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{{chembox |
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{{Chembox |
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| verifiedrevid = 400325570 |
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| verifiedrevid = 442654399 |
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| ImageFile = Fluorid nikelnatý.PNG |
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| ImageFile = Fluorid nikelnatý.PNG |
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| IUPACName = Nickel(II) fluoride |
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| IUPACName = Nickel(II) fluoride |
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| OtherNames = |
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| OtherNames = |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 23210 |
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| ChemSpiderID = 23210 |
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| InChIKey1 = DBJLJFTWODWSOF-UHFFFAOYSA-L |
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| InChIKey1 = DBJLJFTWODWSOF-UHFFFAOYSA-L |
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| CASNo = 10028-18-9 |
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| CASNo = 10028-18-9 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| UNII_Ref = {{fdacite|changed|FDA}} |
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| EINECS = |
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| UNII = 69NBB20493 |
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| EINECS = 233-071-3 |
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| PubChem = 24825 |
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| PubChem = 24825 |
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| InChI = |
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| RTECS = QR6825000 |
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| RTECS = QR6825000 |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = NiF<sub>2</sub> |
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| Formula = NiF<sub>2</sub> |
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| MolarMass = 96.6902 g/mol |
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| MolarMass = 96.6902 g/mol |
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| Appearance = Yellowish to green tetragonal crystals |
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| Appearance = Yellowish to green tetragonal crystals |
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| Density = 4.72 g/cm<sup>3</sup> |
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| Density = 4.72 g/cm<sup>3</sup> |
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| MeltingPtC = 1474 |
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| MeltingPt = 1474°C <ref>http://www.slac.stanford.edu/BFROOT/www/Detector/Backgrounds/BkG4Sim/Planning/Validations/neutronCounters/04_02_85.pdf</ref> |
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| MeltingPt_ref = <ref> stanford.edu {{dead link|date=June 2023}}</ref> |
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| BoilingPt = 1750°C <ref>http://www.indiamart.com/primechemicals/inorganic-fluorine.html</ref> |
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| Solubility = 4 g/100 ml water (25°C) |
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| Solubility = 4 g/100 mL |
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| SolubleOther = insoluble in ], ] |
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| Solvent = |
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| LogP = |
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| MagSus = +2410.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section3 = {{Chembox Structure |
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| CrystalStruct = ] |
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| CrystalStruct = ] |
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| Coordination = Nickel: ]<br/>Oxygen: Trigonal planar |
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| Coordination = Nickel: ]<br />Oxygen: Trigonal planar |
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| Section4 = {{Chembox Thermochemistry |
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| Section7 = {{Chembox Hazards |
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| FlashPt = |
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| Section8 = {{Chembox Related |
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|Section8={{Chembox Related |
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| OtherAnions = ]<br/>]<br/>] |
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| OtherAnions = ]<br />]<br />] |
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| OtherCations = ]<br/>] |
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| OtherCations = ]<br />] |
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'''Nickel(II) fluoride''' is the ] with the formula NiF<sub>2</sub>. Unlike many fluorides, NiF<sub>2</sub> is stable in air. NiF<sub>2</sub> comprises the ] surface that forms on nickel alloys, e.g. ], which is why such materials are good to store or transport ] or elemental ]. Nickel is one of the few materials that can be used to store fluorine because it forms this coating. It is also used as a catalyst for the synthesis of ]. |
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'''Nickel(II) fluoride''' is the ] with the formula NiF<sub>2</sub>. It is an ionic compound of ] and ] and forms yellowish to green tetragonal crystals. Unlike many fluorides, NiF<sub>2</sub> is stable in air. |
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Nickel(II) fluoride is also produced when nickel metal is exposed to fluorine. In fact, NiF<sub>2</sub> comprises the ] surface that forms on nickel alloys (e.g. ]) in the presence of ] or elemental ]. For this reason, nickel and its alloys are suitable materials for storage and transport these fluorine and related fluorinating agents. NiF<sub>2</sub> is also used as a catalyst for the synthesis of ]. |
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NiF<sub>2</sub> is prepared by treatment of anhydrous ] with ] at 350 °C:<ref>Priest, H. F. “Anhydrous Metal Fluorides” Inorganic Syntheses McGraw-Hill: New York, 1950; Vol. 3, pages 171-183.</ref> |
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== Preparation and structure== |
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:] + ] → NiF<sub>2</sub> + ] |
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NiF<sub>2</sub> is prepared by treatment of anhydrous ] with ] at 350 °C:<ref>{{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 }}</ref> |
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:NiCl<sub>2</sub> + F<sub>2</sub> → NiF<sub>2</sub> + Cl<sub>2</sub> |
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The corresponding reaction of ] results in ] of the ], whereas nickel remains in the +2 ] 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. |
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The corresponding reaction of ] results in ] of the ], whereas nickel remains in the +2 ] 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. |
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Like some other metal difluorides, NiF<sub>2</sub> crystallizes in the ] structure, which features octahedral Ni centers and planar fluorides.<ref>{{cite journal |doi=10.1021/ja01650a005|title=The Crystal Structure of MnF<sub>2</sub>, FeF<sub>2</sub>, CoF<sub>2</sub>, NiF<sub>2</sub> and ZnF<sub>2</sub>|first1=J. W.|last1=Stout|first2=Stanley A.|last2=Reed|journal= J. Am. Chem. Soc.|year=1954|volume=76|issue=21|pages=5279–5281}}</ref> |
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A melt of NiF<sub>2</sub> and KF reacts to give the green compound K<sub>2</sub>. The structure of this material is closely related to some superconducting oxide materials.<ref>Balz, D. "Über die Struktur des K<sub>2</sub>NiF<sub>4</sub>" Naturwissenschaften 1953, page 241.</ref> |
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At low temperatures, its magnetic structure is antiferromagnetic.<ref>{{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}}</ref> |
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== Reactions == |
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Nickel(II) fluoride reacts with strong ] to make ], a green colored compound. |
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A melt of NiF<sub>2</sub> and KF reacts to give successively potassium trifluoronickelate and ]:<ref>{{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}}</ref> |
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:NiF<sub>2</sub> + KF → K |
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:K + KF → K<sub>2</sub> |
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The structure of this material is closely related to some superconducting oxide materials.<ref>{{cite journal|author=Balz, D.|title=Über die Struktur des K<sub>2</sub>NiF<sub>4</sub>|journal=Naturwissenschaften|year=1953|page=241|volume=40|issue=8 |doi=10.1007/BF00591545|bibcode=1953NW.....40..241B |s2cid=32692990 }}</ref> |
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NiF<sub>2</sub> + 2 NaOH → Ni(OH)<sub>2</sub> + 2 NaF |
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Nickel(II) fluoride reacts with strong ] to give ]: |
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:NiF<sub>2</sub> + 2 NaOH → Ni(OH)<sub>2</sub> + 2 NaF |
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==References== |
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== External links == |
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== External links == |
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{{Commons cat|Nickel(II) fluoride}} |
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{{Commons category|Nickel(II) fluoride}} |
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