رباعي فلوروبورات الليثيوم
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| الأسماء | |||
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| اسم أيوپاك
Lithium tetrafluoroborate
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| أسماء أخرى
Borate(1-), tetrafluoro-, lithium
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| المُعرِّفات | |||
| رقم CAS | |||
3D model (JSmol)
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| ChemSpider | |||
| ECHA InfoCard | 100.034.692 
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PubChem CID
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| UNII | |||
CompTox Dashboard (EPA)
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| الخصائص | |||
| الصيغة الجزيئية | LiBF4 | ||
| كتلة مولية | 93.746 g/mol | ||
| المظهر | White/grey crystalline solid | ||
| الرائحة | odorless | ||
| الكثافة | 0.852 g/cm3 solid | ||
| نقطة الانصهار | |||
| نقطة الغليان | |||
| قابلية الذوبان في الماء | Very soluble[1] | ||
| المخاطر | |||
| خطر رئيسي | Harmful, causes burns, hygroscopic. | ||
| صفحة بيانات السلامة | External MSDS | ||
| NFPA 704 (معيـَّن النار) | |||
| مركبات ذا علاقة | |||
أنيونات أخرى
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Tetrafluoroborate, | ||
مركـّبات ذات علاقة
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Nitrosyl tetrafluoroborate | ||
ما لم يُذكر غير ذلك، البيانات المعطاة للمواد في حالاتهم العيارية (عند 25 °س [77 °ف]، 100 kPa). | |||
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| مراجع الجدول | |||
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]
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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 Archived 2006-03-16 at the Wayback Machine
- ^ أ ب Xu, Kang. "Nonaqueous Liquid Electrolytes for Lithium-Based Rechargeable Batteries."Chemical Reviews 2004, volume 104, pp. 4303-418. DOI:10.1021/cr030203g
- ^ S. Zhang; K. Xu; T. Jow (2003). "Low-temperature performance of Li-ion cells with a LiBF4-based electrolyte". Journal of Solid State Electrochemistry. 7 (3): 147–151. doi:10.1007/s10008-002-0300-9. S2CID 96775286. Retrieved 16 February 2014.
- ^ S. S. Zhang; z K. Xu & T. R. Jow (2002). "Study of LiBF4 as an Electrolyte Salt for a Li-Ion Battery". Journal of the Electrochemical Society. 149 (5): A586–A590. Bibcode:2002JElS..149A.586Z. doi:10.1149/1.1466857. Retrieved 16 February 2014.
- ^ أ ب ت Robert Brotherton; Joseph Weber; Clarence Guibert & John Little (2000). "Boron Compounds". Ullmann's Encyclopedia of Industrial Chemistry. p. 10. doi:10.1002/14356007.a04_309. ISBN 3527306730.
- ^ Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. New York: Academic Press. p. 773. ISBN 978-0121266011.