Lithium iodide
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| Identifiers | |
|---|---|
10377-51-2  17023-24-4 (monohydrate) 17023-25-5 (dihydrate) 7790-22-9 (trihydrate) | |
| ChemSpider | 59699 |
| |
| Jmol-3D images | Image |
| PubChem | 66321 |
| |
| 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) |
| 151 g/100 mL (0 °C) 167 g/100 mL (25 °C) 433 g/100 mL (100 °C) [1] | |
| Solubility | soluble in ethanol, propanol, ethanediol, ammonia |
| Solubility in methanol | 343 g/100 mL (20 °C) |
| Solubility in acetone | 42.6 g/100 mL (18 °C) |
| Refractive index (nD) |
1.955 |
| Thermochemistry | |
| Specific heat capacity (C) |
0.381 J/g K or 54.4 J/mol K |
| Std molar entropy (S |
75.7 J/mol K |
| Std enthalpy of formation (ΔfH |
-2.02 kJ/g or -270.48 kJ/mol |
| Gibbs free energy (ΔfG˚) |
-266.9 kJ/mol |
| Hazards | |
| MSDS | External MSDS |
| EU Index | Not listed |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions |
Lithium fluoride Lithium chloride Lithium bromide |
| Other cations |
Sodium iodide Potassium iodide Rubidium iodide Caesium iodide |
| Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
verify (what is: / ?) | |
| 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] Various hydrates are also known.[4]
Applications
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.[5] It is also used, in a complex with Iodine, in the electrolyte of dye-sensitized solar cell.
In organic synthesis, LiI is useful for cleaving C-O bonds. For example it can be used to convert methyl esters to carboxylic acids:[6]
- 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 and replaced with organic iodine molecules. Inorganic Iodine solutions suffered from hyperosmolarity and high viscosities.[7]
See also
References
- ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- ↑ "A PDF file from ESPICorp Inc., a supplier of lithium iodide" (PDF). Retrieved 2005-09-16.
- ↑ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ↑ Ulrich Wietelmann, Richard J. Bauer "Lithium and Lithium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH: Weinheim. doi:10.1002/14356007.a15_393.
- ↑ Nicholson, K. P. et al. (1955). "Some lithium iodide phosphors for slow neutron detection". Br. J. Appl. Phys. 6: 104–106. doi:10.1088/0508-3443/6/3/311.
- ↑ André B. Charette, J. Kent Barbay, Wei He "Lithium Iodide" in Encyclopedia of Reagents for Organic Synthesis, 2005, John Wiley & Sons. doi:10.1002/047084289X.rl121.pub2
- ↑ Hrvoje Lusic and Mark W. Grinstaff. X-ray-Computed Tomography Contrast Agents| Chem. Rev. 2013, 113 pp. 1641-1666.
External links
- "Webelements – Lithium Iodide". Retrieved 2005-09-16. -->
- "Composition of LITHIUM IODIDE - NIST". Retrieved 2006-02-03. -->
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