-fluorid.png) | |
| Names | |
|---|---|
| IUPAC names Zirconium(IV) fluoride Zirconium tetrafluoride | |
| Identifiers | |
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3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.029.107 |
| EC Number |
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| UNII | |
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| 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 | |
| GHS labelling: | |
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| Danger | |
| H314 | |
| P260,P264,P280,P301+P330+P331,P302+P361+P354,P304+P340,P305+P354+P338,P316,P321,P363,P405,P501 | |
| 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 | |
Otheranions | Zirconium(IV) chloride Zirconium(IV) bromide Zirconium(IV) iodide |
Othercations | Titanium(IV) fluoride Hafnium(IV) fluoride |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Zirconium(IV) fluoride describes members of a familyinorganic compounds with the formulaZrF4(H2O)x. All are colorless, diamagnetic solids. Anhydrous Zirconium(IV) fluoride is a component ofZBLANfluoride glass.[2]
Three crystalline phases of ZrF4 have been reported, the stable β phase (monoclinic,space group I2/c) , α (tetragonal, space group P42/m) which is a high-temperaturemeta-stable form that can be stabilized by quenching. The γ-form (monoclinic,space group P21/c) is a high-pressure phase, forming at pressures between (4-8 GPa)[3]. α and γ phases are unstable and transform into the β phase at 400[4] and 723°C[3] respectively. There also exists an amorphous phase[3].
Zirconium(IV) fluoride forms several hydrates. The trihydrate has the structure(μ−F)2[ZrF3(H2O)3]2.[5]
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 solidammonium bifluoride to give the heptafluorozirconate salt, which can be converted to the tetrafluoride at 500 °C:
Addition of hydrofluoric acid to solutions ofzirconium nitrate precipitates solid monohydrate. Hydrates of zirconium tetrafluoride can be dehydrated by heating under a stream of hydrogen fluoride.
Zirconium fluoride can be purified bydistillation orsublimation.[2]
Zirconium fluoride forms double salts with otherfluorides. The most prominent ispotassium hexafluorozirconate, formed by fusion of potassium fluoride and zirconium tetrafluoride:[6]
The major and perhaps only commercial application of zirconium fluoride is as a precursor to ZBLAN glasses.[2]
Mixture of sodium fluoride, zirconium fluoride, anduranium tetrafluoride (53-41-6 mol.%) was used as a coolant in theAircraft Reactor Experiment. A mixture oflithium fluoride,beryllium fluoride, zirconium fluoride, anduranium-233 tetrafluoride was used in theMolten-Salt Reactor Experiment. (Uranium-233 is used in thethorium fuel cycle reactors.)[citation needed]
