Magnesium is a common chemical element found in the earth’s crust and seawater. It is used in truck and automobile components and is highly reactive, flammable, and difficult to extinguish once ignited. Humans require magnesium for over 300 biochemical reactions, and plants require it for photosynthesis. Magnesium salts have many uses, including as a drying agent and plant fertilizer.
Magnesium is a chemical element required by all living cells of all known organisms. When the elements in the earth’s crust are measured by mass, magnesium is the eighth most common. In seawater, it is the third most common. The properties of magnesium lead to its use in truck and automobile components, such as magnetic wheels. The name of magnesium comes from the ancient Greek district of Magnesia.
The symbol for magnesium is Mg and this element, uncombined, does not occur naturally on Earth. It forms a metal and is part of a group known as the alkaline earth metals, elements of the periodic table that make up group 2. The properties of metallic magnesium are that it is very reactive and highly flammable when in fine strip or powder form, but not Randomly.
Magnesium fires are difficult to extinguish once ignited, as they can burn in both nitrogen and carbon dioxide. Water cannot be used, as the magnesium reacts with it to form hydrogen gas, which is highly flammable. The only way to extinguish this type of fire is to smother it in sand or use a dry chemical fire extinguisher. This property of magnesium led to its use in bombing of cities in World War II.
The powder formed from magnesium is used in marine rockets and for the manufacture of pyrotechnic articles. It was used to create bright white light in the early days of photography. The temperature of magnesium flames can reach 2500°F (1,371°C). There are numerous other practical uses for this metal, including combining it in alloys with zinc, aluminum or manganese to make aerospace components, racing bicycles and rockets.
Humans require magnesium for over 300 biochemical reactions, including those that produce DNA and RNA. Deficiency in the human diet is relatively common and can lead to diseases such as osteoporosis and asthma. About half of the body’s magnesium is found in bones. Leafy green vegetables are a good dietary source of magnesium. Other sources include grains, coffee, cocoa, tea, nuts and spices.
Magnesium has an atomic mass of 24.3 and is number 12 in the period table. The physical properties of magnesium include a melting point of 1202°F (650°C) and a boiling point of 1994°F (1091°C). This high melting point causes magnesium to remain solid in fires. Its crystals are hexagonal. The density is 1.74 g/cm3, which is low compared to other metals, such as aluminum.
The chemical properties of magnesium include the tendency to react with halogens, such as chlorine, to form ionic salts. Magnesium has two electrons in its outer shell, which gives it an oxidation state of +2. The loss of these two electrons to form a stable ionic compound is energetically beneficial, so magnesium is generally found as a salt. This reaction is that of magnesium with chlorine in sea water to form MgCl2.
Magnesium salts have many uses, especially magnesium sulfate, MgSO4. The properties of magnesium sulfate include a tendency to absorb water from the air. This makes it useful as a drying agent. Such magnesium sulfate is known as anhydrous or water-free.
Magnesium sulfate that occurs naturally in mineral deposits and used medicinally is in hydrated form, meaning it is associated with water molecules. For example, Epsom salt is MgSO4.7H2O. A significant medical use has been to reduce eclampsia in pregnant women. In rare cases, excessive consumption of magnesium from laxatives and antacids can be toxic.
Plants require magnesium, because it is at the heart of the chlorophyll molecules used in photosynthesis. To ensure that plants get enough of this element, magnesium sulfate is often used as a plant fertilizer. Magnesium sulfate’s high solubility gives it an advantage over other types of magnesium fertilizers.
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