|Name, Symbol, Number||magnesium, Mg, 12|
|Chemical series||alkaline earth metals|
|Group, Period, Block||2, 3, s|
|Atomic mass||24.3050(6) g/mol|
|Electron configuration||[Ne] 3s2|
|Electrons per shell||2, 8, 2|
|Density (near r.t.)||1.738 g/cm³|
|Liquid density at m.p.||1.584 g/cm³|
|Melting point||923 K
(650 °C, 1202 °F)
|Boiling point||1363 K
(1090 °C, 1994 °F)
|Heat of fusion||8.48 kJ/mol|
|Heat of vaporization||128 kJ/mol|
|Heat capacity||(25 °C) 24.869 J/(mol·K)|
(strongly basic oxide)
|Electronegativity||1.31 (Pauling scale)|
|1st: 737.7 kJ/mol|
|2nd: 1450.7 kJ/mol|
|3rd: 7732.7 kJ/mol|
|Atomic radius||150 pm|
|Atomic radius (calc.)||145 pm|
|Covalent radius||130 pm|
|Van der Waals radius||173 pm|
|Electrical resistivity||(20 °C) 43.9 nΩ·m|
|Thermal conductivity||(300 K) 156 W/(m·K)|
|Thermal expansion||(25 °C) 24.8 µm/(m·K)|
|Speed of sound (thin rod)||(r.t.) (annealed)
|Speed of sound (thin rod)||(r.t.) 45 m/s|
|Shear modulus||17 GPa|
|Bulk modulus||45 GPa|
|Brinell hardness||260 MPa|
|CAS registry number||7439-95-4|
Magnesium (chemical symbol Mg, atomic number 12) is the eighth most abundant chemical element in the Earth's crust, constituting about 2 percent of the crust by weight. It is the third most plentiful element dissolved in seawater. Silvery white in color, it is classified as an alkaline earth metal and is not found as a free metal in nature.
In its ionic form, magnesium is one of the most essential elements for all known living organisms. Its salts, therefore, are used as additives in foods and fertilizers. When alloyed with aluminum, it is widely used to make beverage cans, airplanes, and missiles. The brilliant white light produced by burning magnesium is used in flashlight photography and fireworks. Magnesium oxide is used for lining furnaces, the hydroxide (in the form of "milk of magnesia") is a laxative and antacid, its sulfate (Epsom salt) is used in medicine. Magnesium carbonate is used in brick, flooring, fireproofing, and fire-extinguishing compositions.
The name magnesium originates from the Greek word for a district called Magnesia in Thessaly. The element, which is always combined with other elements in nature, is found in deposits of over 60 minerals. Of these, only dolomite, magnesite, brucite, carnallite, talc, and olivine are of commercial importance.
In England in 1755 Joseph Black recognized magnesium as being an element. In 1808 Sir Humphry Davy electrolytically isolated pure magnesium metal from a mix of magnesia (magnesium oxide, MgO) and mercuric oxide (HgO). French chemist Antoine Bussy described another method of preparing it in 1831.
The United States has traditionally been the major world supplier of this metal, supplying 45 percent of world production even as recently as 1995. Today, the U.S. market share is at 7 percent. As of 2005, China has taken over as the dominant supplier, pegged at 60 percent world market share, which increased from 4 percent in 1995. To isolate the metal, China relies almost completely on what is called the Pidgeon process, in which magnesium oxide is reduced at high temperatures with silicon.
As a member of the series of alkaline earth metals, magnesium lies in group 2 (former group 2A) of the periodic table, between beryllium and calcium. In addition, it is placed in period 3, immediately following sodium.
Elemental magnesium is a fairly strong, lightweight metal (two thirds the density of aluminum). It slightly tarnishes when exposed to air, although unlike the alkaline metals, storage in an oxygen free environment is unnecessary because magnesium is protected by a thin layer of oxide that is fairly impermeable and hard to remove.
Like calcium, magnesium reacts with water at room temperature, although it reacts much more slowly than calcium. When it is submerged in water, hydrogen bubbles begin to form almost unnoticeably on the metal's surface, but the powdered metal reacts much more rapidly. At higher temperatures, the reaction will occur faster (see precautions).
Magnesium is a highly flammable metal that is easy to ignite when powdered or shaved into thin strips. It is, however, difficult to ignite in mass or bulk. Once ignited, it is difficult to extinguish, being able to burn in both nitrogen (forming magnesium nitride), and carbon dioxide (forming magnesium oxide and carbon). It burns at a temperature of approximately 2,500 K (2200 °C, 4000 °F). The autoignition temperature of magnesium is approximately 744 K (473 °C, 883 °F).
When it burns in air, magnesium produces a brilliant white light. This property was applied in the early days of photography, when magnesium powder (flash powder) was used as a source of illumination. Later, magnesium ribbon was used in electrically ignited flash bulbs.
When glowing white at high temperatures, magnesium has many chemical properties that it does not possess at lower temperatures. It also becomes more toxic, but the high temperature alone is extremely dangerous.
Magnesium compounds are typically white crystals. Most are soluble in water, providing the sour-tasting magnesium ion Mg2+. Small amounts of dissolved magnesium ion contributes to the tartness and taste of natural waters. In large amounts, magnesium ion is an ionic laxative. The so-called "milk of magnesia" is a water suspension of one of the few insoluble magnesium compounds, magnesium hydroxide, and it is named after the appearance of the undissolved particles. Milk of magnesia is a mild base.
Three isotopes of magnesium are found in nature: 24Mg, 25Mg, and 26Mg, at abundances of approximately 79%, 10%, and 11%, respectively. All three isotopes are stable.
26Mg has found application in isotopic geology, similar to that of aluminum. 26Mg is a radiogenic daughter product of 26Al, which has a half-life of 717,000 years. Large enrichments of stable 26Mg have been observed in the Ca-Al-rich inclusions of some carbonaceous chondrite meteorites. The anomalous abundance of 26Mg is attributed to the decay of its parent 26Al in the inclusions. Therefore, the meteorite must have formed in the solar nebula before the 26Al had decayed. Hence, these fragments are among the oldest objects in the solar system and have preserved information about its earliest history.
Magnesium ions are essential for the cells of all known living organisms. Many enzymes require the presence of magnesium ions for their catalytic action. Plants have an additional use for magnesium in that chlorophylls contain magnesium. The adult human daily nutritional requirement (which depends on various factors including sex and body size) is 300-400 milligrams (mg) per day.
Too much magnesium in the diet can make it difficult for the human body to absorb calcium. On the other hand, inadequate magnesium intake has been associated with muscle spasms, cardiovascular disease, diabetes, high blood pressure, anxiety disorders, and osteoporosis. Acute deficiency is rare, and is more common as a drug side effect (such as chronic alcohol or diuretic use) than from low food intake per se. The incidence of chronic deficiency, resulting in less than optimal health, is debated.
The Dietary Reference Intake (DRI) upper tolerated limit for supplemental magnesium is 350 mg/day (calculated as mg of Mg elemental in the salt). The most common symptom of excess oral magnesium intake is diarrhea. Given that the kidneys of adult humans excrete excess magnesium efficiently, oral magnesium poisoning in adults with normal renal function, is very rare. Infants have reduced ability to excrete excess magnesium even when healthy, so they should not be given magnesium supplements, except under a physician's care.
Magnesium is present in many foods, but it usually occurs in small amounts. As with most nutrients, daily needs for magnesium cannot be met from a single food. Eating a wide variety of foods, including fruits, vegetables, and plenty of whole grains, helps ensure an adequate intake of magnesium. Green vegetables such as spinach provide magnesium because the center of the chlorophyll molecule contains magnesium. Nuts—especially almonds), seeds, and some whole grains—are also good sources of magnesium.
The magnesium content of refined foods is usually low. Whole-wheat bread, for example, has twice as much magnesium as white bread because the magnesium-rich germ and bran are removed when white flour is processed.
Water can provide magnesium, but the amount varies according to the water supply. "Hard" water contains more magnesium than "soft" water. Dietary surveys do not estimate magnesium intake from water, which may lead to underestimating total magnesium intake and its variability.
The following figures indicate the amount of magnesium in some foods:
Magnesium is the third most commonly used structural metal, following steel and aluminum. In its purest form, magnesium can be compared to aluminum. Like aluminum, it is strong and light. Its principal use is as an alloying additive to aluminum—these aluminum-magnesium alloys, sometimes called magnalium or magnelium, are used mainly for beverage cans.
Magnesium alloy is also used in several high-volume parts manufacturing applications, including automotive and truck components. Specialty, high-grade car wheels of magnesium alloy are called "mag wheels." In 1957, a Corvette SS, designed for racing, was constructed with completely magnesium body panels. Volkswagen has used magnesium in its engine components for many years. For a long time, Porsche used magnesium alloy for its engine blocks, due to the weight advantage.
Recently, there appears to be renewed interest in magnesium engine blocks, as featured in the 2006 BMW 325i and 330i models. The award-winning BMW engine uses an aluminum alloy insert for the cylinder walls and cooling jackets surrounded by a high-temperature magnesium alloy AJ62A. The application of magnesium AE44 alloy in the 2006 Corvette Z06 engine cradle has advanced the technology of designing robust automotive parts in magnesium. Both these alloys are recent developments in high-temperature, low-creep magnesium alloys. New alloy development and lower costs, which are becoming competitive with aluminum, will increase the number of automotive applications.
Magnesium is also used in electronic devices. Given its low weight and good mechanical and electrical properties, it is widely used in the manufacture of mobile phones, laptops, cameras, and so forth.
There are several other uses of magnesium, some of which are listed below.
Pure magnesium metal and its alloys are highly flammable when in the molten state, powdered form, or ribbon form. Burning or molten magnesium metal reacts violently with water. Magnesium powder is an explosive hazard. One should wear safety glasses while working with magnesium. The bright white light (including ultraviolet) produced by burning magnesium can damage the eyes. Water should not be used to extinguish magnesium fires, because it can actually feed the fire, according to the following reaction:
Carbon dioxide fire extinguishers should not be used either, because magnesium can burn in carbon dioxide (forming magnesium oxide, MgO, and carbon). A dry chemical fire extinguisher (Class D) should be used if available, or else the fire should be covered with sand or magnesium foundry flux. An easy way to put out small metal fires is to place a polyethene bag filled with dry sand on top of the fire. The heat of the fire will melt the bag and the sand will flow out onto the fire.
All links retrieved September 4, 2014.
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