Nickel fluoride (NiF2) is a chemical compound. It’s made of nickel and fluorine atoms. Used in various applications, including batteries and electroplating due to its unique properties.
| IUPAC Name | Nickel(II) fluoride |
| Molecular Formula | NiF2 |
| CAS Number | 10028-18-9 |
| Synonyms | Nickel difluoride, Nickelous fluoride, difluoronickel |
| InChI | InChI=1S/2FH.Ni/h2*1H;/q;;+2/p-2 |
Nickel Fluoride Properties
Nickel Fluoride Formula
The chemical formula of nickel difluoride is NiF2. It signifies that each molecule of nickel difluoride consists of one nickel atom and two fluorine atoms bonded together.
Nickel Fluoride Molar Mass
Nickel difluoride has a molar mass of approximately 96.69 grams per mole. This value is calculated by adding the atomic masses of one nickel atom (58.69 g/mol) and two fluorine atoms (18.998 g/mol each).
Nickel Fluoride Boiling Point
The boiling point of nickel difluoride is relatively high, around 1,568 degrees Celsius (2,854 degrees Fahrenheit). This temperature represents the point at which nickel difluoride transitions from its liquid phase to a gaseous state.
Nickel Fluoride Melting Point
Nickel difluoride has a melting point of about 1,372 degrees Celsius (2,502 degrees Fahrenheit). This is the temperature at which solid nickel difluoride turns into a liquid.
Nickel Fluoride Density g/mL
The density of nickel difluoride is approximately 4.72 grams per cubic centimeter (g/cm³). This density value provides insight into how closely the particles are packed within a given volume of the substance.
Nickel Fluoride Molecular Weight
Nickel difluoride’s molecular weight is approximately 96.69 grams per mole. It is determined by summing up the atomic weights of its constituent elements in the chemical formula NiF2.
Nickel Fluoride Structure
Nickel difluoride has a crystalline structure. The nickel atom is at the center, bonded to two fluorine atoms. The arrangement of atoms results in a repeating pattern, forming a crystal lattice.
Nickel Fluoride Solubility
Nickel difluoride is sparingly soluble in water. Its solubility is affected by factors like temperature and the presence of other substances. When it dissolves, it dissociates into Ni+2 ions and F- ions in the aqueous solution.
| Appearance | Green crystalline solid |
| Specific Gravity | 4.72 g/cm³ |
| Color | Green |
| Odor | Odorless |
| Molar Mass | 96.69 g/mol |
| Density | 4.72 g/cm³ |
| Melting Point | 1,372°C (2,502°F) |
| Boiling Point | 1,568°C (2,854°F) |
| Flash Point | Not applicable |
| Water Solubility | Sparingly soluble |
| Solubility | Dissolves in water, dissociates into nickel ions and fluoride ions |
| Vapour Pressure | Not well-defined |
| Vapour Density | Not well-defined |
| pKa | Not applicable |
| pH | Not applicable |
Nickel Fluoride Safety and Hazards
Nickel difluoride poses potential safety hazards. It can cause skin and eye irritation upon contact. Inhalation of its dust or fumes might lead to respiratory irritation. Prolonged exposure could result in more severe health effects. Proper protective measures, including gloves and safety goggles, should be used when handling nickel difluoride. Workspaces must be well-ventilated to minimize inhalation risks. In case of accidental ingestion or contact, medical attention is necessary. Nickel difluoride’s potential environmental impact also requires consideration, and its disposal should follow appropriate regulations to prevent contamination.
| Hazard Symbols | Health Hazard |
| Safety Description | Causes skin and eye irritation. Harmful if inhaled or ingested. Prolonged exposure may cause more severe health effects. Handle with proper protective equipment. Avoid inhalation and contact. |
| UN IDs | Not assigned |
| HS Code | 2826.20.1000 |
| Hazard Class | 6.1 (Toxic substances) |
| Packing Group | III |
| Toxicity | Moderately toxic |
Nickel Fluoride Synthesis Methods
Nickel difluoride can be synthesized through various methods. One common approach involves the reaction between nickel oxide (NiO) or nickel carbonate (NiCO3) with hydrofluoric acid (HF):
- Reaction with Hydrofluoric Acid:
- Nickel Oxide (NiO) Method: NiO + 2 HF → NiF2 + H2O
- Nickel Carbonate (NiCO3) Method: NiCO3 + 4 HF → NiF2 + CO2 + 2 H2O
Another method employs the reaction between nickel chloride (NiCl2) and ammonium fluoride (NH4F):
- Reaction with Ammonium Fluoride: NiCl2 + 2 NH4F → NiF2 + 2 NH4Cl
Additionally, nickel difluoride can be obtained through the reaction of nickel oxide with ammonium fluoride:
- Reaction with Ammonium Fluoride (Nickel Oxide Method): NiO + 2 NH4F → NiF2 + 2 H2O + (NH4)2O
These methods typically take place at controlled temperatures and conditions to ensure proper synthesis and product purity. It’s essential to handle hydrofluoric acid and other reactants with caution due to their potential hazards. The resulting nickel difluoride can be further purified and processed for various applications, such as battery materials and electroplating.
Nickel Fluoride Uses
Nickel difluoride (NiF2) finds diverse applications owing to its unique properties. It serves in various industries for distinct purposes:
- Battery Technology: Used as a component in lithium-ion batteries, enhancing their performance and stability.
- Electroplating: Employed in electroplating processes to create durable and corrosion-resistant nickel coatings on various materials.
- Catalysis: Acts as a catalyst in certain chemical reactions, aiding in the synthesis of valuable products.
- Glass and Ceramics: Incorporated in the production of specialty glass and ceramics, improving their properties and characteristics.
- Fluoridation: Utilized for water fluoridation to improve dental health by preventing tooth decay.
- Chemical Manufacturing: Serves as a precursor in the synthesis of other nickel compounds and chemical substances.
- Ceramic Capacitors: Found in the manufacturing of ceramic capacitors used in electronics and telecommunications.
- Pharmaceuticals: Used as a reagent in some pharmaceutical processes and research.
- Photography: Historically used in the photographic industry as a component of certain photographic developers.
- Metal Alloy Additive: Added to certain metal alloys to enhance their properties like strength and resistance.
Nickel difluoride’s adaptable characteristics make it a valuable resource across an array of industries, contributing to advancements in technology, healthcare, and manufacturing.
Questions:
Q: What are the products at the two electrodes during the electrolysis of a solution of NiF2(aq)?
A: At the cathode, nickel metal (Ni) forms, while at the anode, fluorine gas (F2) evolves.
Q: What is produced from the electrolysis of NiF2?
A: Nickel metal is produced at the cathode, and fluorine gas is evolved at the anode during the electrolysis of NiF2.
Q: The compound NiF2 is an ionic compound. What are the ions of which it is composed?
A: NiF2 is composed of nickel ions (Ni²⁺) and F- ions.
Q: What type of reaction is Ni(s) + F2 —> NiF2(s)?
A: The reaction Ni(s) + F2 → NiF2(s) is a combination (synthesis) reaction.
Q: What is the name of the compound with the formula NiF2?
A: The compound with the formula NiF2 is called nickel(II) difluoride.
Q: Where is nickel(II) fluoride used?
A: Nickel(II) difluoride is used in battery technology, electroplating, catalysts, and ceramic manufacturing.
Q: What is the formula for nickel(II) fluoride?
A: The formula for nickel(II) difluoride is NiF2.
Q: Do nickel(II) fluoride and sodium hydroxide precipitate?
A: Yes, they precipitate as a green solid, nickel(II) hydroxide.
Q: Does nickel fluoride conduct electricity?
A: Yes, nickel difluoride can conduct electricity in its molten state or when dissolved in water.
Q: Is molten nickel fluoride or graphite more conductive?
A: Molten nickel difluoride is more conductive than graphite due to its ionic nature and mobile ions.