Loading AI tools
Chemical compound From Wikipedia, the free encyclopedia
Zirconium(IV) fluoride describes members of a family inorganic compounds with the formula ZrF4(H2O)x. All are colorless, diamagnetic solids. Anhydrous Zirconium(IV) fluoride is a component of ZBLAN fluoride glass.[2]
-fluorid.png) | |
| Names | |
|---|---|
| IUPAC names
Zirconium(IV) fluoride Zirconium tetrafluoride | |
| Identifiers | |
| |
3D model (JSmol) |
|
| ChemSpider | |
| ECHA InfoCard | 100.029.107 |
| EC Number |
|
PubChem CID |
|
| UNII | |
CompTox Dashboard (EPA) |
|
| |
| |
| Properties | |
| ZrF4 | |
| Molar mass | 167.21 g/mol |
| Appearance | white crystalline powder |
| Density | 4.43 g/cm3 (20 °C) |
| Melting point | 910 °C (1,670 °F; 1,180 K) |
| 1.32 g/100mL (20 °C) 1.388 g/100mL (25 °C) | |
| Structure | |
| Monoclinic, mS60 | |
| C12/c1, No. 15 | |
| Hazards | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) |
98 mg/kg (oral, mouse) 98 mg/kg (oral, rat)[1] |
| Related compounds | |
Other anions |
Zirconium(IV) chloride Zirconium(IV) bromide Zirconium(IV) iodide |
Other cations |
Titanium(IV) fluoride Hafnium(IV) fluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Three crystalline phases of ZrF4 have been reported, α (monoclinic), β (tetragonal, Pearson symbol tP40, space group P42/m, No 84) and γ (unknown structure). β and γ phases are unstable and irreversibly transform into the α phase at 400 °C.[3]
Zirconium(IV) fluoride forms several hydrates. The trihydrate has the structure (μ−F)2[ZrF3(H20)3]2.[4]
Zirconium fluoride can be produced by several methods. Zirconium dioxide reacts with hydrogen fluoride and hydrofluoric acid to afford the anhydrous and monohydrates:
The reaction of Zr metal reacts at high temperatures with HF as well:
Zirconium dioxide reacts at 200 °C with solid ammonium bifluoride to give the heptafluorozirconate salt, which can be converted to the tetrafluoride at 500 °C:
Addition of hydrofluoric acid to solutions of zirconium nitrate precipitates solid monohydrate. Hydrates of zirconium tetrafluoride can be dehydrated by heating under a stream of hydrogen fluoride.
Zirconium fluoride can be purified by distillation or sublimation.[2]
Zirconium fluoride forms double salts with other fluorides. The most prominent is potassium hexafluorozirconate, formed by fusion of potassium fluoride and zirconium tetrafluoride:[5]
The major and perhaps only commercial application of zirconium fluoride is as a precursor to ZBLAN glasses.[2]
Mixture of sodium fluoride, zirconium fluoride, and uranium tetrafluoride (53-41-6 mol.%) was used as a coolant in the Aircraft Reactor Experiment. A mixture of lithium fluoride, beryllium fluoride, zirconium fluoride, and uranium-233 tetrafluoride was used in the Molten-Salt Reactor Experiment. (Uranium-233 is used in the thorium fuel cycle reactors.)[citation needed]
Seamless Wikipedia browsing. On steroids.
Every time you click a link to Wikipedia, Wiktionary or Wikiquote in your browser's search results, it will show the modern Wikiwand interface.
Wikiwand extension is a five stars, simple, with minimum permission required to keep your browsing private, safe and transparent.
