPt =
| ExploLimits =
| PEL = }}
|Section8={{Chembox Related
| OtherAnions = Cobalt(II) fluoride
Cobalt(II) chloride
Cobalt(II) bromide
| OtherCations = Nickel(II) iodide
Copper(I) iodide
}}
}}
Cobalt(II) iodide or cobaltous iodide are the inorganic compounds with the formula CoI2 and the hexahydrate CoI2(H2O)6. These salts are the principal iodides of cobalt.
Synthesis
Cobalt(II) iodide is prepared by treating cobalt powder with gaseous hydrogen iodide. The hydrated form CoI2.6H2O can be prepared by the reaction of cobalt(II) oxide (or related cobalt compounds) with hydroiodic acid.
Cobalt(II) iodide crystallizes in two polymorphs, the α- and β-forms. The α-polymorph consists of black hexagonal crystals, which turn dark green when exposed to air. Under a vacuum at 500 °C, samples of α-CoI2 sublime, yielding the β-polymorph as a yellow crystals. β-CoI2 also readily absorbs moisture from the air, converting into green hydrate. At 400 °C, β-CoI2 reverts to the α-form.O. Glemser "Cobalt, Nickel" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1518.
Structures
The anhydrous salts adopt the cadmium halide structures.
The hexaaquo salt consists of separated [Co(H2O)6]2+ and iodide ions as verified crystallographically.“Structure Cristalline et Expansion Thermique de L’Iodure de Nickel Hexahydrate“ (Crystal structure and thermal expansion of nickel(II) iodide hexahydrate) Louër, Michele; Grandjean, Daniel; Weigel, Dominique Journal of Solid State Chemistry (1973), 7(2), 222-8. {{doi| 10.1016/0022-4596(73)90157-6}}"The crystal structure of the crystalline hydrates of transition metal salts. The structure of CoI2·6H2O" Shchukarev, S. A.; Stroganov, E. V.; Andreev, S. N.; Purvinskii, O. F. Zhurnal Strukturnoi Khimii 1963, vol. 4, pp. 63-6.
Reactions and applications
Anhydrous cobalt(II) iodide is sometimes used to test for the presence of water in various solvents.
{{Citation
| last1 = Armarego
| first1 = Wilfred L. F.
| author-link =
| last2 = Chai
| first2 = Christina L. L.
| author2-link =
| publication-date =
| year = 2003
| title = Purification of Laboratory Chemicals
| edition =
| volume =
| series =
| location =
| place =
| publisher = Butterworth-Heinemann
| id =
| isbn = 0-7506-7571-3
| doi =
| oclc =
| pages = 26
| url = https://books.google.com/books?id=SYzm1tx2z3QC&q=%22Cobalt(II)+iodide%22&pg=PA26
| access-date = 2008-06-03
}}
Cobalt(II) iodide is used as a catalyst, e.g. in carbonylations. It catalyzes the reaction of diketene with Grignard reagents, useful for the synthesis of terpenoids
{{Citation
| last1 = Agreda
| first1 = V. H.
| author-link =
| last2 = Zoeller
| first2 = Joseph R.
| author2-link =
| publication-date =
| year = 1992
| title = Acetic Acid and Its Derivatives
| edition =
| volume =
| series =
| location =
| place =
| publisher = CRC Press
| id =
| isbn = 0-8247-8792-7
| doi =
| oclc =
| pages = 74
| url = https://books.google.com/books?id=3MjdGp1v1YIC&q=%22Cobalt(II)+iodide%22&pg=RA1-PA784
| access-date = 2008-06-03
}}
References
{{Reflist}}
{{Cobalt compounds}}
{{Iodides}}
{{DEFAULTSORT:Cobalt(Ii) Iodide}}