What Is Lithium Iodide?
Lithium iodide, with the chemical formula LiI, is an inorganic compound and an iodide of lithium. It appears as a white to light yellowish-brown crystalline substance.
It is produced through reactions involving lithium carbonate and hydroiodic acid or by introducing hydrogen iodide gas into a lithium carbonate slurry.
Uses of Lithium Iodide
1. Catalyst
Used as a catalyst in acetic acid production, lithium iodide helps control the formation of hydrogen iodide in the reaction medium.
2. Batteries
In lithium batteries, lithium iodide serves as an inorganic solid electrolyte, enhancing battery safety through its self-healing properties. This makes it especially valuable in pacemakers.
3. Other Uses
Its applications extend to absorption refrigerators, dye-sensitized solar cells, electronic materials, and neutron-detection phosphors.
Properties of Lithium Iodide
With a molecular weight of 133.85 and a melting point of 446°C, lithium iodide is soluble in water and ethanol, deliquescent, and may alter under light exposure. It is stable under normal conditions but can decompose into hazardous halides and metal oxides.
Other Information on Lithium Iodide
1. Handling Methods
Recommended safety measures include local exhaust ventilation, safety showers, and protective gear to prevent dust exposure. Eating, drinking, and smoking should be avoided during handling.
2. First Aid Measures
First aid measures include seeking fresh air for inhalation exposure, washing with soap and water for skin contact, flushing eyes with water, and rinsing the mouth if swallowed. Immediate medical attention is advised if symptoms persist.
3. Fire Precautions
In case of fire, use appropriate extinguishing media and wear protective equipment due to potential toxic fumes.
4. Storage Methods
Store in a tightly closed, light-shielded container in a cool environment, preferably refrigerated and away from direct sunlight and moisture.
5. Crystal Structure
Lithium iodide has a NaCl-type structure, contributing to its use in pacemaker batteries since 1972 due to its ion conductivity and polarization properties.