Lithium | Wikipedia audio article
Channel: wikipedia tts
Date: 2019-01-31

This is an audio version of the Wikipedia Article:
https://en.wikipedia.org/wiki/Lithium


00:02:45 1 Properties
00:02:55 1.1 Atomic and physical
00:06:12 1.2 Chemistry and compounds
00:09:44 1.2.1 Organic chemistry
00:10:44 1.3 Isotopes
00:14:49 2 Occurrence
00:14:58 2.1 Astronomical
00:17:42 2.2 Terrestrial
00:22:26 2.3 Biological
00:23:18 3 History
00:29:40 4 Production
00:30:50 4.1 Reserves
00:36:50 4.2 Pricing
00:37:57 4.3 Extraction
00:39:04 4.4 Investment
00:39:41 5 Applications
00:39:51 5.1 Ceramics and glass
00:40:39 5.2 Electrical and electronics
00:41:47 5.3 Lubricating greases
00:42:22 5.4 Metallurgy
00:43:40 5.5 Silicon nano-welding
00:44:02 5.6 Other chemical and industrial uses
00:44:13 5.6.1 Pyrotechnics
00:44:32 5.6.2 Air purification
00:46:00 5.6.3 Optics
00:47:31 5.6.4 Organic and polymer chemistry
00:48:45 5.6.5 Military applications
00:49:45 5.7 Nuclear
00:54:07 5.8 Medicine
00:54:54 6 Biological role
00:56:15 7 Precautions
00:57:02 7.1 Regulation
00:58:20 8 See also



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SUMMARY
=======
Lithium (from Greek: λίθος, translit. lithos, lit. 'stone') is a chemical element with symbol Li and atomic number 3. It is a soft, silvery-white alkali metal. Under standard conditions, it is the lightest metal and the lightest solid element. Like all alkali metals, lithium is highly reactive and flammable, and is stored in mineral oil. When cut, it exhibits a metallic luster, but moist air corrodes it quickly to a dull silvery gray, then black tarnish. It never occurs freely in nature, but only in (usually ionic) compounds, such as pegmatitic minerals, which were once the main source of lithium. Due to its solubility as an ion, it is present in ocean water and is commonly obtained from brines. Lithium metal is isolated electrolytically from a mixture of lithium chloride and potassium chloride.
The nucleus of the lithium atom verges on instability, since the two stable lithium isotopes found in nature have among the lowest binding energies per nucleon of all stable nuclides. Because of its relative nuclear instability, lithium is less common in the solar system than 25 of the first 32 chemical elements even though its nuclei are very light: it is an exception to the trend that heavier nuclei are less common. For related reasons, lithium has important uses in nuclear physics. The transmutation of lithium atoms to helium in 1932 was the first fully man-made nuclear reaction, and lithium deuteride serves as a fusion fuel in staged thermonuclear weapons.Lithium and its compounds have several industrial applications, including heat-resistant glass and ceramics, lithium grease lubricants, flux additives for iron, steel and aluminium production, lithium batteries, and lithium-ion batteries. These uses consume more than three quarters of lithium production.
Lithium is present in biological systems in trace amounts; its functions are uncertain. Lithium salts have proven to be useful as a mood-stabilizing drug in the treatment of bipolar disorder in humans.