Nickel(II) fluoride

Summary

Nickel(II) fluoride
Fluorid nikelnatý.PNG
Nickel(II)-fluoride-unit-cell-3D-balls.png
Names
IUPAC name
Nickel(II) fluoride
Identifiers
  • 10028-18-9 checkY
3D model (JSmol)
  • Interactive image
ChemSpider
  • 23210 checkY
ECHA InfoCard 100.030.053 Edit this at Wikidata
EC Number
  • 233-071-3
  • 24825
RTECS number
  • QR6825000
UNII
  • 69NBB20493 ☒N
  • DTXSID5064912 Edit this at Wikidata
  • InChI=1S/2FH.Ni/h2*1H;/q;;+2/p-2 checkY
    Key: DBJLJFTWODWSOF-UHFFFAOYSA-L checkY
  • InChI=1S/2FH.Ni/h2*1H;/q;;+2/p-2
    Key: DBJLJFTWODWSOF-NUQVWONBAA
  • Key: DBJLJFTWODWSOF-UHFFFAOYSA-L
  • F[Ni]F
Properties
NiF2
Molar mass 96.6902 g/mol
Appearance Yellowish to green tetragonal crystals
Density 4.72 g/cm3
Melting point 1,474 °C (2,685 °F; 1,747 K) [2]
Boiling point 1,750 °C (3,180 °F; 2,020 K) [1]
4 g/100 mL
Solubility insoluble in alcohol, ether
+2410.0·10−6 cm3/mol
Structure
Rutile
Nickel: Octahedral
Oxygen: Trigonal planar
Hazards
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
Nickel(II) chloride
Nickel(II) bromide
Nickel(II) iodide
Other cations
Cobalt(II) fluoride
Copper(II) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Nickel(II) fluoride is the chemical compound with the formula NiF2. Its is an ionic compound of nickel and fluorine and forms yellowish to green tetragonal crystals. Unlike many fluorides, NiF2 is stable in air.

NiF2 comprises the passivating surface that forms on nickel alloys (e.g. monel) in the presence of hydrogen fluoride or elemental fluorine, which is why nickel and its alloys are among the few materials that can be used to store or transport these fluorine compounds. NiF2 is also used as a catalyst for the synthesis of chlorine pentafluoride.

Preparation and structure

NiF2 is prepared by treatment of anhydrous nickel(II) chloride with fluorine at 350 °C:[3]

NiCl2 + F2 → NiF2 + Cl2

The corresponding reaction of cobalt(II) chloride results in oxidation of the cobalt, whereas nickel remains in the +2 oxidation state after fluorination because its +3 oxidation state is less stable. Chloride is more easily oxidized than nickel(II). This is a typical halogen displacement reaction, where a halogen plus a less active halide makes the less active halogen and the more active halide.

Nickel(II) fluoride is also produced when fluorine reacts with nickel metal.


Like some other metal difluorides, NiF2 crystallizes in the rutile structure, which features octahedral Ni centers and planar fluorides.[4]

Reactions

A melt of NiF2 and KF reacts to give the green compound K2[NiF4]. The structure of this material is closely related to some superconducting oxide materials.[5]

Nickel(II) fluoride reacts with strong bases to make nickel(II) hydroxide, a green colored compound.

NiF2 + 2 NaOH → Ni(OH)2 + 2 NaF

References

  1. ^ http://www.indiamart.com/primechemicals/inorganic-fluorine.html
  2. ^ http://www.slac.stanford.edu/BFROOT/www/Detector/Backgrounds/BkG4Sim/Planning/Validations/neutronCounters/04_02_85.pdf[bare URL PDF]
  3. ^ Priest, H. F. "Anhydrous Metal Fluorides" Inorganic Syntheses McGraw-Hill: New York, 1950; Vol. 3, pages 171-183.
  4. ^ Stout, J. W.; Reed, Stanley A. (1954). "The Crystal Structure of MnF2, FeF2, CoF2, NiF2 and ZnF2". J. Am. Chem. Soc. 76 (21): 5279–5281. doi:10.1021/ja01650a005.
  5. ^ Balz, D. "Über die Struktur des K2NiF4" Naturwissenschaften 1953, page 241.

External links

  • IARC Monograph "Nickel and Nickel compounds"
  • National Pollutant Inventory - Fluoride compounds fact sheet
  • National Pollutant Inventory - Nickel and compounds fact sheet