PRODUCTS

NICKEL FLUORIDE

CAS NO.: 10028-18-9
EC/LIST NO.: 233-071-3

Nickel fluoride is the chemical compound with the formula NiF2.

Nickel fluoride is an ionic compound of nickel and fluorine and forms yellowish to green tetragonal crystals.
Unlike many fluorides, NiF2 is stable in air.

Nickel fluoride 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.
Nickel fluoride is also used as a catalyst for the synthesis of chlorine pentafluoride.

Nickel Fluoride is a water insoluble Nickel source for use in oxygen-sensitive applications, such as metal production.
Fluoride compounds have diverse applications in current technologies and science, from oil refining and etching to synthetic organic chemistry and the manufacture of pharmaceuticals.
Magnesium Fluoride, for example, was used by researchers at the Max Planck Institute for Quantum Optics in 2013 to create a novel mid-infrared optical frequency comb composed of crystalline microresonators, a development that may lead to future advances in molecular spectroscopy.
Fluorides are also commonly used to alloy metals and for optical deposition. Nickel Fluoride is generally immediately available in most volumes.
Ultra high purity and high purity compositions improve both optical quality and usefulness as scientific standards.
Nanoscale elemental powders and suspensions, as alternative high surface area forms, may be considered.
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Nickel fluoride is a water insoluble Nickel source and an ionic compound of nickel and fluorine.
Nickel fluoride forms yellowish to green tetragonal crystals.
Unlike many fluorides, Nickel fluoride is stable in air.

Nickel fluoride has the tetragonal rutile structure with only slightly tetragonally compressed NiF6 octahedra; the Ni-F distances being 2.01 and 1.98 ?.
Above the melting point it sublimes as a linear gaseous molecule.
The anhydrous fluoride is rather unreactive towards concentrated acids;
Nickel fluoride is only slightly soluble in anhydrous hydrogen fluoride and is not attacked by electronegative elements such as chlorine, sulphur and phosphorus.
The pale green tetrahydrate is slightly soluble in water;
when heated, several intermediate hydrates are formed prior to N1F2.

Nickel fluoride is a group VIII transition metal.
Nickel fluoride is used with other metals to form alloys to make such items as coins, jewelry, valves, heat exchangers, and stainless steel.
Nickel compounds are also used to color ceramics, in batteries, and as catalysts.
Although it can exist in several different oxidation states, the only important oxidation state under environmental conditions is Ni2+.
Nickel fluoride has been suggested that nickel may be essential in humans, at levels of less than 0.1 mg Ni/day (<0.001 mg Ni/kg/day for a 70 kg adult), although no nickel requirement or allowance has been set.
Nickel fluoride is present in most dietary items, and food is considered to be a major source of exposure to nickel for the general population.
Systemic reactions, such as generalized eczematous reactions or dyshidrotic hand eczema, can occur due to dietary ingestion of nickel.

Nickel Fluoride, CAS 13940-83-5, has the formula NiF2.
Nickel Fluoride is used in metal plating operations, as a passivation layer on advanced nickel metals such as monel, in metal cold sealing applications, as a catalyst for the production of chlorine pentafluoride, in marking ink compositions for fluorescent lamps, as a transhalogenation catalyst for fluoroolefins, in the manufacture of varistors, as a catalyst for hydrofluorination, in the synthesis of xenon hexafluoride, and in the preparation of high purity elemental fluorine for research and chemical lasers.

This report is divided into four sections.
The first contains the data on electrolyte studies, particularly those to be used with nickel fluoride cathode.
Conductivity, viscosity, and equivalent conductivity at infinite dilution, are given for most of the solute-solvent combinations.
The second section deals with the nickel fluoride cathode.
Data on porosity, pore size distribution, true surface area by the BET method and electrode performance are given for a variety of electrode mixes.
Variations of conductive diluent, binder, and extender, as well as various types of nickel fluoride were used.
The third section contains cell testing data.
Automatic cycling and chronopotentiometric tests are presented.
The fourth section contains the conclusions.
Those are that propylene carbonate with potassium hexafluorophosphate is still the most practical electrolyte.
The conductive diluent has the greatest effect on the surface areas and pore size distribution so it has the greatest electrochemical effect on the electrode.
Conductex, a high conductivity carbon produced the best electrode

In this study, the use of nickel fluoride tetrahydrate (NiF 2 ·4H 2 O) as a surface activator and sealant at the same time for the coating of electroless nickel-phosphorus (Ni-P) on anodized aluminum alloy AA1050 is proposed.
The usage of the activator resulted in more efficient deposition of Ni-P, improved adhesion properties, and increased wear and friction behavior as opposed to non-activated conditions.
Scanning electron microscopy (SEM) and confocal laser microscopy (CLM) analyses of ultramicrotome-cut cross sections of Ni-P coated specimens, surface-activated by NiF 2 ·4H 2 O, revealed a more well-structured metal-coating interface as opposed to non-activated conditions.

Nickel fluoride is the chemical compound with the formula NiF2.
Unlike many fluorides, Nickel fluoride is stable in air.
Nickel fluoride comprises the passivating surface that forms on nickel alloys, e.g. monel, which is why such materials are good to store or transport hydrogen fluoride or elemental fluorine.
Nickel is one of the few materials that can be used to store fluorine because it forms this coating.
Nickel fluoride is also used as a catalyst for the synthesis of chlorine pentafluoride.

Nickel fluoride 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.

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

Compound Formula   : F2Ni
Molecular Weight   : 96.69
Appearance   : Yellow Crystalline Solid
Melting Point   : 1,474° C (2,685° F)
Boiling Point   : 1,750° C (3,182° F)
Density   : 4.72 g/cm3
Solubility in H2O   : N/A
Exact : Mass   N/A
Monoisotopic Mass   : 95.932155 Da
Charge   : N/A

Nickel fluoride comprises the passivating surface that forms on nickel alloys, e.g. monel, which is why such materials are good to store or transport hydrogen fluoride or elemental fluorine.

IUPAC NAME:

dinickel(2+) tetrahydrate tetrafluoride

nickel difluoride

Nickel Difluoride

nickel difluoride

Nickel Fluoride

SYNONYMS:

10028-18-9
233-071-3
Difluorure de nickel(2+)
NICKEL DIFLUORIDE
Nickel fluoride
Nickel(2+) difluoride
Nickel(2+)difluorid
Nickel(II) fluoride
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11113-73-8 [RN]