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Water-reactive substances [1] are those that spontaneously undergo a chemical reaction with water, often noted as generating flammable gas. [2] Some are highly reducing in nature. [ 3 ] Notable examples include alkali metals , lithium through caesium , and alkaline earth metals , magnesium through barium .
When finely powdered, magnesium reacts with water to produce hydrogen gas: Mg(s) + 2 H 2 O(g) → Mg(OH) 2 (aq) + H 2 (g) + 1203.6 kJ/mol. However, this reaction is much less dramatic than the reactions of the alkali metals with water, because the magnesium hydroxide builds up on the surface of the magnesium metal and inhibits further reaction ...
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 reacts with water to produce magnesium hydroxide: MgO + H 2 O → Mg(OH) 2; Calcium oxide reacts with water to produce calcium hydroxide: CaO + H 2 O → Ca(OH) 2; Strontium oxide reacts with water to produce strontium hydroxide: SrO + H 2 O → Sr(OH) 2; Barium oxide reacts with water to produce barium hydroxide: BaO + H 2 O ...
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 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 .
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.
Magnesium nitrate reacts with alkali metal hydroxide to form the corresponding nitrate: Mg(NO 3) 2 + 2 NaOH → Mg(OH) 2 + 2 NaNO 3.. Since magnesium nitrate has a high affinity for water, heating the hexahydrate does not result in the dehydration of the salt, but rather its decomposition into magnesium oxide, oxygen, and nitrogen oxides: