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History and Production
From Greek Magnesia, meaning district of Thessaly. It was first identified by J. Black in 1755 and subsequently isolated H. Davy in 1808. Is can be prepared from electrolysis of fused magnesium chloride derived from brines or sea water. It is used in flashlight photography, flares.
It is also used as alloys for airplane construction and as a reducing agent in the production of titanium, uranium and other metals.
Physical Data
It is a light, silvery-white metal. It tarnishes slightly in air due to formation of the oxide film on the metal. Finely divided magnesium burns easily with a very bright white flame. Magnesium does not occur free in nature, but in the forms of carbonates, sulfates and silicates.
It is an important element in both plant and animal life. For example, the Mg-porphine complexes involved in photosynthesis.
Interatomic distance: 319.8 pm
Melting point: 650°C
Boiling point: 1090°C
Thermal conductivity/Wm-1K-1: 156 (27°C)
Density/kgm-3: 1738 (20°C), 1585 (m.p.)
Standard Thermodynamic Data (atomic gas)
Enthalpy of formation: 147.1 kJ/mol
Gibbs free energy of formation: 112.5 kJ/mol
Entropy: 148.6 J/mol K
Heat capacity: 20.8 J/mol K
Electronic data
Electronic configuration: [Ne] 3s2
Term symbol: 1S0
Electron affinity: (not stable) Electronegativity (Pauline): 1.31
Ionization energy (first, second, third): 737.751, 1450.69, 7732.70 kJ/mol
Chemical properties
Magnesium burns brilliantly white in air to give magnesium oxide, MgO and Mg3N2. With steam, it forms
the oxide and hydrogen. In addition, magnesium also reacts with some organic compounds. For instance, with alkyl halides give
Grignard reagent, an important starting reagent in synthesis of some organic compounds.
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