Magnesium iodide is the name for the chemical compounds with the formulas MgI2 and its various hydrates MgI2(H2O)x. These salts are typical ionic halides, being highly soluble in water.
Chemical formula：MgI2 (anhydrous)
Molar mass：278.1139 g/mol (anhydrous)
Appearance：white crystalline solid
Odor：odorless
Density：4.43 g/cm3 (anhydrous solid)
Melting point：637 °C (1,179 °F; 910 K) (anhydrous, decomposes)
Solubility in water：54.7 g/100 cm3 (anhydrous, 0 °C)
Solubility:soluble in ether, alcohol and ammonia
Magnetic susceptibility (χ)：−111.0·10−6 cm3/mol
Organic Synthesis: Magnesium iodide is used in organic chemistry as a reducing agent, especially for deoxygenating compounds. For example, it is useful in the reduction of epoxides to alkenes.
Catalyst: In some cases, MgI₂ is used as a catalyst or a catalyst precursor in specific organic reactions.
Nutritional Supplement: Magnesium and iodine are both essential nutrients. Magnesium iodide may serve as a source of these elements in some supplement formulations, though other compounds are often preferred due to MgI₂’s hygroscopic nature.
Decomposition: Magnesium iodide decomposes upon exposure to air, especially in humid conditions, where it breaks down to magnesium oxide (MgO) and releases iodine (I₂). This decomposition is accelerated by moisture and light.
Storage Conditions: MgI₂ should be stored in airtight containers, ideally in a cool, dry, and dark environment to prevent degradation.
Hazards: Magnesium iodide is relatively safe in small amounts but, like other iodide salts, can cause skin and eye irritation. Inhalation of its dust should be avoided.
Environmental Impact: It should be handled carefully to avoid large-scale environmental exposure, particularly due to iodine’s environmental reactivity.
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