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Nickel(II) fluoride

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Nickel(II) fluoride
Names
IUPAC name Nickel(II) fluoride
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.053 Edit this at Wikidata
EC Number
  • 233-071-3
PubChem CID
RTECS number
  • QR6825000
UNII
CompTox Dashboard (EPA)
InChI
  • InChI=1S/2FH.Ni/h2*1H;/q;;+2/p-2Key: DBJLJFTWODWSOF-UHFFFAOYSA-L
  • InChI=1S/2FH.Ni/h2*1H;/q;;+2/p-2Key: DBJLJFTWODWSOF-NUQVWONBAA
  • Key: DBJLJFTWODWSOF-UHFFFAOYSA-L
SMILES
  • FF
Properties
Chemical formula NiF2
Molar mass 96.6902 g/mol
Appearance Yellowish to green tetragonal crystals
Density 4.72 g/cm
Melting point 1,474 °C (2,685 °F; 1,747 K)
Solubility in water 4 g/100 mL
Solubility insoluble in alcohol, ether
Magnetic susceptibility (χ) +2410.0·10 cm/mol
Structure
Crystal structure Rutile
Coordination geometry 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 , 100 kPa). ☒verify (what is  ?) Infobox references
Chemical compound

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:

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. At low temperatures, its magnetic structure is antiferromagnetic.

Reactions

A melt of NiF2 and KF reacts to give successively potassium trifluoronickelate and potassium tetrafluoronickelate:

NiF2 + KF → K
K + KF → K2

The structure of this material is closely related to some superconducting oxide materials.

Nickel(II) fluoride reacts with strong bases to give nickel(II) hydroxide:

NiF2 + 2 NaOH → Ni(OH)2 + 2 NaF

References

  1. Planning. Validations stanford.edu
  2. Priest, H. F. (1950). "Anhydrous Metal Fluorides". Inorganic Syntheses. Vol. 3. pp. 171–183. doi:10.1002/9780470132340.ch47. ISBN 9780470132340.
  3. 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.
  4. Strempfer, J; Ruett, U; Bayrakci, S.P.; Brueckel, Th.; Jauch, W (2004). "Magnetic properties of transition metal fluorides". Phys. Rev. B. 69: 014417. doi:10.1103/PhysRevB.69.014417.
  5. Plevey, R. G.; Rendell, R. W.; Steward, M. P. (1974-01-01). "Fluorination with complex metal fluorides Part III. The fluorination of benzene over potassium hexafluoronickelate(IV)". Journal of Fluorine Chemistry. 3 (3–4): 267–273. Bibcode:1974JFluC...3..267P. doi:10.1016/S0022-1139(00)82626-3. ISSN 0022-1139.
  6. Balz, D. (1953). "Über die Struktur des K2NiF4". Naturwissenschaften. 40 (8): 241. Bibcode:1953NW.....40..241B. doi:10.1007/BF00591545. S2CID 32692990.

External links

Nickel compounds
Nickel(0)
Nickel(II)
Nickel(III)
Nickel(IV)
Salts and covalent derivatives of the fluoride ion
HF ?HeF2
LiF BeF2 BF
BF3
B2F4
+BO3
CF4
CxFy
+CO3
NF3
FN3
N2F2
NF
N2F4
NF2
?NF5
OF2
O2F2
OF
O3F2
O4F2
?OF4
F2 Ne
NaF MgF2 AlF
AlF3
SiF4 P2F4
PF3
PF5
S2F2
SF2
S2F4
SF3
SF4
S2F10
SF6
+SO4
ClF
ClF3
ClF5
?ArF2
?ArF4
KF CaF
CaF2
ScF3 TiF2
TiF3
TiF4
VF2
VF3
VF4
VF5
CrF2
CrF3
CrF4
CrF5
?CrF6
MnF2
MnF3
MnF4
?MnF5
FeF2
FeF3
FeF4
CoF2
CoF3
CoF4
NiF2
NiF3
NiF4
CuF
CuF2
?CuF3
ZnF2 GaF2
GaF3
GeF2
GeF4
AsF3
AsF5
Se2F2
SeF4
SeF6
+SeO3
BrF
BrF3
BrF5
KrF2
?KrF4
?KrF6
RbF SrF
SrF2
YF3 ZrF2
ZrF3
ZrF4
NbF4
NbF5
MoF4
MoF5
MoF6
TcF4
TcF
5

TcF6
RuF3
RuF
4

RuF5
RuF6
RhF3
RhF4
RhF5
RhF6
PdF2
Pd
PdF4
?PdF6
Ag2F
AgF
AgF2
AgF3
CdF2 InF
InF3
SnF2
SnF4
SbF3
SbF5
TeF4
?Te2F10
TeF6
+TeO3
IF
IF3
IF5
IF7
+IO3
XeF2
XeF4
XeF6
?XeF8
CsF BaF2   LuF3 HfF4 TaF5 WF4
WF5
WF6
ReF4
ReF5
ReF6
ReF7
OsF4
OsF5
OsF6
?OsF
7

?OsF
8
IrF2
IrF3
IrF4
IrF5
IrF6
PtF2
Pt
PtF4
PtF5
PtF6
AuF
AuF3
Au2F10
?AuF6
AuF5•F2
Hg2F2
HgF2
?HgF4
TlF
TlF3
PbF2
PbF4
BiF3
BiF5
?PoF2
PoF4
PoF6
AtF
?AtF3
?AtF5
RnF2
?RnF
4

?RnF
6
FrF RaF2   LrF3 Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
LaF3 CeF3
CeF4
PrF3
PrF4
NdF2
NdF3
NdF4
PmF3 SmF2
SmF3
EuF2
EuF3
GdF3 TbF3
TbF4
DyF2
DyF3
DyF4
HoF3 ErF3 TmF2
TmF3
YbF2
YbF3
AcF3 ThF3
ThF4
PaF4
PaF5
UF3
UF4
UF5
UF6
NpF3
NpF4
NpF5
NpF6
PuF3
PuF4
PuF5
PuF6
AmF2
AmF3
AmF4
?AmF6
CmF3
CmF4
 ?CmF6
BkF3
BkF
4
CfF3
CfF4
EsF3
EsF4
?EsF6
Fm Md No
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