Lithium iodide

Source: Wikipedia, the free encyclopedia.
Lithium iodide
Lithium iodide
__ Li+     __ I−
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.030.735 Edit this at Wikidata
UNII
  • InChI=1S/HI.Li/h1H;/q;+1/p-1 checkY
    Key: HSZCZNFXUDYRKD-UHFFFAOYSA-M checkY
  • InChI=1/HI.Li/h1H;/q;+1/p-1
    Key: HSZCZNFXUDYRKD-REWHXWOFAM
  • [Li+].[I-]
Properties
LiI
Molar mass 133.85 g/mol
Appearance White crystalline solid
Density 4.076 g/cm3 (anhydrous)
3.494 g/cm3 (trihydrate)
Melting point 469 °C (876 °F; 742 K)
Boiling point 1,171 °C (2,140 °F; 1,444 K)
1510 g/L (0 °C)
1670 g/L (25 °C)
4330 g/L (100 °C) [1]
Solubility soluble in
ethanediol, ammonia
Solubility in methanol 3430 g/L (20 °C)
Solubility in acetone 426 g/L (18 °C)
−50.0·10−6 cm3/mol
1.955
Thermochemistry
0.381 J/g K or 54.4 J/mol K
75.7 J/mol K
Std enthalpy of
formation
(ΔfH⦵298)
 -2.02 kJ/g or −270.48 kJ/mol
-266.9 kJ/mol
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point Non-flammable
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
 Lithium fluoride
Lithium chloride
Lithium bromide
Lithium astatide
Other cations
Francium iodide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Lithium iodide, or LiI, is a

oxidation of iodide to iodine.[2] It crystallizes in the NaCl motif.[3] It can participate in various hydrates.[4]

Applications

LiI chains grown inside double-wall carbon nanotubes.[5]

Lithium iodide is used as a

artificial pacemakers[6] due to the long cycle life it enables.[7] The solid is used as a phosphor for neutron detection.[8] It is also used, in a complex with Iodine, in the electrolyte of dye-sensitized solar cells
.

In organic synthesis, LiI is useful for cleaving C-O bonds. For example, it can be used to convert methyl esters to carboxylic acids:[9]

RCO2CH3 + LiI → RCO2Li + CH3I

Similar reactions apply to epoxides and aziridines.

Lithium iodide was used as a

organoiodine compounds.[10]

See also

References

  1. ISBN 0-07-049439-8
  2. ^ "Lithium iodide" (PDF). ESPI Corp. MSDS. Archived from the original (PDF) on 2008-03-09. Retrieved 2005-09-16.
  3. ISBN 0-19-855370-6
    .
  4. doi:10.1002/14356007.a15_393
    .
  5. PMID 26228378
    .
  6. S2CID 138189063
    .
  7. ^ Hanif, Maryam (2008). "The Pacemaker Battery - Review Article". UIC Bioengineering Student Journal.
  8. doi:10.1088/0508-3443/6/3/311
    .
  9. doi:10.1002/047084289X.rl121.pub2
  10. PMID 23210836
    .

External links

Wikimedia Commons has media related to Lithium iodide.
Retrieved from "https://en.wikipedia.org/w/index.php?title=Lithium_iodide&oldid=1190439179"