nickel(II) fluoride
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| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 442654399
| ImageFile = Fluorid nikelnatý.PNG
| ImageSize =
| ImageFile1 = Nickel(II)-fluoride-unit-cell-3D-balls.png
| ImageCaption1 = {{color box|rgb(96, 64, 256)}} Nickel, Ni; {{color box|rgb(192,256,128)}} Fluorine, F
| IUPACName = Nickel(II) fluoride
| OtherNames =
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 23210
| InChI = 1S/2FH.Ni/h2*1H;/q;;+2/p-2
| InChIKey = DBJLJFTWODWSOF-NUQVWONBAA
| SMILES = F[Ni]F
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/2FH.Ni/h2*1H;/q;;+2/p-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = DBJLJFTWODWSOF-UHFFFAOYSA-L
| InChIKey1 = DBJLJFTWODWSOF-UHFFFAOYSA-L
| CASNo = 10028-18-9
| CASNo_Ref = {{cascite|correct|CAS}}
| UNII_Ref = {{fdacite|changed|FDA}}
| UNII = 69NBB20493
| EINECS = 233-071-3
| PubChem = 24825
| RTECS = QR6825000
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|Section2={{Chembox Properties
| Formula = NiF2
| MolarMass = 96.6902 g/mol
| Appearance = Yellowish to green tetragonal crystals
| Density = 4.72 g/cm3
| MeltingPtC = 1474
| BoilingPtC =
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| Solubility = 4 g/100 mL
| SolubleOther = insoluble in alcohol, ether
| Solvent =
| LogP =
| MagSus = +2410.0·10−6 cm3/mol
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|Section3={{Chembox Structure
| CrystalStruct = Rutile
| Coordination = Nickel: Octahedral
Oxygen: Trigonal planar
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|Section4={{Chembox Thermochemistry
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|Section7={{Chembox Hazards
| ExternalSDS = [http://www.gfschemicals.com/Search/MSDS/A5352MSDS.PDF External MSDS]
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|Section8={{Chembox Related
| OtherAnions = Nickel(II) chloride
Nickel(II) bromide
Nickel(II) iodide
| OtherCations = Cobalt(II) fluoride
Copper(II) fluoride
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Nickel(II) fluoride is the chemical compound with the formula NiF2. It is an ionic compound of nickel and fluorine and forms yellowish to green tetragonal crystals. Unlike many fluorides, NiF2 is stable in air.
Nickel(II) fluoride is also produced when nickel metal is exposed to fluorine. In fact, NiF2 comprises the passivating surface that forms on nickel alloys (e.g. monel) in the presence of hydrogen fluoride or elemental fluorine. For this reason, nickel and its alloys are suitable materials for storage and transport these fluorine and related fluorinating agents. 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:{{cite book|author=Priest, H. F. |title=Inorganic Syntheses |chapter=Anhydrous Metal Fluorides|year=1950|volume=3|pages=171–183|doi=10.1002/9780470132340.ch47|isbn=9780470132340 }}
: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.
Like some other metal difluorides, NiF2 crystallizes in the rutile structure, which features octahedral Ni centers and planar fluorides.{{cite journal |doi=10.1021/ja01650a005|title=The Crystal Structure of MnF2, FeF2, CoF2, NiF2 and ZnF2|first1=J. W.|last1=Stout|first2=Stanley A.|last2=Reed|journal= J. Am. Chem. Soc.|year=1954|volume=76|issue=21|pages=5279–5281}}
At low temperatures, its magnetic structure is antiferromagnetic.{{cite journal|doi=10.1103/PhysRevB.69.014417| first1=J|last1=Strempfer |first2=U|last2=Ruett |first3=S.P.|last3=Bayrakci|first4=Th.|last4=Brueckel|first5=W|last5=Jauch|title=Magnetic properties of transition metal fluorides |journal=Phys. Rev. B| volume=69|pages=014417|year=2004}}
Reactions
A melt of NiF2 and KF reacts to give successively potassium trifluoronickelate and potassium tetrafluoronickelate:{{Cite journal |last1=Plevey |first1=R. G. |last2=Rendell |first2=R. W. |last3=Steward |first3=M. P. |date=1974-01-01 |title=Fluorination with complex metal fluorides Part III. The fluorination of benzene over potassium hexafluoronickelate(IV) |url=https://www.sciencedirect.com/science/article/pii/S0022113900826263 |journal=Journal of Fluorine Chemistry |volume=3 |issue=3–4 |pages=267–273 |doi=10.1016/S0022-1139(00)82626-3 |bibcode=1974JFluC...3..267P |issn=0022-1139}}
:NiF2 + KF → K[NiF3]
:K[NiF3] + KF → K2[NiF4]
The structure of this material is closely related to some superconducting oxide materials.{{cite journal|author=Balz, D.|title=Über die Struktur des K2NiF4|journal=Naturwissenschaften|year=1953|page=241|volume=40|issue=8 |doi=10.1007/BF00591545|bibcode=1953NW.....40..241B |s2cid=32692990 }}
Nickel(II) fluoride reacts with strong bases to give nickel(II) hydroxide:
:NiF2 + 2 NaOH → Ni(OH)2 + 2 NaF
References
External links
{{Commons category|Nickel(II) fluoride}}
- [http://monographs.iarc.fr/ENG/Monographs/vol49/mono49-7.pdf IARC Monograph "Nickel and Nickel compounds"]
- [https://web.archive.org/web/20060116134617/http://www.npi.gov.au/database/substance-info/profiles/44.html National Pollutant Inventory - Fluoride compounds fact sheet]
- [https://web.archive.org/web/20060820043848/http://www.npi.gov.au/database/substance-info/profiles/62.html National Pollutant Inventory - Nickel and compounds fact sheet]
{{Nickel compounds}}
{{fluorides}}