Zinc fluoride (ZnF2) is a chemical compound. It’s formed by zinc and fluorine. It’s used in various industries like dental care and electronics due to its unique properties.
| IUPAC Name | Zinc Fluoride |
| Molecular Formula | ZnF2 |
| CAS Number | 7783-49-5 |
| Synonyms | Zinc difluoride, Zinc(II) fluoride |
| InChI | InChI=1S/2FH.Zn/h2*1H;/q;;+2/p-2 |
Zinc Fluoride Properties
Zinc Fluoride Formula
The chemical formula of zinc difluoride is ZnF2. This formula signifies that each molecule of zinc difluoride consists of one zinc atom (Zn) and two fluorine atoms (F).
Zinc Fluoride Molar Mass
The molar mass of zinc difluoride (ZnF2) is approximately 103.38 g/mol. This value is calculated by adding the atomic masses of one zinc atom and two fluorine atoms.
Zinc Fluoride Boiling Point
Zinc difluoride has a boiling point of around 872°C (1602°F). This is the temperature at which the compound transitions from a liquid to a gaseous state under standard atmospheric pressure.
Zinc Fluoride Melting Point
The melting point of zinc difluoride is approximately 872°C (1602°F). At this temperature, the solid form of zinc difluoride changes into a liquid.
Zinc Fluoride Density g/mL
The density of zinc difluoride is about 4.95 g/mL. This value represents the mass of the compound per unit volume and indicates its heaviness.
Zinc Fluoride Molecular Weight
The molecular weight of zinc difluoride (ZnF2) is approximately 103.38 g/mol. This value represents the sum of the atomic weights of all the atoms in one molecule of the compound.
Zinc Fluoride Structure
Zinc difluoride (ZnF2) has a crystal structure in which each zinc atom is surrounded by four fluoride ions in a tetrahedral arrangement. This arrangement contributes to the compound’s stability.
Zinc Fluoride Solubility
Zinc difluoride demonstrates limited solubility in water. It is sparingly soluble, meaning that only a small amount of the compound can dissolve in water to form a solution. This characteristic is important for various industrial applications and chemical processes.
| Appearance | White solid |
| Specific Gravity | 4.95 g/cm³ |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 103.38 g/mol |
| Density | 4.95 g/mL |
| Melting Point | 872°C (1602°F) |
| Boiling Point | 872°C (1602°F) |
| Flash Point | Not applicable |
| Water Solubility | Limited solubility |
| Solubility | Sparingly soluble, only a small amount can dissolve in water |
| Vapor Pressure | Not well-defined |
| Vapor Density | Not well-defined |
| pKa | Not applicable |
| pH | Neutral |
Zinc Fluoride Safety and Hazards
Zinc difluoride (ZnF2) poses certain safety considerations. It’s important to handle this compound with care. Avoid inhalation or ingestion, as it can lead to respiratory and gastrointestinal irritation. When working with ZnF2, wear appropriate personal protective equipment like gloves and safety goggles to prevent skin and eye contact. In case of accidental contact, rinse affected areas thoroughly with water. Store zinc difluoride away from incompatible materials and sources of heat. While it’s not highly toxic, it’s wise to follow proper handling procedures and ensure good ventilation to minimize potential risks associated with its use.
| Hazard Symbols | Corrosive, Irritant, Acute Toxic |
| Safety Description | Handle with care. Avoid inhalation and ingestion. Wear protective equipment. |
| UN IDs | Not applicable |
| HS Code | 28261900 |
| Hazard Class | Not classified |
| Packing Group | Not applicable |
| Toxicity | Low toxicity |
Zinc Fluoride Synthesis Methods
Zinc difluoride can be synthesized through various methods. One common approach involves the reaction between zinc oxide (ZnO) and hydrofluoric acid (HF). In this method, ZnO is mixed with HF, resulting in the formation of Zinc difluoride and water. Another method involves the reaction between zinc carbonate (ZnCO3) and hydrofluoric acid. Zinc carbonate reacts with HF to produce Zinc difluoride, carbon dioxide, and water.
Additionally, Zinc difluoride can also be prepared by reacting zinc metal with fluorine gas (F2) at elevated temperatures. This reaction yields Zinc difluoride directly along with the release of heat.
Furthermore, precipitation methods can be employed, where soluble zinc salts are reacted with soluble fluoride salts to form insoluble Zinc difluoride, which can then be separated and collected.
It’s important to exercise caution during these synthesis processes due to the reactivity of the chemicals involved. Proper safety measures and equipment should be used to ensure the successful and safe synthesis of Zinc difluoride.
Zinc Fluoride Uses
Zinc difluoride (ZnF2) finds versatile applications across various industries due to its unique properties. Here are its primary uses:
- Dental Care: Strengthen tooth enamel and enhance oral hygiene by incorporating ZnF2 into toothpaste formulations.
- Optics and Coatings: Improve lens anti-reflective properties and enhance light transmission using ZnF2 in optical coatings.
- Electronics: Integrate ZnF2 into thin-film transistor (TFT) displays for creating transparent conducting films.
- Fluoride Ion Source: Utilize ZnF2 as a source of fluoride ions in electrolytic cells to aid in producing reactive metals like aluminum.
- Chemical Synthesis: Employ ZnF2 as a catalyst and fluorinating agent in various chemical reactions to facilitate the synthesis of pharmaceuticals and agrochemicals.
- Galvanizing: Apply ZnF2 in metal finishing processes to ready metal surfaces for galvanization, boosting adhesion and durability.
- Infrared Windows: Manufacture infrared sensor windows and thermal imaging systems using ZnF2 due to its transparency in the infrared region.
- Laser Applications: Use ZnF2 as a laser gain medium to contribute to developing tunable lasers for scientific and industrial purposes.
- Crystal Growth: Incorporate ZnF2 into crystal growth processes for semiconductors and other electronic components.
- Chemical Research: Employ ZnF2 as a reactant and reagent in various laboratory-scale chemical reactions, aiding in exploring new compounds.
These diverse applications highlight zinc difluoride’s significance in modern technologies, manufacturing, and scientific research across multiple domains.
Questions:
Q: What is the chemical formula for zinc fluoride?
A: The chemical formula for zinc difluoride is ZnF2.
Q: What is the formula for zinc(II) fluoride?
A: The formula for zinc(II) difluoride is ZnF2.
Q: What is the formula of the ionic compound formed from zinc and fluoride ions?
A: The formula of the ionic compound formed from Zn+2 and fluoride ions is ZnF2.
Q: What may happen due to deficiencies in zinc, iodine, or fluoride?
A: Deficiencies in Zn, iodine, or fluoride can lead to various health issues, affecting metabolism, thyroid function, and dental health.
Q: Which of the following does not have an RDA? a. iron b. zinc c. iodine d. fluoride
A: Fluoride does not have an RDA (Recommended Dietary Allowance).
Q: How can zinc fluoride affect a human?
A: Zinc difluoride can affect humans through potential ingestion, inhalation, or skin contact, possibly causing irritation or toxicity.
Q: Is ZnF2 ionic or molecular?
A: ZnF2 is an ionic compound.
Q: Why is it ZnF2 and not ZnF?
A: ZnF2 indicates that each Zn atom is bonded to two F- ions, forming the correct stoichiometry.
Q: Will ZnF2 and NaOH form a precipitate?
A: Yes, ZnF2 and NaOH can form a white precipitate of zinc hydroxide (Zn(OH)2).
Q: Is ZnF2 soluble?
A: ZnF2 is sparingly soluble in water.
Q: What is the name of the compound with the formula ZnF2?
A: The compound with the formula ZnF2 is called zinc difluoride.
Q: The Ksp of ZnF2 is 3.0 × 10⁻² at 25°C. What is ΔG°?
A: The value of ΔG° can be calculated based on the given Ksp value and temperature using the appropriate thermodynamic equation.
Q: What is ZnF2?
A: ZnF2 is the chemical formula for zinc difluoride, a compound of zinc and fluorine.
Q: How many moles in ZnF2?
A: The number of moles in ZnF2 depends on the given mass and the molar mass of the compound.