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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.
It produces intense, bright, white light when it burns. Once ignited, magnesium fires are difficult to extinguish, because combustion continues in nitrogen (forming magnesium nitride), carbon dioxide (forming magnesium oxide and carbon), and water (forming magnesium oxide and hydrogen).
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 .
Magnesium: Colorless due to Magnesium Oxide layer, but burning Mg metal gives an intense white: Mn(II) Manganese(II) Yellowish green: Mo Molybdenum: Yellowish green: Na Sodium: Bright yellow; invisible through cobalt blue glass. See also Sodium-vapor lamp: Nb Niobium: Green or blue Ni Nickel: Colorless to silver-white P Phosphorus: Pale blue ...
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]
The creation of sparks from metals is based on the pyrophoricity of small metal particles, and pyrophoric alloys are made for this purpose. [2] Practical applications include the sparking mechanisms in lighters and various toys, using ferrocerium; starting fires without matches, using a firesteel; the flintlock mechanism in firearms; and spark testing ferrous metals.
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 .
Reaction with nitrogen. Only Be and Mg form nitrides directly. 3Be + N 2 → Be 3 N 2 3Mg + N 2 → Mg 3 N 2. Reaction with hydrogen. Alkaline earth metals react with hydrogen to generate saline hydride that are unstable in water. Ca + H 2 → CaH 2. Reaction with water. Ca, Sr, and Ba readily react with water to form hydroxide and hydrogen gas.