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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 |
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 |
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 |
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 |
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 |
Number of isotopes: 2 |
Oxide(s): Li2O |
Hydride(s): LiH |
Chloride(s): LiCl |
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 |
Thermal conductivity: 84.8 J/m-sec-deg |
Electrical conductivity: 107.8 1/mohm-cm |
Polarizability: 24.3 A^3 |
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 |
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(Gr. lithos: stone) 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 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.
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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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