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[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
Magnesium iodide is stable at high heat under a hydrogen atmosphere, but decomposes in air at normal temperatures, turning brown from the release of elemental iodine. When heated in air, it decomposes completely to magnesium oxide. [4] Another method to prepare MgI 2 is mixing powdered elemental iodine and magnesium metal.
The most common Lewis bases are anions. The strength of Lewis basicity correlates with the pK a of the parent acid: acids with high pK a 's give good Lewis bases. As usual, a weaker acid has a stronger conjugate base. Examples of Lewis bases based on the general definition of electron pair donor include: simple anions, such as H − and F −
Magnesium fluoride is an ionically bonded inorganic compound with the formula Mg F 2. The compound is a colorless to white crystalline salt and is transparent over a wide range of wavelengths , with commercial uses in optics that are also used in space telescopes .
Magnesium bromide can be synthesized by treating magnesium oxide (and related basic salts) with hydrobromic acid. [3] It can also be made by reacting magnesium carbonate and hydrobromic acids, and collecting the solid left after evaporation. [2] As suggested by its easy conversion to various hydrates, anhydrous MgBr 2 is a Lewis acid.
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