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| Names | |
|---|---|
| IUPAC name Nickel(II) fluoride | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider | |
| ECHA InfoCard | 100.030.053  |
| EC Number |
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PubChem CID | |
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| UNII | |
CompTox Dashboard (EPA) | |
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SMILES
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| Properties | |
Chemical formula | 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 | |
Crystal structure | Rutile |
| Nickel: Octahedral Oxygen: Trigonal planar | |
| Hazards | |
| Safety data sheet | 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). | |
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
NiF2 is prepared by treatment of anhydrous nickel(II) chloride with fluorine at 350 °C:[3]
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.
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.[4]
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
- ^ http://www.indiamart.com/primechemicals/inorganic-fluorine.html
- ^ http://www.slac.stanford.edu/BFROOT/www/Detector/Backgrounds/BkG4Sim/Planning/Validations/neutronCounters/04_02_85.pdf
- ^ Priest, H. F. “Anhydrous Metal Fluorides” Inorganic Syntheses McGraw-Hill: New York, 1950; Vol. 3, pages 171-183.
- ^ Balz, D. "Über die Struktur des K2NiF4" Naturwissenschaften 1953, page 241.