Lithium

This article is about the chemical element lithium. For other uses, see lithium (disambiguation).

3 helium ← lithium → beryllium H ↑ Li ↓ Na periodic table
General
Name, Symbol, Number	lithium, Li, 3
Chemical series	alkali metals
Group, Period, Block	1, 2, s
Appearance	silvery white/gray
Atomic mass	6.941(2) g/mol
Electron configuration	1s2 2s1
Electrons per shell	2, 1
Physical properties
Phase	solid
Density (near r.t.)	0.534 g/cm³
Liquid density at m.p.	0.512 g/cm³
Melting point	453.69 K (180.54 °C, 356.97 °F)
Boiling point	1615 K (1342 °C, 2448 °F)
Critical point	(extrapolated) 3223 K, 67 MPa
Heat of fusion	3.00 kJ/mol
Heat of vaporization	147.1 kJ/mol
Heat capacity	(25 °C) 24.860 J/(mol·K)
Vapor pressure P/Pa 1 10 100 1 k 10 k 100 k at T/K 797 885 995 1144 1337 1610
Atomic properties
Crystal structure	cubic body centered
Oxidation states	1 (strongly basic oxide)
Electronegativity	0.98 (Pauling scale)
Ionization energies	1st: 520.2 kJ/mol
	2nd: 7298.1 kJ/mol
	3rd: 11815.0 kJ/mol
Atomic radius	145 pm
Atomic radius (calc.)	167 pm
Covalent radius	134 pm
Van der Waals radius	182 pm
Miscellaneous
Magnetic ordering	nonmagnetic
Electrical resistivity	(20 °C) 92.8 nΩ·m
Thermal conductivity	(300 K) 84.8 W/(m·K)
Thermal expansion	(25 °C) 46 µm/(m·K)
Speed of sound (thin rod)	(20 °C) 6000 m/s
Speed of sound (thin rod)	(r.t.) 4.9 m/s
Shear modulus	4.2 GPa
Bulk modulus	11 GPa
Mohs hardness	0.6
CAS registry number	7439-93-2
Notable isotopes
Main article: Isotopes of lithium iso NA half-life DM DE (MeV) DP 6Li 7.5% Li is stable with 3 neutrons 7Li 92.5% Li 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%.

Lithium (chemical symbol Li, atomic number 3) (from Greek: lithos: stone) is the lightest solid chemical element. It is classified as an alkali metal. Lithium in its pure form is a soft, silver white metal that tarnishes and oxidizes very rapidly in air and water. It is used primarily in heat-transfer, household appliances like toasters and microwaves alloys and batteries, and also in some mood stabilizing drugs. Lithium is one of only four elements theorized to have been created in the first three minutes of the universe through a process called Big Bang nucleosynthesis.

Notable characteristics

Lithium is a metallic element in group 1, period 2 of the periodic table.

Though in group 1, lithium also exhibits properties of the alkaline-Earth metals in group 2. Like all alkali metals, it has a single valence electron, and will readily lose this electron to become a positive ion. Because of this, lithium reacts easily with water and does not occur freely in nature. Nevertheless, it is less reactive than the chemically similar sodium.

Lithium is soft enough to be cut with a knife, though this is significantly more difficult to do than cutting sodium. The fresh metal is silver, rapidly tarnishing black in air. Lithium has only about half the specific gravity of water, giving solid metal lithium sticks the odd heft of a very light wood, such as balsa. The metal floats highly in hydrocarbons due to its low density, and jars of lithium in the laboratory are typically composed of black-coated sticks held down in hydrocarbon mechanically by the lid of the jar and other sticks.

When placed over a flame, lithium gives off a striking crimson color but when it burns strongly, the flame becomes a brilliant white. Lithium will ignite and burn when exposed to water and water vapors in oxygen. It is the only metal that reacts with nitrogen at room temperature. Lithium has a high specific heat capacity, 3582 J/(kg·K), and a great temperature range in its liquid form, which makes it a useful chemical.

Lithium in its pure form is highly flammable and slightly explosive when exposed to air and especially water. Lithium fires are difficult to extinguish, requiring special chemicals designed to smother them. Lithium metal is also corrosive and requires special handling to avoid skin contact. Lithium should be stored in a non-reactive compound such as naphtha or a hydrocarbon. In humans lithium compounds play no natural biological role and are considered to be slightly toxic. Humans aside, lithium appears to be an essential trace element for goats and possibly rats. When used as a drug, blood concentrations of Li⁺ must be carefully monitored.

Isotopes

Naturally occurring lithium is composed of 2 stable isotopes, ⁶Li and ⁷Li, of which the latter is the more abundant (92.5% natural abundance). In addition, seven radioisotopes have been characterized. Among them, ⁸Li has a half-life of 838 milliseconds (ms), ⁹Li has a half-life of 178.3 ms, and the others have half-lives that are less than 8.6 ms. The shortest-lived isotope of lithium is ⁴Li, which decays through proton emission and has a half-life of 7.58043x10^-23 seconds.

According to the "Big Bang" model of the origin of the universe, the nuclei of ⁷Li were among the few types of atomic nuclei formed shortly after the Big Bang, during a phase called the "Big Bang nucleosynthesis".

Occurrence

Lithium pellets (covered in white lithium hydroxide)

Lithium is widely distributed but does not occur in nature in its free form. Because of its reactivity, it is always found bound with one or more other elements or compounds. It forms a minor part of almost all igneous rocks and is also found in many natural brines. Lithium is the thirty-first most abundant element, contained in trace amounts in the minerals spodumene, lepidolite, and amblygonite. The Earth's crust contains 65 parts per million (ppm) of lithium. Along with hydrogen, helium, and beryllium, some lithium was created in the big bang.

Since the end of World War II, lithium production has greatly increased. The metal is separated from other elements in igneous rocks, and is also extracted from the water of mineral springs. Lepidolite, spodumene, petalite, and amblygonite are the more important minerals containing it.

In the United States lithium is recovered from brine pools in Nevada. Today, most commercial lithium is recovered from brine sources in Argentina and Chile. The metal, which is silvery in appearance like sodium, potassium and other members of the alkali metal series, is produced electrolytically from a mixture of fused lithium and potassium chloride. In 1998 it was about US$ 43 per pound ($95 per kg). Chile is currently the leading pure metal lithium producer in the world.

History

Petalite, which contains lithium, was first discovered by the Brazilian scientist José Bonifácio de Andrada e Silva toward the end of the 1700s on a trip to Sweden. Lithium was discovered by Johann Arfvedson in 1817. Arfvedson found the new element within the minerals spodumene and lepidolite in a petalite ore, LiAl(Si₂O₅)₂, he was analyzing during a routine investigation of some minerals from a mine on the island Utö in Sweden. In 1818 Christian Gmelin was the first to observe that lithium salts give a bright red color in flame. Both men tried and failed to isolate the element from its salts.

The element was not isolated until William Thomas Brande and Sir Humphrey Davy later used electrolysis on lithium oxide in 1818. Bunsen and Matiessen isolated larger quantities of the metal by electrolysis of lithium chloride in 1855. Commercial production of lithium metal was achieved in 1923 by the German company Metallgesellschaft through using electrolysis of molten lithium chloride and potassium chloride. It was apparently given the name "lithium" (Greek λιθoς (lithos), meaning "stone") because it was discovered from a mineral while other common alkali metals were first discovered from plant tissue.

Applications

Because of its specific heat, the largest of any solid, lithium is used in heat transfer applications. It is also an important battery anode material, used in lithium ion batteries due to its high electrochemical potential. In addition to being lighter than the standard dry cell, these batteries produce a higher voltage (3 volts versus 1.5 volts). Other uses:

• See lithium pharmacology for pharmacological information. Lithium salts such as lithium carbonate (Li₂CO₃), lithium citrate, and lithium orotate are mood stabilizers (the effect is due to the lithium ion, so the type of salt is unimportant). They are used in the treatment of bipolar disorder, since unlike most other mood altering drugs, they counteract both mania and depression. Lithium can also be used to augment other antidepressant drugs. Useful amounts of lithium for this use are only slightly lower than toxic amounts, so the blood levels of lithium must be carefully monitored during such treatment.
• Lithium chloride and lithium bromide are extremely hygroscopic and frequently used as desiccants.
• Lithium stearate is a common all-purpose high-temperature lubricant.
• Lithium is an alloying agent used to synthesize organic compounds.
• Lithium is used as a flux to promote the fusing of metals during welding and soldering. It also eliminates the forming of oxides during welding by absorbing impurities. This fusing quality is also important as a flux for producing ceramics, enamels, and glass.
• Lithium is sometimes used in glasses and ceramics including the glass for the 200-inch (5.08 m) telescope at Mt. Palomar.
• Alloys of the metal with aluminium, cadmium, copper, and manganese are used to make high performance aircraft parts.
• Lithium niobate is used extensively in telecommunication products, such as mobile phones and optical modulators.
• The high non-linearity of lithium niobate also makes a good choice for non-linear optics applications.
• Lithium deuteride was the fusion fuel of choice in early versions of the hydrogen bomb. When bombarded by neutrons, both ⁶Li and ⁷Li produce tritium. Tritium fuses with deuterium in a fusion reaction that is relatively easy to achieve. Although details remain secret, lithium apparently no longer plays a role in modern nuclear weapons, having been replaced entirely for the purpose by elemental tritium, which is lighter and easier to handle than lithium salts. ^{[citation needed]}
• Lithium is used as a source for alpha particles, or helium nuclei. When ⁷Li is bombarded by accelerated protons, ⁸Be is formed, which undergoes spontaneous fission to form two alpha particles. This was the first man-made nuclear reaction, produced by Cockroft and Walton in 1929.
• Lithium hydroxide (LiOH) is an important compound of lithium obtained from lithium carbonate (Li₂CO₃). It is a strong base, and when heated with a fat, it produces a lithium soap. Lithium soap has the ability to thicken oils and so is used commercially to manufacture lubricating greases.
• Lithium metal is used as a catalyst in some types of methamphetamine production, particularly in illegal amateur “meth labs.”
• Lithium hydroxide is an efficient and lightweight purifier of air. In confined areas, such as aboard spacecraft and submarines, the concentration of carbon dioxide can approach unhealthy or toxic levels. Lithium hydroxide absorbs the carbon dioxide from the air by reacting with it to form lithium carbonate. Any alkali hydroxide will absorb CO₂, but lithium hydroxide is preferred because of its low atomic weight. Even better materials for this purpose include lithium peroxide (Li₂O₂) and lithium superoxide (LiO₂) that, in presence of moisture, not only absorb carbon dioxide to form lithium carbonate, also release oxygen. E.g. 4 LiO₂ + 2CO₂ —> 2Li₂CO₃ + 3 O₂.

Market trend

Prices of lithium carbonate rose by 20% in 2005 and growth of up to 25% is forecast by Roskill Consulting Group for 2006, bringing prices back to the peak levels seen prior to SQM's entry into the market in 1996. New capacity due on-stream in Chile, Argentina and China is forecast to alleviate the upward pressure on prices after 2007.

Consumption of lithium increased by 4-5% per year between 2002 and 2005, driven by demand in lithium secondary batteries. Batteries accounted for 20% of total consumption in 2005, a rise from under 10% in 2000.

Continued expansion in the portable electronic products market and commercialisation of hybrid electric vehicles using lithium batteries suggest growth of up to 10% per year in lithium carbonate consumption in this market through 2010.

Between 2002 and 2005, lithium minerals production rose by 7% per year to reach 18,800 tonnes Li. Chile and Australia account for over 60% of total output. FMC Lithium of the USA, Chemetall of Germany and SQM of Chile continue to dominate production of downstream lithium chemicals.

China may emerge as a significant producer of brine-based lithium carbonate towards the end of this decade. Potential capacity of up to 45,000 tonnes per year could come on-stream if projects in Qinghai province and Tibet proceed. [1]

Regulation

Some jurisdictions limit the sale of lithium batteries, which are the most readily available source of lithium metal for ordinary consumers. Lithium can be used to reduce pseudoephedrine and ephedrine to methamphetamine in the Birch reduction method, which employs solutions of alkali metals dissolved in anhydrous ammonia. However, the effectiveness of such restrictions in controlling illegal production of methamphetamine remains indeterminate and controversial.

Carriage and shipment of some kinds of lithium batteries may be prohibited aboard certain types of transportation (particularly aircraft), because of the ability of most types of lithium batteries to fully discharge very rapidly when short-circuited, leading to overheating and possible explosion. However, most consumer lithium batteries have thermal overload protection built-in to prevent this type of incident, or their design inherently limits short-circuit currents.

Lithium application in nuclear weapons industry is now strongly pursued in developing countries like India.

Lithium ion (salts) for medical use

See also John Cade

Lithium carbonate (Li₂CO₃) has been used since the 1960’s for treatment of those who suffer from the psychological disorder of manic depression or bipolar affective disorder. The active principle in these salts is the lithium ion Li⁺, which interacts with the normal function of sodium ion to product numerous changes in the neurotransmitter activity of the brain.

See also

• Lithium compounds

References

ISBN links support NWE through referral fees

Book references

• Stwertka, Albert (2002). A Guide to the Elements. New York, NY: Oxford University Press. ISBN 0195150279. 
• Krebs, Robert E. (1998). The History and Use of Our Earth's Chemical Elements : A Reference Guide. Westport, Conn.: Greenwood Press. ISBN 0313301239. 
• Newton, David E. (1994). The Chemical Elements. New York, NY: Franklin Watts. ISBN 0531125017. 

External links

• USGS: Lithium Statistics and Information
• WebElements.com – Lithium
• It's Elemental – Lithium

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