The Magnesium reference article from the English Wikipedia on 24-Jul-2004
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Magnesium

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sodium - magnesium - aluminium
Be
Mg
Ca  
 
 
Image:Mg-TableImage.png
General
Name, Symbol, Number magnesium, Mg, 12
Series alkaline earth metals
Group, Period, Block 2 (IIA), 3, s
Density, Mohs hardness scale>Hardness kg/m³, 2.5
Appearance silvery white
125px
Atomic properties
Atomic weight 24.305 amu
Atomic radius (calc.) 150 pm (145 pm)
Covalent radius 130 pm
van der Waals radius 173 pm
Electron configuration Ne]3s²
e-'s per energy level 2, 8, 2
Oxidation states (Oxide) base)
Crystal structure Hexagonal
Physical properties
State of matter solid (magnetism>paramagnetic)
Melting point K (1202 ðF)
Boiling point 1363 K (1994 ðF)
Molar volume ×10-6 m³/mol
Heat of vaporization kJ/mol
Heat of fusion 8.954 kJ/mol
Vapor pressure Pa at 923 K
Speed of sound m/s at 293.15 K
Miscellaneous
Electronegativity 1.31 (Pauling scale)
Specific heat capacity J/(kg·K)
Electrical conductivity 22.6 106/m ohm
Thermal conductivity W/(m·K)
1st ionization potential 737.7 kJ/mol
2nd ionization potential 1450.7 kJ/mol
3rd ionization potential 7732.7 kJ/mol
Most Stable Isotopes
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
SI units & STP are used except where noted.
Magnesium is a chemical element in the periodic table that has the symbol Mg and atomic number 12. Magnesium is the eighth most abundant element and constitutes about 2% of the Earth's crust, 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.

Table of contents
1 Notable characteristics
2 Uses
3 History
4 Sources
5 Compounds in living organisms
6 Food sources
7 Isotopes
8 Precautions
9 External links

Notable characteristics

Magnesium is a fairly strong, silvery-white, light-weight metal (one third lighter than aluminium) that slightly tarnishes when exposed to air. In a powder, this metal heats and ignites when exposed to air 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.

Uses

Magnesium compounds, primarily magnesium oxide, are used mainly as refractory material in furnace linings for producing iron and steel, nonferrous metals, glass, and cement. Magnesium oxide and other compounds also are used in agricultural, chemical, and construction industries. This element's principal use is as an alloying additive to aluminium with these aluminium-magnesium alloys being used mainly for beverage cans. Magnesium alloys also are used as structural components of automobiles and machinery. Another use of this metal is to aid the removal of sulfur from iron and steel.

Other uses include:

History

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 Humphrey Davey 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.

Sources

In the United States this metal is principally obtained by electrolysis of fused magnesium chloride from brines, wells, and sea water. Although magnesium is found in over 60 minerals, only dolomite, magnesite, brucite, carnallite, talc, and olivine are of commercial importance.
Isolation (* follow):
cathode: Mg2+* + 2e- → Mg
anode: 2Cl-* → Cl2 (gas) + 2e-

Compounds in living organisms

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 include weight and size, is about 300 mg/day. Many enzymes require the presence of magnesium ions for their catalytic action.

Food sources

Green vegetables such as spinach provide magnesium because the center of the chlorophyll molecule contains magnesium. Nutss, 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.

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

Isotopes

Magnesium-26 is a stable isotope that has found application in
isotopic geology, similar to that of aluminium. Mg-26 is a radiogenic daughter product of Al-26, which has a half-life of 717000 years. Large enrichments of stable Mg-26 have been observed in the Ca-Al-rich inclusions of some carbonaceous chondrite meteorites. The anomalous abundance of Mg-26 is attributed to the decay of its parent Al-26 in the inclusions. Therefore, the meteorite must have formed in the solar nebula before the Al-26 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 Mg-26/Mg-24 against an Al/Mg ratio. In an isochrone plot, the Al/Mg ratio plotted is Al-27/Mg-24. The slope of the isochron has no age significance, but indicates the initial Al-26/Al-27 ratio in the sample at the time when the systems were separated from a common reservoir.

Precautions

Magnesium metal and alloys are highly flammable in their pure form as melts and when it is a powder.
Magnesium metal quickly reacts
exothermicallyally upon contact with air or water and should be handled with care. Wear safety glasses! The bright white light (including ultraviolet) produced by burning magnesium can damage the eyes. Water should not be used to extinguish magnesium fires.

External links