3: Lithium - Lithium Li Group: 1 Period: 2 Atomic number: 3 Atomic mass: 6.941 Configuration: He 2s 1 Atomic radius: 167 pm Covalent radius: 128 pm Electron affinity: 59.6 eV Ionization energy: 5.3917 eV Electronic term: 2 S 1/2 Mass fraction in the earth crust: 0.000017 Mass fraction in the earth space: 0.000000006 Electronegativity: 0.98. Periodic table of chemical elements with pictures and detailed chemical properties for each. 3 Li 6.9412: 4 Be 9.0121: 5 B 10.811: 6 C 12.010: 7 N 14.006: 8 O 15. Periodic table, in full periodic table of the elements, in chemistry, the organized array of all the chemical elements in order of increasing atomic number —i.e., the total number of protons in the atomic nucleus.
| Johan August Arfwedson discovered lithium in 1817. Lithium batteries have lithium metal or lithium compounds as an anode. |
Lithium
| Atomic Number: | 3 | Atomic Radius: | 182 pm (Van der Waals) |
| Atomic Symbol: | Li | Melting Point: | 180.5 °C |
| Atomic Weight: | 6.94 | Boiling Point: | 1330 °C |
| Electron Configuration: | [He]2s1 | Oxidation States: | +1 (a strongly basic oxide) |
Lithium Periodic Table Square
Li Periodic Table Electrons
History
From the Greek word lithos, stone. Discovered by Arfvedson in 1817. Lithium is the lightest of allmetals, 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 alligneous 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, andfrom those in Nevada. Large deposits of quadramene are found in North Carolina. The metalis 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, butnot as vigorously as sodium. Lithium imparts a beautiful crimson color to a flame, butwhen the metal burns strongly, the flame is a dazzling white.
Uses
Li Periodic Table Atomic Mass
Since World War II, the production of lithium metal and its compounds has increasedgreatly. Because the metal has the highest specific heat of any solid element, it hasfound use in heat transfer applications; however, it is corrosive and requires specialhandling. The metal has been used as an alloying agent, is of interest in synthesis oforganic compounds, and has nuclear applications. It ranks as a leading contender as abattery anode material as it has a high electrochemical potential. Lithium is used inspecial glasses and ceramics. The glass for the 200-inch telescope at Mt. Palomar containslithium as a minor ingredient. Lithium chloride is one of the most hygroscopic materialsknown, and it, as well as lithium bromide, is used in air conditioning and industrialdrying 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 carbonate is used for the treatment of bipolar disease and other mental illness conditions.
