nature of magnesium powder in water
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Home Periodic table Elements and water Magnesium in water (Mg + H2O)
Magnesium (Mg) and water
Magnesium and water: reaction mechanisms, environmental impact and health effects.
Magnesium is present in seawater in amounts of about 1300 ppm. After sodium, it is the most commonly found cation in oceans. Rivers contains approximately 4 ppm of magnesium, marine algae 6000-20,000 ppm, and oysters 1200 ppm.
Dutch drinking water contains between 1 and 5 mg of magnesium per liter.
Magnesium and other alkali earth metals are responsible for water hardness. Water containing large amounts of alkali earth ions is called hard water, and water containing low amounts of these ions is called soft water.
Magnesium metals are not affected by water at room temperature. Magnesium generally is a slow-reacting element, but reactivity increases with oxygen levels. Furthermore, magnesium reacts with water vapor to magnesium hydroxide and hydrogen gas:
Mg (s) + 2H2O(g) -> Mg(OH)2(aq) + H2(g)
Magnesium fires cannot be extinguished by water. Magnesium continues to burn after oxygen is depleted. It than reacts with nitrogen from air to form magnesium nitride (Mg3N2). When attempts are made to extinguish magnesium fires with water, magnesium aggressively reacts with hydrogen gas. To prevent any damage, a magnesium fire must be covered in sand.
An example of a magnesium compound is magnesium phosphide (Mg3P2), an odorous, grey solid. When this compound comes in contact with water or moist air, it is decomposed and phosphine (PH3) is formed. This is a toxic compound, and it is also very flammable in air.
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