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Line 53: }} }} '''Lithium tetrafluoroborate''' is an ] with the formula ]]. 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.<ref name=Kang>Xu, Kang. "Nonaqueous Liquid Electrolytes for Lithium-Based Rechargeable Batteries."Chemical Reviews 2004, volume 104, pp. 4303-418. doi|10.1021/cr030203g}}</ref>   '''Lithium tetrafluoroborate''' is a chemical compound with the formula LiBF<sub>4</sub>. It can be dissolved in ], ], and/or ] for use as an ] in ].   ==Applications== LiBFAlthough BF<sub>4</sub>- ishas usedhigh asionic mobility, solutions of its Li<sup>+</sup> salt are less conductive than other less associated salts.<ref name=Kang/> As an ] in ]. Using, LiBF<sub>4</sub> insteadoffers ofsome advantages relative to the more common ]. salt isIt advantageousexhibits ingreater somethermal applications due to its relative tolerance of temperature extremesstability.<ref>{{cite journal|last=S. Zhang, K. Xu, T. Jow|title=Low-temperature performance of Li-ion cells with a LiBF4-based electrolyte|journal=Journal of Solid State Electrochemistry|year=2003|volume=7|issue=3|pages=147–151|doi=10.1007/s10008-002-0300-9|url=http://www.researchgate.net/publication/241026936_061._Low-temperature_performance_of_Li-ion_cells_with_a_LiBF_4_-based_electrolyte/file/5046351d38dc83bb9b.pdf|accessdate=16 February 2014}}</ref> and moisture.<ref>{{cite journal|last=S. S. Zhang;z K. Xu; and T. R. Jow|title=Study of LiBF4 as an Electrolyte Salt for a Li-Ion Battery|journal=Journal of The Electrochemical Society|year=2002|volume=149|issue=5|pages=A586-A590|doi=10.1149/1.1466857|url=http://www.researchgate.net/publication/244478865_044._Study_of_LiBF_4_as_an_Electrolyte_Salt_for_a_Li-Ion_Battery/file/5046351d3a44c137d3.pdf.|accessdate=16 February 2014}}</ref> For example LiBF<sub>4</sub> can tolerate a moisture content up to 620 ] at room temperature whereas LiPF<sub>6</sub> readily hydrolyzes into toxic ] and ] gases, often destroying the battery's ] materials. Disadvantages of the electrolyte include a relatively low conductivity and difficulties forming a stable solid electrolyte interface with ] electrodes.▼   ==Thermal stability== ▲LiBF<sub>4</sub> is used as an ] in ]. Using LiBF<sub>4</sub> instead of the more common ] salt is advantageous in some applications due to its relative tolerance of temperature extremes<ref>{{cite journal|last=S. Zhang, K. Xu, T. Jow|title=Low-temperature performance of Li-ion cells with a LiBF4-based electrolyte|journal=Journal of Solid State Electrochemistry|year=2003|volume=7|issue=3|pages=147–151|doi=10.1007/s10008-002-0300-9|url=http://www.researchgate.net/publication/241026936_061._Low-temperature_performance_of_Li-ion_cells_with_a_LiBF_4_-based_electrolyte/file/5046351d38dc83bb9b.pdf|accessdate=16 February 2014}}</ref> and moisture.<ref>{{cite journal|last=S. S. Zhang;z K. Xu; and T. R. Jow|title=Study of LiBF4 as an Electrolyte Salt for a Li-Ion Battery|journal=Journal of The Electrochemical Society|year=2002|volume=149|issue=5|pages=A586-A590|doi=10.1149/1.1466857|url=http://www.researchgate.net/publication/244478865_044._Study_of_LiBF_4_as_an_Electrolyte_Salt_for_a_Li-Ion_Battery/file/5046351d3a44c137d3.pdf.|accessdate=16 February 2014}}</ref> For example LiBF<sub>4</sub> can tolerate a moisture content up to 620 ] at room temperature whereas LiPF<sub>6</sub> readily hydrolyzes into toxic ] and ] gases, often destroying the battery's ] materials. Disadvantages of the electrolyte include a relatively low conductivity and difficulties forming a stable solid electrolyte interface with ] electrodes.   Because LiBF<sub>4</sub> and other ] salts thermally decompose to evolve ], the salt is commonly used as a convenient source of the chemical at the laboratory scale:<ref name="Ullmann">{{cite journal|last=Robert, Brotherton; Joseph, Weber; Clarence, Guibert; and John, Little|title=Boron Compounds|year=2000|journal=Ullmann's Encyclopedia of Industrial Chemistry|page=pg. 10|doi=10.1002/14356007.a04_309|accessdate=16 February 2014}}</ref>   Line 68 ⟶ 67: :8 BF<sub>3</sub> + 6 ] → ] + 6 LiBF<sub>4</sub>   LiBF<sub>4</sub> can also be synthesized from LiF and BF<sub>3</sub> in an appropriate solvent (e.g., HF], ], or liquified ]) .<ref name="Ullmann" />; the solvent has to be resistant to fluorination by the BF<sub>3</sub>.   : LiF + BF<sub>3</sub> → LiBF<sub>4</sub>

Revision as of 00:25, 7 October 2014

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 Edit this at Wikidata
PubChem CID
CompTox Dashboard (EPA)
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)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
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). checkY verify (what is  ?) Infobox references
Chemical compound

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.

Applications

Although BF4- has high ionic mobility, solutions of its Li salt are less conductive than other less associated salts. As an electrolyte in Lithium-ion batteries, LiBF4 offers some advantages relative to the more common LiPF6. It exhibits greater thermal stability. 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.

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:

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., hydrogen fluoride, BrF3, or liquified SO2.; the solvent has to be resistant to fluorination by the BF3.

LiF + BF3 → LiBF4

References

  1. GFS-CHEMICALS
  2. ^ Xu, Kang. "Nonaqueous Liquid Electrolytes for Lithium-Based Rechargeable Batteries."Chemical Reviews 2004, volume 104, pp. 4303-418. doi|10.1021/cr030203g}}
  3. 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)
  4. 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)
  5. ^ 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)
  6. Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. Newyork: Academic Press. p. 773. ISBN 978-0121266011.
Lithium compounds (list)
Inorganic (list)
Organic (soaps)
Minerals
Hypothetical
Other Li-related


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