Lithium tetrafluoroborate
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| Names | |||
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| IUPAC name
Lithium tetrafluoroborate
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| Other names
Borate(1-), tetrafluoro-, lithium
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| Identifiers | |||
14283-07-9  |
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| ChemSpider | 3504162 |
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| Jmol 3D model | Interactive image | ||
| PubChem | 4298216 | ||
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| Properties | |||
| LiBF4 | |||
| Molar mass | 93.746 g/mol | ||
| Appearance | White/grey crystalline solid | ||
| Odor | odorless | ||
| Density | 0.852 g/cm3 solid | ||
| Melting point | 296.5 °C (565.7 °F; 569.6 K) | ||
| Boiling point | decomposes | ||
| Very soluble[1] | |||
| Vapor pressure | {{{value}}} | ||
| Related compounds | |||
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Other anions
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Tetrafluoroborate, | ||
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Related compounds
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Nitrosyl tetrafluoroborate | ||
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |||
Lithium tetrafluoroborate is an inorganic compound with the formula LiBF4. It is a white crystalline powder. It has been extensively tested for use in commercial secondary batteries, an application that exploits its high solubility in nonpolar solvents.[2]
Applications
Although BF4− has high ionic mobility, solutions of its Li+ salt are less conductive than other less associated salts.[2] As an electrolyte in Lithium-ion batteries, LiBF4 offers some advantages relative to the more common LiPF6. It exhibits greater thermal stability[3] and moisture tolerance.[4] For example LiBF4 can tolerate a moisture content up to 620 ppm at room temperature whereas LiPF6 readily hydrolyzes into toxic POF3 and HF gases, often destroying the battery's electrode materials. Disadvantages of the electrolyte include a relatively low conductivity and difficulties forming a stable solid electrolyte interface with graphite electrodes.
Thermal stability
Because LiBF4 and other alkali-metal salts thermally decompose to evolve boron trifluoride, the salt is commonly used as a convenient source of the chemical at the laboratory scale:[5]
Production
LiBF4 is a byproduct in the industrial synthesis of diborane:[5][6]
LiBF4 can also be synthesized from LiF and BF3 in an appropriate solvent that is resistant to fluorination by BF3 (e.g. HF, BrF3, or liquified SO2):[5]
- LiF + BF3 → LiBF4
References
- ↑ GFS-CHEMICALS
- ↑ 2.0 2.1 Xu, Kang. "Nonaqueous Liquid Electrolytes for Lithium-Based Rechargeable Batteries."Chemical Reviews 2004, volume 104, pp. 4303-418. doi:10.1021/cr030203g
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