Nickel(II) nitrate

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Nickel(II) nitrate
Nickel(II) nitrate
Nickel(II) nitrate
Names
IUPAC name
Nickel(II) nitrate
Other names
Nickel nitrate
Nickelous nitrate
Nitric acid, nickel(2+) salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.032.774 Edit this at Wikidata
EC Number
  • 238-076-4
UNII
UN number 2725
  • InChI=1S/2NO3.Ni/c2*2-1(3)4;/q2*-1;+2 checkY
    Key: KBJMLQFLOWQJNF-UHFFFAOYSA-N checkY
  • InChI=1/2NO3.Ni/c2*2-1(3)4;/q2*-1;+2
    Key: KBJMLQFLOWQJNF-UHFFFAOYAP
  • [Ni+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
Properties
Ni(NO3)2
Molar mass 182.703 g/mol (anhydrous)
290.79 g/mol (hexahydrate)
Appearance emerald green hygroscopic solid
Odor odorless
Density 2.05 g/cm3 (hexahydrate)
Melting point 56.7 °C (134.1 °F; 329.8 K) (hexahydrate)
Boiling point 120–145 °C (248–293 °F; 393–418 K) (hexahydrate, decomposes to basic nickel nitrate)[1]
243 (hexahydrate) g/100ml (0 °C)[2]
Solubility soluble in ethanol
+4300.0·10−6 cm3/mol (+6 H2O)
1.422 (hexahydrate)
Structure
monoclinic (hexahydrate)
Hazards
GHS labelling:
GHS03: OxidizingGHS05: CorrosiveGHS07: Exclamation markGHS08: Health hazardGHS09: Environmental hazard
Danger
H272, H302, H315, H317, H318, H332, H334, H341, H350, H360, H372, H410
P201, P202, P210, P220, P221, P260, P261, P264, P270, P271, P272, P273, P280, P281, P285, P301+P312, P302+P352, P304+P312, P304+P340, P304+P341, P305+P351+P338, P308+P313, P310, P312, P314, P321, P330, P332+P313, P333+P313, P342+P311, P362, P363, P370+P378, P391, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
2
0
0
OX
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1620 mg/kg (oral, rat)
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
 Nickel(II) sulfate
Nickel(II) chloride
Other cations
 Palladium(II) nitrate
Related compounds
 Cobalt(II) nitrate
Copper(II) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Nickel 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.[3]

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:[3]

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.[3]

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[4] while in the other they are cis.[5]

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.[6] In homogeneous catalysis, the hexahydrate is a precatalyst for cross coupling reactions.[7]

References

  1. ^ Pietsch, E. H. E. (1966). Gmelins Handbuch der Anorganischen Chemie, Nickel Teil B 2 (in German) (8th ed.). Weinheim/Bergstr.: Verlag Chemie GmbH. p. 509.
  2. ^ Perry's Chem Eng Handbook, 7th Ed
  3. ^ a b c Lascelles, Keith; Morgan, Lindsay G.; Nicholls, David; Beyersmann, Detmar (2005). "Nickel Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_235.pub2. ISBN 978-3527306732.
  4. ^ Morosin, B.; Haseda, T. (1979). "Crystal Structure of the β Form of Ni(NO3)2.4H2O". Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 35 (12): 2856–2858. doi:10.1107/S0567740879010827.
  5. ^ Gallezot, P.; Weigel, D.; Prettre, M. (1967). "Structure du Nitrate de Nickel Tétrahydraté". Acta Crystallographica. 22 (5): 699–705. Bibcode:1967AcCry..22..699G. doi:10.1107/S0365110X67001392.
  6. ^ Sarko, Christopher R.; Dimare, Marcello; Yus, Miguel; Alonso, Francisco (2014). "Nickel Catalysts (Heterogeneous)". Encyclopedia of Reagents for Organic Synthesis. pp. 1–8. doi:10.1002/047084289X.rn011.pub2. ISBN 978-0-470-84289-8.
  7. ^ Xiao, Yu-Lan; Zhang, Xingang (2017). "Nickel(II) Nitrate Hexahydrate". Encyclopedia of Reagents for Organic Synthesis. pp. 1–3. doi:10.1002/047084289X.rn02013. ISBN 978-0-470-84289-8.
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