| Lithium - Li
CAS: 7439-93-2 Description: Soft, silvery-white; the lightest metal Classification: Alkali Metal Date of Discovery: 1817 Discoverer: Johann Arfvedson Name Origin: Greek lithos, "stone" |
|
|
Atomic Number: 3
Number of Neutrons: 4 Atomic Mass: 6.941(2) amu Melting Point: 180.5 °C Boiling Point: 1342 °C Density (293 K): 0.534 g/cm3 Atomic volume: 13.10 cm3/mol Electrical resistivity: 0.108 10-6/cm 
Thermal conductivity: 0.847 W/cmK Enthalpy of atomization: 160.67 kJ/mol Enthalpy of vaporization: 145.920 kJ/mol Enthalpy of fusion: 3.00 kJ/mol Specific heat capacity: 3.6 J/gK |
Energy levels: 2-1
Electron configuration: [He]2s1 Crystal Structure: Cubic body centered Atomic radius: 2.05 Å Covalent radius: 1.23 Å Oxidation States: +1 Electronegativity, Pauling: 0.98 Electron affinity: 0.6180 eV First ionization energy: 5.392 eV 2nd ionization energy: 76.638 eV 3rd ionization energy: 122.451 eV Polarizability: 24.3 10-24cm3 |
| Isotope | Natural Abundance | Atomic Mass | Half-life | Decay Mode | Spin |
| 5Li | 5.01254 |  3 x 10-22 |
 - |
3/2- | |
| 6Li | 7.5(2) | 6.015122 | 1+ | ||
| 7Li | 92.5(2) | 7.016004 | 3/2- | ||
| 8Li | 8.022486 | 0.84 s | -,  |
2+ | |
| 9Li | 9.026789 | 0.178 s | - |
3/2- | |
| 10Li | 10.03590 | 4 x 10-22 s | - |
||
| 11Li | 11.04379 | 8.7 ms | - |
(1/2-) | |
|
Discovered by Arfvedson in 1817. Lithium is the lightest of all metals, with a density only about half that of water. It does not occur free in nature; combined it is found in small amounts in nearly all igneous rocks and in the waters of many mineral springs. Lepidolite [KLi2Al(Al,Si)3O10(F,OH)2], spodumene (LiAlSi2O6), petalite, and amblygonite [(Li,Na)AlPO4(F,OH)], are the more important minerals containing it. Lithium is presently being recovered from brines of Searles Lake, in California. and from Nevada, Chile, and Argentina. Large deposits of spodumene are found in North Carolina. The metal is produced electrolytically from the fused chloride. Lithium is silvery in appearance, much like Na and K, 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. 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 hygroscopic 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. Seven isotopes of lithium are
recognized. Natural lithium contains two isotopes.
LINKS: Lithium Carbonate Lithium Technology Corporation Return
Sources for the information on this website include: Lide, David R., ed. CRC Handbook of Chemistry and Physics, 78th Ed., 1997-1998. |
|||||