Magnesium

Molecular structure of Magnesium (CAS NO.7439-95-4) is:

Product Name: Magnesium
CAS Registry Number: 7439-95-4
IUPAC Name: Magnesium
Molecular Weight: 24.305 [g/mol]
Molecular Formula: Mg 
EINECS: 231-104-6
Melting Point: 89 °C (dec.)(lit.)
Boiling Point: 1090 °C(lit.)
Density:  0.889 g/mL at 25 °C
Flash Point:  −26 °F
storage temp. water-free area
Solubility: H₂O: 1 M at 20 °C, clear, colorless
Water Solubility: Reacts
Sensitive: Hygroscopic
Product Categories: Inorganics; Inorganic Chemicals; Reagent Plus; MagnesiumEssential Chemicals; Reagent Grade; Routine Reagents; MagnesiumAlternative Energy; Alkali MetalsMetal and Ceramic Science; Magnesium; Materials for Hydrogen Storage; Metals; Alkali Metals; Reduction; Synthetic Reagents

In 1808, the metal magnesium itself was first produced in England by Sir Humphry Davy using electrolysis of a mixture of magnesia and mercury oxide. 
In 1831, Antoine Bussy prepared it in coherent form.
Davy's first suggestion for a name was magnium, but the name magnesium is now used.

 Magnesium (CAS NO.7439-95-4) is the third most commonly used structural metal, following steel and aluminium. In its purest form, can be compared with aluminium, and is strong and light, so it is used in several high volume part manufacturing applications, including automotive and truck components. Its compounds, primarily magnesium oxide (MgO), 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.It is also used in electronic devices. And it can be used to refine titanium in the Kroll process, to remove sulfur from iron and steel, to photoengrave plates in the printing industry, to combine in alloys, where this metal is essential for airplane and missile construction. In the form of turnings or ribbons, It is used to prepare Grignard reagents, which are useful in organic synthesis. Also, it can be used as an additive agent in conventional propellants and the production of nodular graphite in cast iron, as an alloying agent, improving the mechanical, fabrication and welding characteristics of aluminium, as a reducing agent for the production of uranium and other metals from their salts, as a desiccant, since it easily reacts with water and as a sacrificial (galvanic) anode to protect underground tanks, pipelines, buried structures, and water heaters.

 Magnesium (CAS NO.7439-95-4) occurs in seawater and in ores such as dolomite (CaCO₃·MgCO₃), magnesite (MgCO₃), and carnallite (MgCl₂·KCl·6H₂O).It can be made by several methods, but the most common method of manufacture is by the electrolytic process, as for example the electrolysis of magnesium chloride. The magnesium chloride is obtained from saline solution, from brine, and from the reaction of magnesium hydroxide (from seawater or dolomite) with hydrochloric acid. Electrolyzing magnesium chloride from seawater, using oyster shells for the lime needed is also an option. The oyster shells, which are almost pure calcium carbonate, are burned to lime, slaked, and mixed with the seawater, thus precipitating magnesium hydroxide. This magnesium hydroxide is filtered off and treated with hydrochloric acid prepared from the chlorine evolved by the cells to form magnesium chloride solution that is evaporated to solid magnesium chloride in direct-fired evaporators, followed by shelf drying. The chloride tends to decompose on drying and, after dehydrating, the magnesium chloride is fed to the electrolytic cells, where it is decomposed into the metal and chlorine gas. The internal parts of the cell act as the cathode, and 22 graphite anodes are suspended vertically from the top of the cell. The arrangement is very similar to the Downs sodium cell.
 Sodium chloride is added to the bath to lower the melting point and also increase the conductivity. The salts are kept molten by the electric current used to extract the magnesium plus external heat supplied by external gas-fired furnaces. The usual operating temperature is 710 °C, which is sufficient to melt the magnesium (melting point 651 °C). The molten magnesium is liberated at the cathode and rises to the bath surface, where troughs lead to the metal wells in front of the cell. The 99.9% pure magnesium metal is dipped out several times during the day, each dipperful containing enough metal to fill a 20-kg self-pelleting mold.
 The silicothermic, or ferrosilicon, process involves mixing ground burned dolomite with ground ferrosilicon and fluorspar (eutectic) and pelletizing after which the pellets are charged into the furnace. High vacuum and heat (1170 °C) are applied and the calcium oxide present in the burnt dolomite forms infusible calcium silicate that is removed from the retort.
12(MgO·CaO) + 6FeSi₆ → 12Mg + 6(CaO)₂SiO₂ + 6Fe

Inhalation of dust and fumes can cause metal fume fever. The powdered metal ignites readily on the skin causing burns. Particles embedded in the skin can produce gaseous blebs that heal slowly.
A dangerous fire hazard in the form of dust or flakes when exposed to flame or oxidizing agents. In solid form, magnesium is difficult to ignite because heat is conducted rapidly away from the source of ignition; it must be heated above its melting point before it will burn. However, in finely divided form, it may be ignited by a spark or the flame of a match. Magnesium fires do not flare up violently unless there is moisture present. Therefore, it must be kept away from water, moisture, etc. It may ignited spontaneously when the material is finely divided and damp, particularly with water-oil emulsion. Moderately explosive in the form of dust when exposed to flame. Also, magnesium reacts with moisture, acids, etc., to evolve hydrogen, a highly dangerous fire and explosion hazard.
Explosive reaction or ignition with calcium carbonate + hydrogen + heat, gold cyanide + heat, mercury cyanide + heat, silver oxide + heat, fused nitrates, phosphates, or sulfates (e.g., ammonium nitrate, metal nitrates), chloroformamidinium nitrate + water (when ignited with powder). The powder may explode on contact with halocarbons (e.g., chloromethane, chloroform, or carbon tetrachloride), and explodes when sparked in dichlorodifluoromethane. Hypergolic reaction with nitric acid + 2-nitroaniline. Mixtures of powdered magnesium and methanol are more powerful than some military explosives. Mixtures of magnesium powder + water can be detonated. Reacts with acetylenic compounds including traces of acetylene found in ethylene gas to form explosive magnesium acetylide.
Violent reactions with ammonium salts, chlorate salts, beryllium fluoride, boron diiodophosphide, carbon tetrachloride + methanol, 1,1,1-trichloroethane, 1,2-dibromoethane, halogens or interhalogens (e.g., fluorine, chlorine, bromine, iodine vapor, chlorine trifluoride, iodine heptafluoride), hydrogen iodide, metal oxides + heat (e.g., beryllium oxide, cadmium oxide, copper oxide, mercury oxide, molybdenum oxide, tin oxide, zinc oxide), nitrogen (when ignited), silicon dioxide powder + heat, polytetrafluoroethylene powder + heat, sulfur + heat, tellurium + heat, barium peroxide, nitric acid vapor, hydrogen peroxide, ammonium nitrate, sodium iodate + heat, sodium nitrate + heat, dinitrogen tetraoxide (when ignited), lead dioxide. Ignites in carbon dioxide at 780°C, molten barium carbonate + water, fluorocarbon polymers + heat, carbon tetrachloride or trichloroethylene (on impact), dichlorodifluoromethane + heat.
Incompatible with ethylene oxide, metal oxosalts, oxidants, potassium carbonate, Al + KClO₄, [Ba(NO₃)₂ + BaO₂ + Zn], bromobenzyl trifluoride, CaC, carbonates, CHCl₃, [CuSO₄ (anhydrous) + NH₄NO₃ + KClO₃ + H₂O], CuSO₄, (H₂ + CaCO₃), CH₃Cl, NO₂, liquid oxygen, metal cyanides (e.g., cadmium cyanide, cobalt cyanide, copper cyanide, lead cyanide, nickel cyanide, zinc cyanide), performic acid, phosphates, KClO₃, KClO₄, AgNO₃, NaClO₄, (Na₂O₂ + CO₂), sulfates, trichloroethylene, Na₂O₂.
To fight fire, operators and firefighters can approach a magnesium fire to within a few feet if no moisture is present. Water and ordinary extinguishers, such as CO₂, carbon tetrachloride, etc., should not be used on magnesium fires. G-1 powder or powdered talc should be used on open fires. Dangerous when heated; burns violently in air and emits fumes; will react with water or steam to produce hydrogen.
Hazard Codes: F,Xn
Risk Statements: 34-15-11-17-36/37/38-22-19 
R34:Causes burns. 
R15:Contact with water liberates extremely flammable gases. 
R11:Highly flammable. 
R17:Spontaneously flammable in air. 
R36/37/38:Irritating to eyes, respiratory system and skin. 
R22:Harmful if swallowed. 
R19:May form explosive peroxides.
Safety Statements: 43-7/8-43A-36-33-26 
S43:In case of fire use ... (there follows the type of fire-fighting equipment to be used.) 
S7/8:Keep container tightly closed and dry. 
S36:Wear suitable protective clothing. 
S33:Take precautionary measures against static discharges. 
S26: In case of contact with eyes, rinse immediately with plenty of water and seek medical advice.
RIDADR: UN 2056 3/PG 2
WGK Germany: 1
RTECS: OM3756000
F: 3-9
HazardClass: 4.1
PackingGroup: III
HS Code: 81049000

DOT Classification:  4.3; Label: Dangerous When Wet (UN 2950); DOT Class: 4.1; Label: Flammable Solid (UN 1869); DOT Class: 4.3; Label: Danger When Wet, Spontaneously Combustible

For occupational chemical analysis use NIOSH: Elements (ICP), 7300.

 Magnesium , its cas register number is 7439-95-4. It also can be called EckaGranules PK 31 ; Ecka Granules PK 51 ; Magnesium element ; Magnum Forte ; Ozone magnez .It is a silver or grey rod, turnings or ribbon. The more finely divided material reacts with water to liberate hydrogen, a flammable gas, though this reaction is not as vigorous as that of sodium or lithium with water. In finely divided forms is easily ignited. It burns with an intense white flame and it can be wax coated to render magnesium as nonreactive.It slowly oxidizes in moist air. Reacts very slowly with water at ordinary temperatures, less slowly at 100 °C.