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Magnesium Data tables and historic information.
| USGS_Minerals_Information__Magnesium Statistics and information on the worldwide supply, demand, and flow of the element (PDF format).
| Visual_Elements__Magnesium Image, general and physical information, source, uses, key isotopes, and ionisation energies.
| WebElements__Magnesium Extensive information on history, uses, occurrence, compounds, and properties of the element.
| Wikipedia__Magnesium Properties of the element, including its history, applications, and characteristics.
| Radiochemistry_of_Magnesium Full text of the monograph by A. W. Fairhall (Dept. of Chemistry, University of Washington, Seattle, Washington). [PDF] (January, 1961)
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Magnesium (Mg) - Chemical properties, Health and Environmental effects
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Chemical properties of magnesium
- Health
effects of magnesium - Environmental effects of magnesium
Atomic number
12
Atomic mass
24.305 g.mol -1
Electronegativity
according to Pauling
1.2
Density
1.74 g.cm -3 at 20 °C
Melting point
650 °C
Boiling point
1107 °C
Vanderwaals
radius
0.16 nm
Ionic radius
0.065 nm
Isotopes
5
Electronic
shell
[Ne] 3s2
Energy of
first ionisation
737.5 kJ.mol -1
Energy of
second ionisation
1450 kJ.mol -1
Standard
potential
- 2.34 V
Discovered by
Sir Humphrey Davy in 1808
Magnesium
Chemical element, metallic, symbol Mg, situated in group IIa in
the periodic table, atomic number: 12, atomic weight: 24,312. Magnesium
is silvery white and very light. Its relative density is 1,74 and it’s
density 1740 kg/m3 (0.063
lb/in3 or 108.6 lb/ft3). Magnesium is known for a
long time as the lighter structural metal in the industry, due to it’s
low weight and to it’s capability of forming mechanically resistant
alloys.
Magnesium is very chemically active, it takes the place of hydrogen in
boiling water and a great number of metals can be produced by thermic
reduction of its salts and oxidized forms with magnesium. It joins
together with most non-metals and almost every acid. Magnesium reacts
only slightly or not at all with most of the alkalis and many
organic substances, like hydrocarbons, aldehides, alcohols, phenols,
amines, esters and most of the oils. Used as a catalyst, magnesium
promotes organic reactions of condensation, reduction, addition and
dehalogenization. It was used for a long time for synthesizing special
and complex organic components by the well-known Grignard reaction. The
main ingredients of the alloys are: aluminum, manganese,
zircon, zinc,
rare-earth metals and thorium.
Applications
Magnesium compounds are used as
refractory material in furnace linings for producing metals (iron and steel,
nonferrous metals), glass, and cement.
With a density of only two thirds of the aluminum’s, it has
countless applications in cases where weight reducing is important, i.e.
in aeroplane and missile construction. It
also has many useful chemical and metallurgic properties, which make it
appropriate for many other non-structural applications.
Magnesium components are widely used in industry and agriculture.
Other uses include: removal of sulphur form iron and steel,
photoengraved plates in the printing industry; reducing agent for
the production of pure uranium and other metals from their salts; flashlight photography, flares, and pyrotechnics.
Magnesium in the environment
Magnesium is the eighth most abundant element and constitutes about 2% af the Earth's crust
by weight, and it is the third most plentiful element dissolved in
seawater.
It’s very abundant in nature, and it’s found in important
quantities in many rocky minerals, like dolomite, magnetite, olivine and
serpentine. It’s also found in seawater, underground brines and salty
layers. It’s the third most abundant structural metal in the earth’s
crust, only exceeded by
aluminum and iron.
The United States has traditionally been the major world supplier of
this metal, supplying 45% of world production even as recently as 1995.
Dolomite and magnesite are mined to the extent of 10 million tonnes per
year, in countries such as China, Turkey, North Korea, Slovakia,
Austria, Russia and Greece.
Health
effects of magnesium
Humans take in between 250 and 350 mg/day of magnesium and need at
least 200 mg, but the body deals very effectively with this element,
taking it form food when it can, and recycling what we already have when
it cannot.
There is no evidence that magnesium
produces systemic poisoning although persistent over-indulgence in
taking magnesium supplements and medicines can lead to muscule weakness,
lethargy and confusion.
Effects
of exposure to magnesium powder:
low toxicity & not considered to be hazardous to health. Inhalation:
dust may irritate mucous membranes or upper respiratory tract. Eyes:
mechanical injury or particle may embed in eye. Viewing of burning
magnesium powder without fire glasses may result in "Welder's
flash", due to intense white flame. Skin: embedding of particle in
skin. Ingestion: unlikely; however, ingestion of large amounts of
magnesium powder could cause injury.
Magnesium has not been tested, but it’s not suspected of being
carcinogenic, mutagenic or teratogenic. Exposure to magnesium oxide fume
subsequent to burning, welding or molten metal work can result in metal
fume fever with the following temporary symptoms: fever, chills, nausea,
vomiting & muscle pain. These usually occur 4-12 hours after
exposure & last up to 48 hours. Magnesium oxide fume is a by-product
of burning magnesium.
Physical dangers:
Dust
explosion possible if in powder or granular form, mixed with air. If
dry, it can be charged electrostatically by swirling, pneumatic
transport, pouring, etc.
Chemical dangers: The substance may spontaneously ignite on
contact with air or moisture producing irritating or toxic fumes. Reacts
violently with strong oxidants. Reacts violently with many substances
causing fire and explosion hazard. Reacts with acids and water forming
flammable hydrogen gas (see ICSC0001), causing fire and explosion
hazard.
First
Aid: Inhalation: remove to
fresh air. Eyes: flush eyes with water thoroughly. Consult a physician.
Skin: wash with soap & water thoroughly to remove particles.
Ingestion: if large amounts of magnesium powder are ingested, induce
vomiting & consult a physician.
Note
to physician: no specific treatment or antidote. Supportive care
recommended. Treatment should be based on reactions of the patient.
Environmental effects of magnesium
There is very little
information available on the environmental effects of magnesium oxide
fume. If other mammals inhale magnesium oxide fume, they may suffer
similar effects as do humans.
On
an environmental spectrum of 0 - 3 Magnesium oxide fume registers 0.8. A
score of 3 represents a very high hazard to the environment and 0 a
negligible hazard. Factors that are taken into account to obtain this
ranking include the extent of the material's toxic or poisonous nature
and/or its lack of toxicity, and the measure of its ability to remain
active in the environment and whether it accumulates in living
organisms. It does not take into exposure to the substance.
Magnesium
powder is not suspected of being highly harmful to the environment. As
magnesium oxide an aquatic toxicity rating of tlm 1000 ppm has been
established. "Water Quality Characteristics of Hazardous
Materials", Hann & Jensen, Enviro. End. Div., Texas A&M,
vol. 3 (1974).
Read more on
magnesium in
water
Back to the
periodic table of elements.
Recommended daily intake of
magnesium
[ Home
] [ Back ] [ More
Information or question on Magnesium? ]
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