Nickel(II) nitrate
{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 442344977
| Name = Nickel(II) nitrate
| ImageFile = Ni(NO3)2 hexahydrate edit.jpg
| ImageSize =
| ImageName = Nickel(II) nitrate
| ImageCaption = Hexahydrate
| ImageFile1 = Cis-Niaaq4(NO3)2.svg
| ImageSize1 =
| ImageName1 = Nickel(II) nitrate
| IUPACName = Nickel(II) nitrate
| OtherNames = Nickel nitrate
Nickelous nitrate
Nitric acid, nickel(2+) salt
|Section1={{Chembox Identifiers
| CASNo = 13138-45-9
| CASNo_Comment = anhydrous
| CASNo1 = 13478-00-7
| CASNo1_Comment = hexahydrate
| CASNo2 = 72937-94-1
| CASNo2_Comment = tetrahydrate (rare)
| CASNo3 = 16456-84-1
| CASNo3_Comment = 2nd tetrahydrate (also rare)
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 23976
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 50L0S38I2D
| UNII2_Ref = {{fdacite|correct|FDA}}
| UNII2 = XBT61WLT1J
| PubChem = 25736
| EINECS = 238-076-4
| UNNumber = 2725
| InChI = 1/2NO3.Ni/c2*2-1(3)4;/q2*-1;+2
| InChIKey = KBJMLQFLOWQJNF-UHFFFAOYAP
| SMILES = [Ni+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/2NO3.Ni/c2*2-1(3)4;/q2*-1;+2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = KBJMLQFLOWQJNF-UHFFFAOYSA-N
}}
|Section2={{Chembox Properties
| Formula = Ni(NO3)2
| MolarMass = 182.703 g/mol (anhydrous)
290.79 g/mol (hexahydrate)
| Appearance = emerald green hygroscopic solid
| Odor = odorless
| Density = 2.05 g/cm3 (hexahydrate)
| Solubility = 243 (hexahydrate) g/100ml (0 °C)Perry's Chem Eng Handbook, 7th Ed
| SolubleOther = soluble in ethanol
| MeltingPtC = 56.7
| MeltingPt_notes = (hexahydrate)
| BoilingPtC = 120-145
| BoilingPt_notes = (hexahydrate, decomposes to basic nickel nitrate){{cite book| last = Pietsch| first = E. H. E.| title = Gmelins Handbuch der Anorganischen Chemie, Nickel Teil B 2| publisher = Verlag Chemie GmbH| edition = 8th| date = 1966| location = Weinheim/Bergstr.| pages = 509| language = German}}
| RefractIndex = 1.422 (hexahydrate)
| MagSus = +4300.0·10−6 cm3/mol (+6 H2O)
}}
|Section3={{Chembox Structure
| Coordination =
| CrystalStruct = monoclinic (hexahydrate)
| Dipole =
}}
|Section7={{Chembox Hazards
| ExternalSDS = [http://hazard.com/msds/mf/baker/baker/files/n3030.htm External MSDS]
| GHSPictograms = {{GHS03}}{{GHS05}}{{GHS07}}{{GHS08}}{{GHS09}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|272|302|315|317|318|332|334|341|350|360|372|410}}
| PPhrases = {{P-phrases|201|202|210|220|221|260|261|264|270|271|272|273|280|281|285|301+312|302+352|304+312|304+340|304+341|305+351+338|308+313|310|312|314|321|330|332+313|333+313|342+311|362|363|370+378|391|405|501}}
| NFPA-H = 2
| NFPA-R = 0
| NFPA-F = 0
| NFPA-S = OX
| FlashPt = Non-flammable
| LD50 = 1620 mg/kg (oral, rat)
}}
|Section8={{Chembox Related
| OtherAnions = Nickel(II) sulfate
Nickel(II) chloride
| OtherCations = Palladium(II) nitrate
| OtherCompounds = Cobalt(II) nitrate
Copper(II) nitrate
}}
}}
Nickel (II) nitrate is the inorganic compound Ni(NO3)2 or any hydrate thereof. In the hexahydrate, the nitrate anions are not bonded to nickel. Other hydrates have also been reported: Ni(NO3)2.9H2O, Ni(NO3)2.4H2O, and Ni(NO3)2.2H2O.{{Ullmann|doi=10.1002/14356007.a17_235.pub2|title=Nickel Compounds|year=2005|last1=Lascelles|first1=Keith|last2=Morgan|first2=Lindsay G.|last3=Nicholls|first3=David|last4=Beyersmann|first4=Detmar|isbn=3527306730}}
It is prepared by the reaction of nickel oxide with nitric acid:
: NiO + 2 HNO3 + 5 H2O → Ni(NO3)2.6H2O
The anhydrous nickel nitrate is typically not prepared by heating the hydrates. Rather it is generated by the reaction of hydrates with dinitrogen pentoxide or of nickel carbonyl with dinitrogen tetroxide:
: Ni(CO)4 + 2 N2O4 → Ni(NO3)2 + 2 NO + 4 CO
The hydrated nitrate is often used as a precursor to supported nickel catalysts.
Structure
Nickel(II) compounds with oxygenated ligands often feature octahedral coordination geometry. Two polymorphs of the tetrahydrate Ni(NO3)2.4H2O have been crystallized. In one the monodentate nitrate ligands are trans{{cite journal |doi=10.1107/S0567740879010827|title=Crystal Structure of the β Form of Ni(NO3)2.4H2O|year=1979|last1=Morosin|first1=B.|last2=Haseda|first2=T.|journal=Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry|volume=35|issue=12|pages=2856–2858}} while in the other they are cis.{{cite journal |doi=10.1107/S0365110X67001392|title=Structure du Nitrate de Nickel Tétrahydraté|year=1967|last1=Gallezot|first1=P.|last2=Weigel|first2=D.|last3=Prettre|first3=M.|journal=Acta Crystallographica|volume=22|issue=5|pages=699–705|doi-access=free|bibcode=1967AcCry..22..699G }}
Reactions and uses
Nickel(II) nitrate is primarily used in electrotyping and electroplating of metallic nickel.
In heterogeneous catalysis, nickel(II) nitrate is used to impregnate alumina. Pyrolysis of the resulting material gives forms of Raney nickel and Urushibara nickel.{{cite book |doi=10.1002/047084289X.rn011.pub2 |chapter=Nickel Catalysts (Heterogeneous) |title=Encyclopedia of Reagents for Organic Synthesis |date=2014 |last1=Sarko |first1=Christopher R. |last2=Dimare |first2=Marcello |last3=Yus |first3=Miguel |last4=Alonso |first4=Francisco |pages=1–8 |isbn=978-0-470-84289-8 }} In homogeneous catalysis, the hexahydrate is a precatalyst for cross coupling reactions.{{cite book |doi=10.1002/047084289X.rn02013 |chapter=Nickel(II) Nitrate Hexahydrate |title=Encyclopedia of Reagents for Organic Synthesis |date=2017 |last1=Xiao |first1=Yu-Lan |last2=Zhang |first2=Xingang |pages=1–3 |isbn=978-0-470-84289-8 }}