|Classification||Lithium is an alkali metal|
|Melting point||180.54 oC, 453.69 K|
|Boiling point||1347 oC, 1615 K|
|Neutrons in most abundant isotope:||4|
|Electron configuration||1s2 2s1|
|Density @ 20oC||0.53 g/cm3|
|Atomic volume||13.10 cm3/mol|
|Structure||bcc body-centered cubic|
|Specific heat capacity||3.58 J g-1 K-1|
|Heat of fusion||3.00 kJ mol-1|
|Heat of atomization||159 kJ mol-1|
|Heat of vaporization||147.1 kJ mol-1|
|1st ionization energy||520.2 kJ mol-1|
|2nd ionization energy||7298.1 kJ mol-1|
|3rd ionization energy||11815.0 kJ mol-1|
|Electron affinity||59.63 kJ mol-1|
|Minimum oxidation number||-1|
|Min. common oxidation no.||0|
|Maximum oxidation number||1|
|Max. common oxidation no.||1|
|Electronegativity (Pauling Scale)||0.98|
|Polarizability volume||24.3 Å3|
|Reaction with air||vigorous,⇒ Li2O|
|Reaction with 15 M HNO3||vigorous,⇒ LiNO3|
|Reaction with 6 M HCl||vigorous,⇒ H2, LiCl|
|Reaction with 6 M NaOH||mild, ⇒ H2, LiOH|
|Atomic radius||145 pm|
|Ionic radius (1+ ion)||90 pm|
|Ionic radius (2+ ion)||–|
|Ionic radius (3+ ion)||–|
|Ionic radius (1- ion)||–|
|Ionic radius (2- ion)||–|
|Ionic radius (3- ion)||–|
|Thermal conductivity||84.8 W m-1 K-1|
|Electrical conductivity||11.7 x 106 S m-1|
|Freezing/Melting point:||180.54 oC, 453.69 K|
Discovery of Lithium
Lithium was discovered by Johan Arfvedson in 1817 in Stockholm, Sweden, during an analysis of petalite (LiAlSi4O10).
He found the petalite contained “silica, alumina and an alkali.” (1)
The new alkali metal in the petalite had unique properties.
It required more acid to neutralize it than sodium and its carbonate was only sparingly soluble in water – unlike sodium carbonate.
The new alkali differed from potassium because it did not give a precipitate with tartaric acid.
Arfvedson tried to produce a pure sample of the new metal by electrolysis, but he was unsuccessful; the battery he used was not powerful enough. (2)
The pure metal was isolated the following year by both Swedish chemist William Brande and English chemist Humphry Davy working independently.
Davy obtained a small quantity of lithium metal by electrolysis of lithium carbonate. (3)
He noted the new element had a red flame color somewhat like strontium and produced an alkali solution when dissolved in water.
In days less safety-conscious than the present, Brande said of lithium, “its solution tastes acrid like the other fixed alkalies.” (4)
By 1855 Robert Bunsen and Augustus Matthiessen were independently producing the metal in large quantities by electrolysis of molten lithium chloride.
Lithium’s name is derived from the Greek word ‘lithos’ meaning, ‘stone.’
Interesting Facts about Lithium
- Lithium is believed to be one of only three elements – the others are hydrogen and helium – produced in significant quantities by the Big Bang. Synthesis of these elements took place within the first three minutes of the universe’s existence.
- Lithium is the only alkali metal that reacts with nitrogen.
- Humphrey Davy produced some of the world’s first lithium metal from lithium carbonate. Today lithium carbonate – or more precisely the lithium ions in lithium carbonate – are used to inhibit the manic phase of bipolar (manic-depressive) disorder.
- Lithium based batteries have revolutionized consumer devices such as computers and cell phones. For a given battery weight, lithium batteries deliver more energy than batteries based on other metals; in other words, lithium batteries have high energy density.
Appearance and Characteristics
Lithium is corrosive, causing skin burns as a result of the caustic hydroxide produced in contact with moisture. Women taking lithium carbonate for bi-polar disorder may be advised to vary their treatment during pregnancy as lithium may cause birth defects.
Lithium is soft and silvery white and it is the least dense of the metals. It is highly reactive and does not occur freely in nature.
Lithium burns with a crimson flame, but when the metal burns sufficiently well, the flame becomes a brilliant white.
Lithium has a high specific heat capacity and it exists as a liquid over a wide temperature range.
Uses of Lithium
Lithium also has various nuclear applications, for example as a coolant in nuclear breeder reactors and a source of tritium, which is formed by bombarding lithium with neutrons.
Lithium carbonate is used as a mood-stabilizing drug.
Lithium chloride and bromide are used as desiccants.
Lithium stearate is used as an all-purpose and high-temperature lubricant.
Abundance and Isotopes
Abundance earth’s crust: 20 parts per million by weight, 60 parts per million by moles
Abundance solar system: 60 parts per trillion by weight, 10 parts per trillion by moles
Cost, pure: $27 per 100g
Cost, bulk: $9.50 per 100g
Source: Lithium does not occur as a free element in nature. It is found in small amounts in ores from igneous rocks and in salts from mineral springs. Pure lithium metal is produced by electrolysis from a mixture of fused (molten) lithium chloride and potassium chloride.
Isotopes: Lithium has 7 isotopes whose half-lives are known, with mass numbers 5 to 11. Naturally occurring lithium is a mixture of its two stable isotopes 6Li and 7Li with natural abundances of 7.6% and 92.4% respectively.
1. Thomas Thomson, A system of chemistry of inorganic bodies, 1831, Volume 1
2. Mary Elvira Weeks, Discovery of the Elements., 2003, p125 Kessinger Publishing.
3. Royal Institution of Great Britain, The Quarterly Journal of Science and the Arts, Volume 5, 1818 p338. (pdf)
4. William Thomas Brande, William James MacNeven A manual of chemistry (1821) p191. (pdf)
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