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Lithium tetrafluoroborate

Names
IUPAC name Lithium tetrafluoroborate
Other names Borate(1-), tetrafluoro-, lithium
Identifiers
CAS Number	14283-07-9
3D model (JSmol)	Interactive image
ChemSpider	3504162
ECHA InfoCard	100.034.692
PubChem CID	4298216
CompTox Dashboard (EPA)	DTXSID00884741
InChI InChI=1S/BF4.Li/c2-1(3,4)5;/q-1;+1Key: UFXJWFBILHTTET-UHFFFAOYSA-N InChI=1/BF4.Li/c2-1(3,4)5;/q-1;+1Key: UFXJWFBILHTTET-UHFFFAOYAL
SMILES .F(F)(F)F
Properties
Chemical formula	LiBF4
Molar mass	93.746 g/mol
Appearance	White/grey crystalline solid
Odor	odorless
Density	0.852 g/cm solid
Melting point	296.5 °C
Boiling point	decomp
Solubility in water	Very soluble
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Harmful, causes burns, hygroscopic.
NFPA 704 (fire diamond)	1 0 1
Related compounds
Other anions	Tetrafluoroborate,
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Y verify (what is  ?) Infobox references

Lithium tetrafluoroborate is a chemical compound with the formula LiBF₄. It can be dissolved in propylene carbonate, dimethoxyethane, and/or gamma-butyrolactone for use as an electrolyte in Lithium-ion batteries.

Applications

LiBF₄ is used as an electrolyte in Lithium-ion batteries. Using LiBF₄ instead of the more common LiPF₆ salt is advantageous in some applications due to its relative tolerance of temperature extremes and moisture. 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.

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:

LiBF₄ → LiF + BF₃

Production

LiBF₄ is a byproduct in the industrial synthesis of diborane:

8 BF₃ + 6 LiH → B₂H₆ + 6 LiBF₄

LiBF₄ can also be synthesized from LiF and BF₃ in an appropriate solvent (e.g. HF, BrF₃, or liquified SO₂) ; the solvent has to be resistant to fluorination by the BF₃.

LiF + BF₃ → LiBF₄

References

1. GFS-CHEMICALS
2. S. Zhang, K. Xu, T. Jow (2003). "Low-temperature performance of Li-ion cells with a LiBF4-based electrolyte" (PDF). Journal of Solid State Electrochemistry. 7 (3): 147–151. doi:10.1007/s10008-002-0300-9. Retrieved 16 February 2014.{{cite journal}}: CS1 maint: multiple names: authors list (link)
3. S. S. Zhang;z K. Xu; and 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. doi:10.1149/1.1466857. Retrieved 16 February 2014.{{cite journal}}: CS1 maint: multiple names: authors list (link)
4. ^ Robert, Brotherton; Joseph, Weber; Clarence, Guibert; and John, Little (2000). "Boron Compounds". Ullmann's Encyclopedia of Industrial Chemistry: pg. 10. doi:10.1002/14356007.a04_309. {{cite journal}}: |access-date= requires |url= (help); |page= has extra text (help)CS1 maint: multiple names: authors list (link)
5. Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. Newyork: Academic Press. p. 773. ISBN 978-0121266011.

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