|Appearance||shiny grey solid|
|Standard atomic weight Ar, std(Mg)||[24.304, 24.307] conventional: 24.305|
|Magnesium in the periodic table|
|Atomic number (Z)||12|
|Group||group 2 (alkaline earth metals)|
|Electron configuration||[Ne] 3s2|
|Electrons per shell||2, 8, 2|
|Phase at STP||solid|
|Melting point||923 K (650 °C, 1202 °F)|
|Boiling point||1363 K (1091 °C, 1994 °F)|
|Density (near r.t.)||1.738 g/cm3|
|when liquid (at m.p.)||1.584 g/cm3|
|Heat of fusion||8.48 kJ/mol|
|Heat of vaporization||128 kJ/mol|
|Molar heat capacity||24.869 J/(mol·K)|
|Oxidation states||+1, +2 (a strongly basic oxide)|
|Electronegativity||Pauling scale: 1.31|
|Atomic radius||empirical: 160 pm|
|Covalent radius||141±7 pm|
|Van der Waals radius||173 pm|
|Spectral lines of magnesium|
|Crystal structure||hexagonal close-packed (hcp)|
|Speed of sound thin rod||4940 m/s (at r.t.) (annealed)|
|Thermal expansion||24.8 µm/(m·K) (at 25 °C)|
|Thermal conductivity||156 W/(m·K)|
|Electrical resistivity||43.9 nΩ·m (at 20 °C)|
|Magnetic susceptibility||+13.1·10−6 cm3/mol (298 K)|
|Young's modulus||45 GPa|
|Shear modulus||17 GPa|
|Bulk modulus||35.4 GPa|
|Brinell hardness||44–260 MPa|
|Naming||after Magnesia, Greece|
|Discovery||Joseph Black (1755)|
|First isolation||Humphry Davy (1808)|
|Main isotopes of magnesium|
Magnesium ( /mæɡˈniːziəm/ mag-NEE-zee-əm) is a chemical element with the symbol Mg, atomic number 12 and common oxidation state +2. It is an alkaline earth metal and the eighth most abundant element in the Earth's crust, where it constitutes about 2% by mass, and ninth in the known universe as a whole. This preponderance of magnesium is related to the fact that it is easily built up in supernova stars from a sequential addition of three helium nuclei to carbon (which in turn is made from three helium nuclei). Magnesium ion's high solubility in water helps ensure that it is the third most abundant element dissolved in seawater.
Magnesium is the 11th most abundant element by mass in the human body. Its ions are essential to all living cells. The ions play a major role in manipulating important biological polyphosphate compounds like ATP, DNA, and RNA. Hundreds of enzymes thus require magnesium ions to function. Magnesium is also the metallic ion at the center of chlorophyll, and is thus a common additive to fertilizers. Magnesium ions are sour to the taste, and in low concentrations help to impart a natural tartness to fresh mineral waters.
The free element (metal) is not found naturally on Earth, as it is highly reactive (though once produced, is coated in a thin layer of oxide (see passivation), which partly masks this reactivity). The free metal burns with a characteristic brilliant white light, making it a useful ingredient in flares. The metal is now mainly obtained by electrolysis of magnesium salts obtained from brine.
Uses[change | change source]
Commercially, the chief use for the metal is as an alloying agent to make aluminium-magnesium alloys, sometimes called "magnalium" or "magnelium". Since magnesium is less dense than aluminium, these alloys are prized for their relative lightness and strength.
Magnesium is used in fireworks to make a brilliant bright light. Another use is to mix it with other metals to make it strong, lightweight alloys such as those used to make bicycle frames.
Magnesium compounds are used medicinally as common laxatives, antacids (i.e., milk of magnesia), and in a number of situations where stabilization of abnormal nerve excitation and blood vessel spasm is required (that is, to treat eclampsia).
Magnesium is used in electronic devices, including: mobile phones, laptop computers, cameras, and other electronic components. Magnesium's low weight, good mechanical and electrical properties are good for these uses.
Magnesium is also used in incendiary bombs, which are bombs that blow up and spread fire everywhere.
Related pages[change | change source]
References[change | change source]
- Bernath, P. F.; Black, J. H. & Brault, J. W. (1985). "The spectrum of magnesium hydride" (PDF). Astrophysical Journal. 298: 375. Bibcode:1985ApJ...298..375B. doi:10.1086/163620.
- Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
- K. A. Gschneider, Solid State Phys. 16, 308 (1964)
- Bernath, P. F.; Black, J. H.; Brault, J. W. (1985). "The spectrum of magnesium hydride" (PDF). Astrophysical Journal. 298: 375. Bibcode:1985ApJ...298..375B. doi:10.1086/163620. Unknown parameter
- Ash, Russell (2005). The Top 10 of Everything 2006: The Ultimate Book of Lists. Dk Pub. ISBN 0756613213. Archived from the original on 2010-02-10. Retrieved 2011-09-26..
- Anthoni, J Floor (2006). "The chemical composition of seawater".
- "Magnesium in health".