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Lithium

From Wikipedia, the free encyclopedia

This article is about the chemical element. For the use of lithium as a medication, see Lithium (medication). For other uses, see Lithium (disambiguation).

Lithium
3Li
H ↑ Li ↓ Na helium ← lithium → beryllium
Lithium in the periodic table
Appearance
silvery-white (shown floating in oil) Spectral lines of lithium
General properties
Name, symbol, number	lithium, Li, 3
Pronunciation	/ˈlɪθiəm/ LI-thee-əm
Element category	alkali metal
Group, period, block	1 (alkali metals), 2, s
Standard atomic weight	6.94(1)
Electron configuration	[He] 2s1 2, 1
Physical properties
Phase	solid
Density (near r.t.)	0.534 g·cm−3
Liquid density at m.p.	0.512 g·cm−3
Melting point	453.65 K, 180.50 °C, 356.90 °F
Boiling point	1603 K, 1330 °C, 2426 °F
Critical point	(extrapolated) 3220 K, 67 MPa
Heat of fusion	3.00 kJ·mol−1
Heat of vaporization	136 kJ·mol−1
Molar heat capacity	24.860 J·mol−1·K−1
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 797 885 995 1144 1337 1610
Atomic properties
Oxidation states	+1 (strongly basic oxide)
Electronegativity	0.98 (Pauling scale)
Ionization energies	1st: 520.2 kJ·mol−1
	2nd: 7298.1 kJ·mol−1
	3rd: 11815.0 kJ·mol−1
Atomic radius	152 pm
Covalent radius	128±7 pm
Van der Waals radius	182 pm
Miscellanea
Crystal structure	body-centered cubic
Magnetic ordering	paramagnetic
Electrical resistivity	(20 °C) 92.8 nΩ·m
Thermal conductivity	84.8 W·m−1·K−1
Thermal expansion	(25 °C) 46 µm·m−1·K−1
Speed of sound (thin rod)	(20 °C) 6000 m·s−1
Young's modulus	4.9 GPa
Shear modulus	4.2 GPa
Bulk modulus	11 GPa
Mohs hardness	0.6
CAS registry number	7439-93-2
History
Discovery	Johan August Arfwedson (1817)
First isolation	William Thomas Brande (1821)
Most stable isotopes
Main article: Isotopes of lithium
iso NA half-life DM DE (MeV) DP 6Li 7.5% 6Li is stable with 3 neutrons 7Li 92.5% 7Li is stable with 4 neutrons 6Li content may be as low as 3.75% in natural samples. 7Li would therefore have a content of up to 96.25%.
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Lithium (from Greek: λίθος lithos, "stone") is a chemical element with symbol Li and atomic number 3. It is a soft, silver-white metal belonging to the alkali metal group of chemical elements. Under standard conditions it is the lightest metal and the least dense solid element. Like all alkali metals, lithium is highly reactive and flammable. For this reason, it is typically stored in mineral oil. When cut open, lithium exhibits a metallic luster, but contact with moist air corrodes the surface quickly to a dull silvery gray, then black tarnish. Because of its high reactivity, lithium never occurs freely in nature, and instead, only appears in compounds, which are usually ionic. Lithium occurs in a number of pegmatitic minerals, but due to its solubility as an ion is present in ocean water and is commonly obtained from brines and clays. On a commercial scale, lithium is isolated electrolytically from a mixture of lithium chloride and potassium chloride.
The nuclei of lithium verge 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 the nuclei are very light in atomic weight.^[1] For related reasons, lithium has important links to nuclear physics. The transmutation of lithium atoms to helium in 1932 was the first fully man-made nuclear reaction, and lithium-6 deuteride serves as a fusion fuel in staged thermonuclear weapons.^[2]
Lithium and its compounds have several industrial applications, including heat-resistant glass and ceramics, high strength-to-weight alloys used in aircraft, lithium batteries and lithium-ion batteries. These uses consume more than half of lithium production.
Trace amounts of lithium are present in all organisms. The element serves no apparent vital biological function, since animals and plants survive in good health without it. Non-vital functions have not been ruled out. The lithium ion Li⁺ administered as any of several lithium salts has proved to be useful as a mood-stabilizing drug in the treatment of bipolar disorder, due to neurological effects of the ion in the human body.