Magnesium

From Free net encyclopedia

Magnesium is the chemical element in the periodic table that has the symbol Mg and atomic number 12 and an atomic mass of 24.31. Magnesium is the eighth most abundant element and constitutes about 2% of the Earth's crust by weight, and it is the third most plentiful element dissolved in seawater. This alkaline earth metal is primarily used as an alloying agent to make aluminium-magnesium alloys, sometimes called "magnalium" or "magnelium".

1 Notable characteristics
2 Applications
3 History
4 Sources
5 Compounds in living organisms
6 Food sources
7 Isotopes
8 Precautions
9 See also
10 External links

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Notable characteristics

Magnesium is a fairly strong, silvery-white, light-weight metal (one third lighter than aluminium) that slightly tarnishes when exposed to air, although unlike the alkaline metals, storage in an oxygen free environment is unnecessary. As a powder, this metal heats and ignites when exposed to moisture and burns with a white flame. It is difficult to ignite in bulk, though it is easy to light if it is shaved into thin strips. Once ignited, it is difficult to extinguish, being able to burn in both nitrogen (forming magnesium nitride), and carbon dioxide (forming magnesium oxide, MgO, and carbon). When a thin ribbon of magnesium metal is ignited and then plunged under water, it continues to burn until the metal ribbon is completely consumed. Magnesium, when it burns in air, produces a brilliant white light. This was used in the early days of photography when magnesium powder was used as a source of illumination (flash powder). Later, magnesium ribbon was used in electrically ignited flash bulbs. Magnesium powder is still used in the manufacture of fireworks and marine flares where a brilliant white light is required.

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Applications

Magnesium compounds, primarily magnesium oxide, are used mainly as refractory material in furnace linings for producing iron, steel, nonferrous metals, glass, and cement. Magnesium oxide and other compounds also are used in agricultural, chemical, and construction industries. As a metal, this element's principal use is as an alloying additive to aluminium with these aluminium-magnesium alloys being used mainly for beverage cans.

Magnesium, in its purest form, can be compared to aluminium, and is strong and light, so it is used in several high volume part 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. However, there is renewed interest in magnesium engine blocks, as featured in the 2006 BMW 325i and 330i models. The award-winning BMW engine uses an aluminium 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 of these alloys are recent developments in high temperature low creep magnesium alloys. New alloy development and lower costs, which are becoming competitive to aluminium, will further the number of automotive applications.

In December 2005, for the first time on record, the automotive grade magnesium alloy price per cm3 dropped below the A380 aluminum alloy price per cm3.

Other uses include:

Removal of sulfur from iron and steel.
Photoengraved plates in the printing industry.
Combined in alloys, this metal is essential for airplane and missile construction.
When used as an alloying agent, this metal improves the mechanical, fabrication and welding characteristics of aluminium.
Additive agent for conventional propellants and used in producing nodular graphite in cast iron.
Reducing agent for the production of pure uranium and other metals from their salts.
Its hydroxide is used in milk of magnesia, its chloride and sulfate in Epsom salts and its citrates in medicine.
Dead-burned magnesite is used for refractory purposes such as brick and liners in furnaces and converters.
Magnesium is also flammable, burning at a temperature of approximately 2500K (2200 °C, 4000 °F).
The extremely high temperature at which magnesium burns makes it a handy tool for starting emergency fires during outdoor recreation.
Magnesium carbonate (MgCO₃) powder is also used by athletes, such as gymnasts and weightlifters, to improve the grip on objects – the apparatus or lifting bar.
Magnesium stearate is a slightly flammable white powder with lubricative properties. In pharmaceutical technology it is used in the manufacturing of tablets, to prevent the tablets from sticking to the equipment during the tablet compression process (i.e., when the tablet's substance is pressed into tablet form).
Other uses include flashlight photography, flares, pyrotechnics,making sparklers, and including incendiary bombs.

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History

Image:MagnesiumMetalUSGOV.jpg The name originates from the Greek word for a district in Thessaly called Magnesia. Joseph Black in England recognized magnesium as being an element in 1755, Sir Humphry Davy electrolytically isolated pure magnesium metal in 1808 from a mix of magnesia and Hg O, and A. A. B. Bussy prepared it in coherent form in 1831. Magnesium is the eighth most abundant element in the earth's crust. It is an alkaline earth metal and therefore does not occur uncombined with other elements. It is found in large deposits of magnesite, dolomite, and other minerals.

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Sources

Although magnesium is found in over 60 minerals, only dolomite, magnesite, brucite, carnallite, talc, and olivine are of commercial importance.

In the United States this metal is principally obtained by electrolysis of fused magnesium chloride from brines, wells, and sea water:

cathode: Mg²⁺ + 2 e^- → Mg

anode: 2 Cl^- → Cl_{2 (gas)} + 2 e^-

The United States has traditionally been the major world supplier of this metal, supplying 45% of world production even as recently as 1995. Today, the US market share is at 7%, with a single domestic producer left, US Magnesium, a company borne from now-defunct Magcorp. As of 2005 China has taken over as the dominant supplier, pegged at 60% world market share, which increased from 4% in 1995. Unlike the above described electrolytic process, China is almost completely reliant on a different method of obtaining the metal from its ores, the silicothermic Pidgeon process.

See also Magnesium minerals.

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Compounds in living organisms

Template:Main Organic magnesium is important in both plant and animal life. Chlorophylls are magnesium-centered porphyrins. The adult daily nutritional requirement, which is affected by various factors including sex, weight and size, is 300-400 mg/day. Many enzymes require the presence of magnesium ions for their catalytic action, especially enzymes utilizing ATP. Inadequate magnesium intake frequently causes muscle spasms, and has been associated with cardiovascular disease, diabetes, high blood pressure, anxiety disorders and osteoporosis. Acute deficiency is rare.

The DRI upper tolerated limit for supplemental magnesium is 350 mg/day. The most common symptom of excess magnesium is diarrhea. Infants should not be given magnesium supplements.

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Food sources

Green vegetables such as spinach provide magnesium because the center of the chlorophyll molecule contains magnesium. Nuts, seeds, and some whole grains are also good sources of magnesium.

Although magnesium is present in many foods, 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 five servings of fruits and vegetables daily and plenty of whole grains, helps to ensure an adequate intake 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. The table of food sources of magnesium suggests many dietary sources of magnesium.

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.

Too much magnesium in the diet can make it difficult for your body to absorb calcium. On the other hand not enough magnesium can lead to irregular heartbeats, high blood pressure, insomnia and muscle spasms.

Following are some foods and the amount of magnesium in them:

spinach (1/2 cup) = 80 milligrams (mg)
peanut butter (2 tablespoons) = 50 mg
black-eyed peas (1/2 cup) = 45 mg
milk, low fat (1 cup) = 40 mg

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Isotopes

²⁶Mg is a stable isotope that has found application in isotopic geology, similar to that of aluminium. 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.

It is conventional to plot ²⁶Mg/²⁴Mg against an Al/Mg ratio. In an isochrone plot, the Al/Mg ratio plotted is²⁷Al/²⁴Mg. The slope of the isochron has no age significance, but indicates the initial ²⁶Al/²⁷Al ratio in the sample at the time when the systems were separated from a common reservoir.

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Precautions

Magnesium metal and alloys are highly flammable in their pure form when molten, as a powder, or in 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 reaction: [1]

Mg _(s) + 2 H₂O _(v) → Mg(OH)₂ _(aq) + H₂ _(g)

or in words:

Magnesium _(solid) + steam → Magnesium hydroxide _(aqueous) + Hydrogen _(gas)

Carbon dioxide fire extinguishers should not be used either, because magnesium can burn in carbon dioxide (forming magnesium oxide, MgO, and carbon)[2]. A Class D dry chemical fire extinguisher should be used if available, or else the fire should be covered with sand. 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.

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