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	{{chembox		{{chembox
			|Watchedfields = changed
	| verifiedrevid = 406007426		|verifiedrevid = 428833766
	| ImageFile = Jodid nikelnatý.PNG		|ImageFile = Jodid nikelnatý.PNG
	| ImageSize =
	| ImageName = Nickel(II) iodide hexahydrate, NiI<sub>2</sub>•6H<sub>2</sub>O		|ImageName = Nickel(II) iodide hexahydrate, NiI<sub>2</sub>•6H<sub>2</sub>O
	| ImageFile1 = Nickel(II)-iodide-xtal-3D-vdW.png		|ImageFile1 = Nickel(II)-iodide-xtal-3D-SF.png
			|ImageName1 = Nickel(II) iodide
	| ImageSize1 =
	| ImageName1 = Nickel(II) iodide		|IUPACName = Nickel(II) iodide
	| IUPACName = Nickel(II) iodide		|OtherNames = Nickelous iodide
		⚫	|Section1={{Chembox Identifiers
	| OtherNames = Nickelous iodide
		⚫	|CASNo_Ref = {{cascite|correct|??}}
⚫	| Section1 = {{Chembox Identifiers
		⚫	|CASNo = 13462-90-3
	| Abbreviations =
			|UNII_Ref = {{fdacite|correct|FDA}}
⚫	| CASNo = 13462-90-3
			|UNII = AQ9OJ30HDD
	| EINECS =
	| PubChem = 26038		|PubChem = 26038
	| SMILES =		|SMILES = (I)I
	| InChI =		|InChI = 1S/2HI.Ni/h2*1H;/q;;+2/p-2
	| RTECS =
	| MeSHName =
	| ChEBI =
⚫	| KEGG_Ref = {{keggcite|correct|kegg}}
	| KEGG =
	| ATCCode_prefix =
	| ATCCode_suffix =
	| ATC_Supplemental =}}
⚫	| Section2 = {{Chembox Properties
⚫	| Ni = 1 | I = 2
⚫	| Appearance = black solid, hydrate is green
⚫	| Density = 5.38 g/cm<sup>3</sup><!--From Aldrich catalogue-->
⚫	| MeltingPtC = 780
	| Melting_notes =
	| BoilingPtC = 797
	| Boiling_notes =
	| Solubility = good
⚫	| SolubleOther = alcohols
	| Solvent =
	| pKa =
	| pKb = }}
⚫	| Section7 = {{Chembox Hazards
	| ExternalMSDS =
	| EUClass =
	| EUIndex =
	| MainHazards =
⚫	| NFPA-H = 2
⚫	| NFPA-F = 0
⚫	| NFPA-R = 0 <!--assuming nickel(II) chloride has same NFPA ratings, took from nickelous chloride article-->
	| NFPA-O =
	| RPhrases =
	| SPhrases =
	| RSPhrases =
	| FlashPt =
	| Autoignition =
	| ExploLimits =
	| PEL = }}
⚫	| Section8 = {{Chembox Related
⚫	| OtherCations = ], ],
⚫	| OtherAnions = ], ], ] }}
	}}		}}
		⚫	|Section2={{Chembox Properties
⚫	'''Nickel(II) iodide''' is an ] with the ] NiI<sub>2</sub>. This paramagnetic black solid dissolves readily in water to give blue-green solutions of the aquo complexes.<ref>{{RubberBible86th}}</ref> This blue-green colour is typical of hydrated nickel(II) compounds. Nickel iodides find some applications in ].
		⚫	|Ni=1 | I=2
		⚫	|Appearance = iron-black solid (anhydrous) <br> bluish-green solid (hexahydrate)
		⚫	|Density = 5.384 g/cm<sup>3</sup>
		⚫	|MeltingPtC = 780
			|MeltingPt_notes = (anhydrous) <br> 43 °C (hexahydrate, loses water)
			|Solubility = 124.2 g/100 mL (0 °C) <br> 188.2 g/100 mL (100 °C)
		⚫	|SolubleOther = alcohols
			|MagSus = +3875.0·10<sup>−6</sup> cm<sup>3</sup>/mol}}
		⚫	|Section7={{Chembox Hazards
		⚫	|NFPA-H = 2
		⚫	|NFPA-F = 0
		⚫	|NFPA-R = 0 <!--assuming nickel(II) chloride has same NFPA ratings, took from nickelous chloride article-->
			}}
		⚫	|Section8={{Chembox Related
		⚫	|OtherCations = ], ],
		⚫	|OtherAnions = ], ], ] }}
			}}
		⚫	'''Nickel(II) iodide''' is an ] with the ] NiI<sub>2</sub>. This paramagnetic black solid dissolves readily in water to give bluish-green solutions,<ref>{{RubberBible86th}}</ref> from which crystallizes the ] I<sub>2</sub> (image above).<ref name=Lou>{{cite journal|title=Structure Cristalline et Expansion Thermique de l'Iodure de Nickel Hexahydrate" (Crystal structure and thermal expansion of nickel(II) iodide hexahydrate)|last1=Louër|first1=Michele|last2=Grandjean|first2=Daniel|last3= Weigel|first3=Dominique|journal=Journal of Solid State Chemistry|year=1973|volume=7|pages=222–8|doi= 10.1016/0022-4596(73)90157-6}}</ref> This bluish-green colour is typical of hydrated nickel(II) compounds. Nickel iodides find some applications in ].
			__TOC__
	==Structure and synthesis==		==Structure and synthesis==
	The anhydrous material crystallizes in the ] motif, featuring octahedral coordination geometry at each Ni(II) center. NiI2 is prepared by ] of the pentahydrate.<ref>Laird G. L. Ward, "Anhydrous Nickel (II) Halides and their Tetrakis(Ethanol) and 1,2-Dimethoxyethane Complexes" Inorganic Syntheses, 1972, Volume 13, Pages: 154–164, 2007. {{DOI|10.1002/9780470132449.ch30}}</ref>		The anhydrous material crystallizes in the ] motif, featuring octahedral coordination geometry at each Ni(II) center. NiI<sub>2</sub> is prepared by ] of the pentahydrate.<ref>{{cite book | last1 = Ward | first1 = Laird G. L. | year = 1972 | title = Anhydrous Nickel (II) Halides and their Tetrakis(Ethanol) and 1,2-Dimethoxyethane Complexes | chapter = Anhydrous Nickel(II) Halides and their Tetrakis(ethanol) and 1,2‐Dimethoxyethane Complexes | series = Inorganic Syntheses | volume = 13 | pages = 154–164 | doi = 10.1002/9780470132449.ch30 | isbn = 9780470132449}}</ref>
	NiI<sub>2</sub> readily hydrates, and the hydrated form can be prepared by dissolution of nickel oxide, hydroxide, or carbonate in ]. The anhydrous form can be produced by treating powdered nickel with iodine.		NiI<sub>2</sub> readily hydrates, and the hydrated form can be prepared by dissolution of nickel oxide, hydroxide, or carbonate in ]. The anhydrous form can be produced by treating powdered nickel with iodine.<ref>{{cite book | last1=Greenwood | first1=N. N. | last2=Earnshaw | first2=Alan | title=Chemie der Elemente | publication-place=Weinheim | date=1990 | isbn=978-3-527-26169-7 | oclc=46170372 | language=de |page=1476}}</ref>
			==Applications in catalysis==
	NiI<sub>2</sub> has found some industrial applications as a ] in ] reactions.<ref name=Bertleff>W. Bertleff, M. Roeper, X. Sava, “Carbonylation” in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH: Weinheim, 2003. DOI: 10.1002/14356007.a05 217.</ref> It is also has niche uses as a reagent in ], especially in conjunction with ].<ref>Shinichi Saito, Nickel(II) Iodide" in Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons, 2008. DOI: 10.1002/047084289X.rn00843. Article Online Posting Date: March 14, 2008.</ref>		NiI<sub>2</sub> has some industrial applications as a ] in ] reactions.<ref name=Bertleff>W. Bertleff, M. Roeper, X. Sava, "Carbonylation" in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH: Weinheim, 2003. {{doi|10.1002/14356007.a05_217}}.</ref> It is also has niche uses as a reagent in ], especially in conjunction with ].<ref>{{cite encyclopedia|author=Shinichi Saito|title=Nickel(II) Iodide|encyclopedia=Encyclopedia of Reagents for Organic Synthesis|publisher=John Wiley & Sons|year=2008|doi=10.1002/047084289X.rn00843|isbn=978-0471936237 }}</ref>
			Like many nickel complexes, those derived from hydrated ] have been used in cross coupling.<ref>{{Cite journal |last1=Everson |first1=Daniel A. |last2=Shrestha |first2=Ruja |last3=Weix |first3=Daniel J. |date=2010-01-27 |title=Nickel-Catalyzed Reductive Cross-Coupling of Aryl Halides with Alkyl Halides |journal=Journal of the American Chemical Society |volume=132 |issue=3 |pages=920–921 |doi=10.1021/ja9093956 |pmid=20047282}}</ref>
			]
	==References==		==References==
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	{{Nickel compounds}}		{{Nickel compounds}}
			{{Iodides}}
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			]
	]		]
	{{inorganic-compound-stub}}
	]
	]
	]
	]
	]