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{{chembox {{chembox
| Verifiedfields = changed
⚫ | verifiedrevid = 402505919
| Watchedfields = changed
⚫ | verifiedrevid = 442344977
| Name = Nickel(II) nitrate | Name = Nickel(II) nitrate
| ImageFile = Nickel nitrate.png | ImageFile = Cis-Niaaq4(NO3)2.svg
| ImageSize = 200px | ImageSize =
| ImageName = Nickel(II) nitrate | ImageName = Nickel(II) nitrate
| ImageFile2 = Nickel(II) nitrate.jpg | ImageFile2 = Ni(NO3)2 hexahydrate edit.jpg
| ImageSize2 = 200px | ImageSize2 =
| ImageName2 = Nickel(II) nitrate | ImageName2 = Nickel(II) nitrate
| ImageCaption2 = Hexahydrate
| IUPACName = Nickel(II) nitrate | IUPACName = Nickel(II) nitrate
| OtherNames = Nickel nitrate<br/>Nickelous nitrate<br/>Nitric acid, nickel(2+) salt | OtherNames = Nickel nitrate<br/>Nickelous nitrate<br/>Nitric acid, nickel(2+) salt
| Section1 = {{Chembox Identifiers |Section1={{Chembox Identifiers
⚫ | CASNo = 13138-45-9
⚫ | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| 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 | 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 | InChI = 1/2NO3.Ni/c2*2-1(3)4;/q2*-1;+2
| InChIKey = KBJMLQFLOWQJNF-UHFFFAOYAP | InChIKey = KBJMLQFLOWQJNF-UHFFFAOYAP
Line 20: Line 38:
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = KBJMLQFLOWQJNF-UHFFFAOYSA-N | StdInChIKey = KBJMLQFLOWQJNF-UHFFFAOYSA-N
⚫ | CASNo = 13138-45-9
⚫ | CASNo_Ref = {{cascite|correct|CAS}}
| CASOther = <br/>13478-00-7 (hexahydrate) <!-- also 14216-75-2 for "nitric acid, nickel salt" -->
⚫ | PubChem = 25736
⚫ | EINECS = 238-076-4
}} }}
| Section2 = {{Chembox Properties |Section2={{Chembox Properties
| Formula = Ni(NO<sub>3</sub>)<sub>2</sub> | Formula = Ni(NO<sub>3</sub>)<sub>2</sub>
| MolarMass = 182.703 g/mol (anhydrous)<br/>290.79 g/mol (hexahydrate) | MolarMass = 182.703 g/mol (anhydrous)<br/>290.79 g/mol (hexahydrate)
| Appearance = emerald green ] solid | Appearance = emerald green ] solid
| Density = 2.05 g/cm<sup>3</sup> (hexahydrate) | Odor = odorless
| Density = 2.05 g/cm<sup>3</sup> (hexahydrate)
| Solubility = 94.2 g/100ml (20°C)<br/>158 g/100ml (60°C) | Solubility = 243 (hexahydrate) g/100ml (0&nbsp;°C)<ref>Perry's Chem Eng Handbook, 7th Ed</ref>
| SolubleOther = soluble in ] | SolubleOther = soluble in ]
| MeltingPt = 56.7 °C (hexahdyrate) | MeltingPtC = 56.7
| BoilingPt = 136.7 °C (hexahydrate) | MeltingPt_notes = (hexahydrate)
| BoilingPtC = 120-145
| BoilingPt_notes = (hexahydrate, decomposes to basic nickel nitrate)<ref>{{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}}</ref>
| RefractIndex = 1.422 (hexahydrate)
| MagSus = +4300.0·10<sup>−6</sup> cm<sup>3</sup>/mol (+6 H<sub>2</sub>O)
}} }}
| Section3 = {{Chembox Structure |Section3={{Chembox Structure
| Coordination = | Coordination =
| CrystalStruct = monoclinic (hexahydrate) | CrystalStruct = monoclinic (hexahydrate)
| Dipole = | Dipole =
}} }}
| Section7 = {{Chembox Hazards |Section7={{Chembox Hazards
| ExternalMSDS = | ExternalSDS =
| GHSPictograms = {{GHS03}}{{GHS05}}{{GHS07}}{{GHS08}}{{GHS09}}
| EUIndex = 028-012-00-1
| GHSSignalWord = Danger
| EUClass = Oxidant ('''O''')<br/>]<br/>]<br/>Repr. Cat. 2<br/>Toxic ('''T''')<br/>Harmful ('''Xn''')<br/>Irritant ('''Xi''')<br/>Dangerous for the environment ('''N''')
| HPhrases = {{H-phrases|272|302|315|317|318|332|334|341|350|360|372|410}}
| RPhrases = {{R49}}, {{R61}}, {{R8}}, {{R20/22}}, {{R38}}, {{R41}}, {{R42/43}}, {{R48/23}}, {{R68}}, {{R50/53}}
| 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}}
| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}}
| NFPA-H = 2 | NFPA-H = 2
| NFPA-R = 0 | NFPA-R = 0
| NFPA-F = 0 | NFPA-F = 0
| NFPA-O = OX | NFPA-S = OX
| FlashPt = Non-flammable | FlashPt = Non-flammable
| LD50 = 1620 mg/kg (oral, rat) | LD50 = 1620 mg/kg (oral, rat)
}} }}
| Section8 = {{Chembox Related |Section8={{Chembox Related
| OtherAnions = ]<br/>] | OtherAnions = ]<br/>]
| OtherCations = ] | OtherCations = ]
| OtherCpds = ]<br/>] | OtherCompounds = ]<br/>]
}} }}
}} }}


'''Nickel nitrate''' is the ] Ni(NO<sub>3</sub>)<sub>2</sub> or any ] thereof. The ] form is not commonly encountered, thus "nickel nitrate" usually refers to nickel(II) nitrate hexahydrate. The formula for this species is written in two ways. Ni(NO<sub>3</sub>)<sub>2</sub><sup>.</sup>6H<sub>2</sub>O and, more descriptively (NO<sub>3</sub>)<sub>2</sub>. The latter formula indicates that the ](II) center is surrounded by six water molecules in this hydrated salt. The ] anions are not bonded to nickel. '''Nickel nitrate''' is the ] Ni(NO<sub>3</sub>)<sub>2</sub> or any ] thereof. In the hexahydrate, the ] anions are not bonded to nickel. Other hydrates have also been reported: Ni(NO<sub>3</sub>)<sub>2</sub><sup>.</sup>9H<sub>2</sub>O, Ni(NO<sub>3</sub>)<sub>2</sub><sup>.</sup>4H<sub>2</sub>O, and Ni(NO<sub>3</sub>)<sub>2</sub><sup>.</sup>2H<sub>2</sub>O.<ref name=Ullmann>{{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}}</ref>


It is prepared by the reaction of nickel oxide with nitric acid:
(NO<sub>3</sub>)<sub>2</sub> is highly soluble in water, giving emerald green solutions. It is a useful precursor to other nickel(II) derivatives where the water ]s would be replaced.
: NiO + 2 HNO<sub>3</sub> + 5 H<sub>2</sub>O → Ni(NO<sub>3</sub>)<sub>2</sub><sup>.</sup>6H<sub>2</sub>O
The anhydrous nickel nitrate is typically not prepared by heating the hydrates. Rather it is generated by the reaction of hydrates with ] or of ] with ]:<ref name=Ullmann/>
: Ni(CO)<sub>4</sub> + 2 N<sub>2</sub>O<sub>4</sub> → Ni(NO<sub>3</sub>)<sub>2</sub> + 2 NO + 4 CO


The hydrated nitrate is often used as a precursor to ] nickel catalysts.<ref name=Ullmann/>
==Safety==

Like other nitrates, nickel nitrate is ], so that caution should be exercised when it contacts with reducing materials such as ]s. It is also irritating to the eyes, skin and, upon inhalation of the dust, ]. It may cause skin ]. Nickel nitrate is a ], along with most other nickel compounds. The nickel ion is also toxic to aquatic organisms.
==Structure==
Nickel(II) compounds with oxygenated ligands often feature octahedral coordination geometry. Two ] of the tetrahydrate Ni(NO<sub>3</sub>)<sub>2</sub><sup>.</sup>4H<sub>2</sub>O have been crystallized. In one the monodentate nitrate ligands are trans<ref>{{cite journal |doi=10.1107/S0567740879010827|title=Crystal Structure of the β Form of Ni(NO<sub>3</sub>)<sub>2</sub><sup>.</sup>4H<sub>2</sub>O|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}}</ref> while in the other they are cis.<ref>{{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 }}</ref>

==Reactions and uses==
Nickel(II) nitrate is primarily used in ] and ] of metallic nickel.

In heterogeneous catalysis, nickel(II) nitrate is used to impregnate ]. Pyrolysis of the resulting material gives forms of ] and ].<ref>{{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 }}</ref> In ], the hexahydrate is a precatalyst for ]s.<ref>{{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 }}</ref>


==References== ==References==
{{Unreferenced|date =September 2007}}
{{reflist}} {{reflist}}


{{Nickel compounds}} {{Nickel compounds}}
{{nitrates}}


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