Magnesium

2007 Schools Wikipedia Selection. Related subjects: Chemical elements

12 sodium ← magnesium → aluminium Be ↑ Mg ↓ Ca Periodic Table - Extended Periodic Table
General
Name, Symbol, Number	magnesium, Mg, 12
Chemical series	alkaline earth metals
Group, Period, Block	2, 3, s
Appearance	silvery white
Atomic mass	24.3050 (6) g/mol
Electron configuration	[Ne] 3s2
Electrons per shell	2, 8, 2
Physical properties
Phase	solid
Density (near r.t.)	1.738 g·cm−3
Liquid density at m.p.	1.584 g·cm−3
Melting point	923  K (650 ° C, 1202 ° F)
Boiling point	1363 K (1090 ° C, 1994 ° F)
Heat of fusion	8.48 kJ·mol−1
Heat of vaporization	128 kJ·mol−1
Heat capacity	(25 °C) 24.869 J·mol−1·K−1
Vapor pressure P/Pa 1 10 100 1 k 10 k 100 k at T/K 701 773 861 971 1132 1361
Atomic properties
Crystal structure	hexagonal
Oxidation states	2 (strongly basic oxide)
Electronegativity	1.31 (Pauling scale)
Ionization energies ( more)	1st: 737.7 kJ·mol−1
	2nd: 1450.7 kJ·mol−1
	3rd: 7732.7 kJ·mol−1
Atomic radius	150 pm
Atomic radius (calc.)	145 pm
Covalent radius	130 pm
Van der Waals radius	173 pm
Miscellaneous
Magnetic ordering	paramagnetic
Electrical resistivity	(20 °C) 43.9 nΩ·m
Thermal conductivity	(300 K) 156 W·m−1·K−1
Thermal expansion	(25 °C) 24.8 µm·m−1·K−1
Speed of sound (thin rod)	( r.t.) (annealed) 4940   m·s−1
Young's modulus	45 GPa
Shear modulus	17 GPa
Bulk modulus	45 GPa
Poisson ratio	0.29
Mohs hardness	2.5
Brinell hardness	260 MPa
CAS registry number	7439-95-4
Selected isotopes
Main article: Isotopes of magnesium iso NA half-life DM DE ( MeV) DP 24Mg 78.99% Mg is stable with 12 neutrons 25Mg 10% Mg is stable with 13 neutrons 26Mg 11.01% Mg is stable with 14 neutrons
References

Magnesium ( IPA: /magˈniːziəm, -ʒəm/) 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. Magnesium ion is essential to all living cells. The free element (metal) is not found in nature. Once produced from magnesium salts, this alkaline earth metal is primarily used as an alloying agent to make aluminium-magnesium alloys, sometimes called "magnalium" or "magnelium".

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 it early history.

It is conventional to plot ²⁶Mg/²⁴Mg against an Al/Mg ratio. In an isochron dating 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.

Notable characteristics of element and compounds

Elemental magnesium is a fairly strong, silvery-white, light-weight metal (two thirds the density of aluminium). 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 which is fairly impermeable and hard to remove. Like its lower periodic table group neighbour calcium, magnesium reacts with water at room temperature, though it reacts much more slowly than calcium. When it is submerged in water hydrogen bubbles will almost unnoticably begin to form on the surface of the metal, though if powdered it will react much more rapidly. The reaction will occur faster with higher temperatures (see precautions). Magnesium is a highly flammable metal, but while it is easy to ignite when powdered or shaved into thin strips, it is 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).

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.

Magnesium, when glowing white, has many chemical properties that it does not possess at lower temperatures. It also becomes more toxic, although this is of little practical import, because the high temperature alone generally prevents human contact.

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. Magnesium ion in large amounts is an ionic laxitive, and magnesium sulfate ( Epsom salts) is sometimes used for this purpose. So-called " milk of magnesia" is a water suspension of one of the few insoluble magnesium compounds, magnesium hydroxide; the undissolved particles give rise to its appearance and name. Milk of magnesia is a mild base, and is commonly used as an antacid.

History

The name originates from the Greek word for a district in Thessaly called Magnesia. Joseph Black in Scotland recognized magnesium as being an element in 1755, Sir Humphry Davy electrolytically isolated pure magnesium metal in 1808 from a mix of magnesia and HgO, 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.

Compounds in living organisms

Magnesium ion is essential to the basic nucleic acid chemistry of life, and thus is essential to all cells of all known living organisms. Plants have an additional use for magnesium in that chlorophylls are magnesium-centered porphyrins. Many enzymes require the presence of magnesium ions for their catalytic action, especially enzymes utilizing ATP, or those which use other nucleotides to synthesize DNA and RNA.

Magnesium deficiency in humans was first described in the medical literature in 1934. The adult human daily nutritional requirement, which is affected by various factors including sex, weight and size, is 300-400 mg/day. Inadequate magnesium intake frequently causes muscle spasms, and has been associated with cardiovascular disease, diabetes, high blood pressure, anxiety disorders and osteoporosis. Acute deficiency (see hypomagnesemia) 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 DRI upper tolerated limit for supplemental magnesium is 350 mg/day (calculated as mg of Mg elemental in the salt). (Supplements based on Amino Acid Chelates, Glycinate, Lysinate etc. are much better tolerated by the digestive system and do not have the side effects of the older compounds used.) The most common symptom of excess oral magnesium intake is diarrhea. Since the kidneys of adult humans excrete excess magnesium efficiently, oral magnesium poisoning in adults with normal renal function, is very rare. Infants, which have less ability to excrete excess magnesium even when healthy, should not be given magnesium supplements, except under a physician's care.

Magnesium salts (usually in the form of magnesium sulfate or chloride when given parenterally) are used therapeutically for a number of medical conditions, especially the hypertension of eclampsia. See epsom salts for a list of conditions which have been treated with supplemental magnesium ion. Magnesium is absorbed with reasonable efficiently (30% to 40%) by the body from any soluble magnesium salt, such as the chloride or citrate. Magnesium is similarly absorbed from epsom salts, although the sulfate in these salts adds to their laxative effect at higher doses. Magnesium absorption from the insoluble oxide and hydroxide salts ( milk of magnesia) is erratic and of poorer efficiency, since it depends on the neutralization and solution of the salt by the acid of the stomach, which may not be (and usually is not), complete.

Applications

As the metal

Magnesium is the third most commonly used structural metal, following steel and aluminium.

Products made of magnesium: firestarter and shavings, sharpener, magnesium band

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. The general strategy for such alloys is to form intermetallic precipitates at the grain boundaries, for example by adding mischmetal or calcium . 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 aluminium alloy price per cm³.

The second application field of magnesium is electronic devices. Due to low weight, good mechanical and electrical properties, magnesium is widely used for manufacturing of mobile phones, laptops, cameras, etc. housings and other electronic components.

Historically, magnesium was one of the main aerospace construction metals and was used for German military aircraft as early as World War I and extensively for German aircraft in World War II. The Germans coined the name 'Elektron' for magnesium alloy which is still used today. However, due to perceived hazards with magnesium parts in the event of fire, the application of magnesium in the commercial aerospace industry was generally restricted to engine related components. Currently the use of magnesium alloys in aerospace is increasing, mostly driven by the increasing importance of fuel economy in aerospace and the need to reduce weight. The development and testing of new magnesium alloys notably Elektron 21 which has successfully undergone extensive aerospace testing for suitability in both engine, internal and airframe components. European Community runs three R&D magnesium projects in Aerospace priority of Six Framework Program.

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.
• Magnesium turnings or ribbon are used to prepare Grignard reagents, which are useful in organic synthesis
• Easily reacting with water, it can serve as a desiccant
• Magnesium is also flammable, burning at a temperature of approximately 2500 K (2200 °C, 4000 °F).
• The autoignition temperature of magnesium is approximately 744 K (473 °C, 883 °F).
• The extremely high temperature at which magnesium burns makes it a handy tool for starting emergency fires during outdoor recreation.
• Other uses include flashlight photography, flares, pyrotechnics, sparklers, and incendiary bombs.

In magnesium compounds

• Magnesium's hydroxide is used in milk of magnesia, its chloride and citrate used as oral magnesium supplements, and its sulfate ( Epsom salts) for various purposes in medicine, and elsewhere.
• Dead-burned magnesite is used for refractory purposes such as brick and liners in furnaces and converters.
• Magnesium carbonate (Mg CO₃) 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).
• The magnesium ion is necessary for all life (see magnesium in biological systems), so magnesium salts are an additive for foods, fertilizers (Mg is a component of chlorophyll), and culture media.

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:

Mg _(s) + 2 H₂O _(g) → Mg(OH)_{2 (aq)} + H_{2 (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). A Class D dry chemical fire extinguisher 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.