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Magnesium reacts with nitrogen in the solid state if it is powdered and heated to just below the melting point, forming Magnesium nitride Mg 3 N 2. [22] Magnesium reacts with water at room temperature, though it reacts much more slowly than calcium, a similar group 2 metal. [20]
Magnesium has a mild reaction with cold water. The reaction is short-lived because the magnesium hydroxide layer formed on the magnesium is almost insoluble in water and prevents further reaction. Mg(s) + 2H 2 O(l) Mg(OH) 2 (s) + H 2 (g) [11] A metal reacting with cold water will produce a metal hydroxide and hydrogen gas.
Magnesium nitride reacts with water to produce magnesium hydroxide and ammonia gas, as do many metal nitrides.. Mg 3 N 2 (s) + 6 H 2 O(l) → 3 Mg(OH) 2 (aq) + 2 NH 3 (g). In fact, when magnesium is burned in air, some magnesium nitride is formed in addition to the principal product, magnesium oxide.
Magnesium oxide (Mg O), or magnesia, is a white hygroscopic solid mineral that occurs naturally as periclase and is a source of magnesium (see also oxide). It has an empirical formula of MgO and consists of a lattice of Mg 2+ ions and O 2− ions held together by ionic bonding .
Magnesium hydroxide is an inorganic compound with the chemical formula Mg(OH) 2. It occurs in nature as the mineral brucite. It is a white solid with low solubility in water (K sp = 5.61 × 10 −12). [5] Magnesium hydroxide is a common component of antacids, such as milk of magnesia.
Magnesium chloride is an ionic compound, which can be electrolysed in a molten state to form magnesium and chlorine gas. The properties of magnesium bromide and magnesium iodide are similar. [ citation needed ] HMgX (X=Cl,Br,I) can be obtained by reacting the corresponding magnesium halide with magnesium hydride.
Magnesium sulfate or magnesium sulphate is a chemical compound, a salt with the formula MgSO 4, consisting of magnesium cations Mg 2+ (20.19% by mass) and sulfate anions SO 2− 4. It is a white crystalline solid , soluble in water but not in ethanol .
The magnesium oxide can also react with water to form the hydroxide, which, being poorly soluble, would coat the oxide grains and stop further hydration. The acidity provided by hydrolysis of the cations in solution dissolves this coating, and thus allows the process to run continuously until one of the reagents is exhausted.