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Lithium


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Atomic symbol: Li
Atomic number: 3
Atomic weight: 6.94
Atomic volume: 13.10 cm3/mol
Density: 0.53 g/cm3
Period Number: 2
Group number: 1
Group name: Alkali Met.
Element classification: Metal


States


Phase at room temperature: Solid
Melting Point: 453.74 K
Boiling point: 1620 K
Heat of fusion: 3.00 kJ/mol
Heat of vaporization: 145.920 kJ/mol


Energies


Ionization Energy: 5.392 eV
1st ionization energy: 520.2 kJ/mole
2nd ionization energy: 7394.4 kJ/mole
3rd ionization energy: 11814.6 kJ/mole
Electronegativity: 0.98
Electron affinity: 59.63 kJ/mole
Specific heat: 3.6 J/gK
Heat atomization: 161 kJ/mole atoms


Oxidation & Electrons


Shells: 2,1
Electron Shell Configuration: [He] 2s1
Minimum oxidation number: -1
Maximum oxidation number: 1
Minimum common oxidation number: 0
Maximum common oxidation no: 1


Appearance & Characteristics


Structure:: bcc: body-centered cubic
Color: silvery
Hardness: 0.6 mohs
Toxicity: ?
Characteristics: soft, lightest solid
Uses: batteries, lubricant


Reactions


Reaction with air: vigorous, =>Li2O
Reaction with 6M HCl: vigorous, =>H2, LiCl
Reaction with 15M HNO3: vigorous, =>LiNO3
Reaction with 6M NaOH: mild, =>H2, LiOH


Other Forms


Number of isotopes: 2
Oxide(s): Li2O
Hydride(s): LiH
Chloride(s): LiCl


Radius


Atomic Radius: 152 pm
Ionic radius (1- ion): 90 pm
Ionic radius (1+ ion): 90 pm
Ionic radius (2- ion): pm
Ionic radius (2+ ion): pm
Ionic radius (3+ ion): 90 pm


Conductivity


Thermal conductivity: 84.8 J/m-sec-deg
Electrical conductivity: 107.8 1/mohm-cm
Polarizability: 24.3 A^3


Abundance


Source: Spodumene (silicate)
Relative abundance solar system: 1.757 log
Abundance earth's crust: 1.3 log
Estimated crustal abundance: 2.0×101 milligrams per kilogram
Estimated oceanic abundance: 1.8×10-1 milligrams per liter
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 


History


(Gr. lithos: stone) Discovered by Arfvedson in 1817. Lithium is the lightest of all metals, with a density only about half that of water.


Sources


It does not occur freely in nature; combined, it is found in small units in nearly all igneous rocks and in many mineral springs. Lepidolite, spodumene, petalite, and amblygonite are the more important minerals containing it.

Lithium is presently being recovered from brines of Searles Lake, in California, and from those in Nevada. Large deposits of quadramene are found in North Carolina. The metal is produced electrolytically from the fused chloride. Lithium is silvery in appearance, much like Na, K, and other members of the alkali metal series. It reacts with water, but not as vigorously as sodium. Lithium imparts a beautiful crimson color to a flame, but when the metal burns strongly, the flame is a dazzling white.


Uses


Since World War II, the production of lithium metal and its compounds has increased greatly. Because the metal has the highest specific heat of any solid element, it has found use in heat transfer applications; however, it is corrosive and requires special handling. The metal has been used as an alloying agent, is of interest in synthesis of organic compounds, and has nuclear applications. It ranks as a leading contender as a battery anode material as it has a high electrochemical potential. Lithium is used in special glasses and ceramics. The glass for the 200-inch telescope at Mt. Palomar contains lithium as a minor ingredient. Lithium chloride is one of the most lyproscopic materials known, and it, as well as lithium bromide, is used in air conditioning and industrial drying systems. Lithium stearate is used as an all-purpose and high-temperature lubricant. Other lithium compounds are used in dry cells and storage batteries. Lithium carbide is used for the treatment of bipolar disease and other mental illness conditions.

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