Lithium iodide

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Lithium iodide
Lithium iodide
Identifiers
10377-51-2 YesY
17023-24-4 (monohydrate) N
17023-25-5 (dihydrate) N
7790-22-9 (trihydrate) N
ChemSpider 59699 YesY
Jmol 3D model Interactive image
PubChem 66321
  • InChI=1S/HI.Li/h1H;/q;+1/p-1 YesY
    Key: HSZCZNFXUDYRKD-UHFFFAOYSA-M YesY
  • 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 ethanol, propanol, ethanediol, ammonia
Solubility in methanol 3430 g/L (20 °C)
Solubility in acetone 426 g/L (18 °C)
1.955
Thermochemistry
0.381 J/g K or 54.4 J/mol K
75.7 J/mol K
-2.02 kJ/g or −270.48 kJ/mol
-266.9 kJ/mol
Vapor pressure {{{value}}}
Related compounds
Other anions
 Lithium fluoride
Lithium chloride
Lithium bromide
Other cations
 Sodium iodide
Potassium iodide
Rubidium iodide
Caesium 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 YesYN ?)
Infobox references

Lithium iodide, or LiI, is a compound of lithium and iodine. When exposed to air, it becomes yellow in color, due to the 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 an electrolyte for high temperature batteries. It is also used for long life batteries as required, for example, by artificial pacemakers. The solid is used as a phosphor for neutron detection.[6] 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:[7]

RCO2CH3 + LiI + H2O → RCO2H + LiOH + CH3I

Similar reactions apply to epoxides and aziridines.

Lithium iodide was used as a radio contrast agent for X-ray computed tomography imaging studies. Its use was discontinued due to renal toxicity, replaced by organic iodine molecules. Inorganic iodine solutions suffered from hyperosmolarity and high viscosities.[8]

See also

References

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External links

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  1. ↑ Patnaik, Pradyot (2002) Handbook of Inorganic Chemicals. McGraw-Hill, ISBN 0-07-049439-8
  2. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  3. ↑ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  4. ↑ Wietelmann, Ulrich and Bauer, Richard J. (2005) "Lithium and Lithium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH: Weinheim. doi:10.1002/14356007.a15_393.
  5. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  6. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  7. ↑ Charette, André B.; Barbay, J. Kent and He, Wei (2005) "Lithium Iodide" in Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons. doi:10.1002/047084289X.rl121.pub2
  8. ↑ Lua error in package.lua at line 80: module 'strict' not found.
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