Lithium tetrafluoroborate
| |||
Names | |||
---|---|---|---|
IUPAC name Lithium tetrafluoroborate | |||
Other names Borate(1-), tetrafluoro-, lithium | |||
Identifiers | |||
CAS Number |
| ||
3D model (JSmol) |
| ||
ChemSpider |
| ||
ECHA InfoCard | 100.034.692 ![]() | ||
PubChem CID |
| ||
UNII |
| ||
CompTox Dashboard (EPA) |
| ||
InChI
| |||
| |||
Properties | |||
Chemical formula | 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 | ||
Solubility in water | Very soluble[1] | ||
Hazards | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards | Harmful, causes burns, hygroscopic. | ||
NFPA 704 (fire diamond) | ![]() 1 0 1 | ||
Safety data sheet (SDS) | External MSDS | ||
Related compounds | |||
Other anions | Tetrafluoroborate, | ||
Related compounds | Nitrosyl tetrafluoroborate | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). ![]() ![]() ![]() 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]
- LiBF4 → LiF + BF3
Production
LiBF4 is a byproduct in the industrial synthesis of diborane:[5][6]
- 8 BF3 + 6 LiH → B2H6 + 6 LiBF4
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
- ^ a b 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.
- ^ a b c 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.
- v
- t
- e
- Li2
- LiAlCl4
- Li1+xAlxGe2−x(PO4)3
- LiAlH4
- LiAlO2
- LiAl1+xTi2−x(PO4)3
- LiAs
- LiAsF6
- Li3AsO4
- LiAt
- Li[AuCl4]
- LiB(C2O4)2
- LiB(C6F5)4
- LiWF6
- LiBF4
- LiBH4
- LiBO2
- LiB3O5
- Li2B4O7
- LiAsF6
- Li2SnF6
- Li2TiF6
- Li2ZrF6
- Li2B4O7·5H2O
- LiBSi2
- LiBr
- LiBr·2H2O
- LiBrO
- LiBrO2
- LiBrO3
- LiBrO4
- Li2C2
- LiCF3SO3
- CH3CH(OH)COOLi
- LiC2H2ClO2
- LiC2H3IO2
- Li(CH3)2N
- LiCHO2
- LiCH3O
- LiC2H5O
- LiCN
- Li2CN2
- LiCNO
- Li2CO3
- Li2C2O4
- LiCl
- LiCl·H2O
- LiClO
- LiFO
- LiClO2
- LiClO3
- LiClO4
- LiCoO2
- Li2CrO4
- Li2CrO4·2H2O
- Li2Cr2O7
- CsLiB6O10
- LiD
- LiF
- Li2F
- LiF4Al
- Li3F6Al
- FLiBe
- LiFePO4
- FLiNaK
- LiGaH4
- Li2GeF6
- Li2GeO3
- LiGe2(PO4)3
- LiH
- LiH2AsO4
- Li2HAsO4
- LiHCO3
- Li3H(CO3)2
- LiH2PO3
- LiH2PO4
- LiHSO3
- LiHSO4
- LiHe
- LiI
- LiIO
- LiIO2
- LiIO3
- LiIO4
- Li2IrO3
- Li7La3Zr2O12
- LiMn2O4
- Li2MoO4
- Li0.9Mo6O17
- LiN3
- Li3N
- LiNH2
- Li2NH
- LiNO2
- LiNO3
- LiNO3·H2O
- Li2N2O2
- LiNa
- Li2NaPO3
- LiNaNO2
- LiNbO3
- Li2NbO3
- LiO−
- LiO2
- LiO3
- Li2O
- Li2O2
- LiOH
- Li3P
- LiPF6
- Li3PO4
- Li2HPO3
- Li2HPO4
- Li3PO3
- Li3PO4
- Li2Po
- Li2PtO3
- Li2RuO3
- Li2S
- LiSCN
- LiSH
- LiSO3F
- Li2SO3
- Li2SO4
- Li[SbF6]
- Li2Se
- Li2SeO3
- Li2SeO4
- LiSi
- Li2SiF6
- Li4SiO4
- Li2SiO3
- Li2Si2O5
- LiTaO3
- Li2Te
- LiTe3
- Li2TeO3
- Li2TeO4
- Li2TiO3
- Li4Ti5O12
- LiTi2(PO4)3
- LiVO3·2H2O
- Li3V2(PO4)3
- Li2WO4
- LiYF4
- LiZr2(PO4)3
- Li2ZrO3
- Hemolithin (extraterrestrial protein)
- Organolithium reagents
- CH3COOLi
- C4H6LiNO4
- LiC2F6NO4S2
- LiN(SiMe3)2
- Li3C6H5O7
- C5H5Li
- LiN(C3H7)2
- (C6H5)2PLi
- C18H35LiO3
- C6H13Li
- C4H9Li
- CH3CHLiCH2CH3
- (CH3)3CLi
- C12H28BLi
- CH3Li
- Li+C10H8−
- C5H11Li
- C5H3LiN2O4
- C6H5Li
- LiC2CH3
- LiO2C(CH2)16CH3
- C4H5LiO4
- LiEt3BH
- LiOC(CH3)3
- C9H18LiN
- LiC2H3 Vinyllithium
- LiC
11H
23COO
- Amblygonite
- Berezanskite
- Brannockite
- Cryolithionite
- Darapiosite
- Darrellhenryite
- Elbaite
- Fluorine Elbaite
- Fluor-liddicoatite
- Emeleusite
- Eucryptite LiAlSiO4
- Faizievite
- Hectorite
- Hsianghualite
- Jadarite LiNaSiB3O7OH
- Keatite Li(AlSi2O6)
- Kunzite
- Lavinskyite
- Lepidolite
- Lithiophilite LiMnPO4
- Lithiophosphate Li3PO4
- Manandonite
- Manganoneptunite
- Nambulite
- Neptunite
- Olympite
- Petalite LiAlSi4010
- Pezzottaite Cs(Be2Li)Al2Si6O18
- Rossmanite
- Saliotite
- Sogdianite
- Spodumene LiAl(SiO3)2
- Sugilite
- Tiptopite
- Tourmaline
- Triphylite LiFePO4
- Zabuyelite Li2CO3
- Zektzerite
- Zinnwaldite
- LixBey
- HLiHe+
- LiFHeO
- LiHe2
- (HeO)(LiF)2
- La2/3-xLi3xTiO3He
- Aluminium–lithium alloys
- Heteroatom-promoted lateral lithiation
- LB buffer
- Lithium atom
- Lithium medication
- LiNixCoyAlzO2
- LiNixMnyCozO2
- Lithium soap
- Lithium Triangle
- Lucifer yellow
- Magnesium–lithium alloys
- NASICON
- Environmentally friendly red light flare
![]() | This electrochemistry-related article is a stub. You can help Wikipedia by expanding it. |
- v
- t
- e