7439-93-2

IUPAC Name: Lithium
Empirical Formula: Li
Molecular Weight: 6.941
EINECS: 231-102-5
Classification Code: Antimanic Agents; Antipsychotic Agents; Central Nervous System Agents; Central Nervous System Depressants; Mutation data; Psychotropic Drugs; Tranquilizing Agents
density 0.534 g/mL at 25 °C(lit.)
storage temp.: water-free area
form: wire
Water Solubility: REACTS
Stability: Stability Stable, but reacts violently with water. Store under oil.
Melting Point: 180 °C(lit.)
Boiling point: 1342 °C
Critical point: 3223 K, 67 MPa
Heat of fusion: 3.00 kJ/mol
Heat of vaporization: 147.1 kJmol
Specific heat capacity of Lithium (CAS NO.7439-93-2): (25 °C) 24.860 J/mol/K

Petalite (LiAlSi₄O₁₀, which is Lithium aluminium silicate) was first discovered in 1800 by the Brazilian chemist José Bonifácio de Andrada e Silva, who discovered this mineral in a mine on the island of Utö, Sweden. However, it was not until 1817 that Johan August Arfwedson, then working in the laboratory of the chemist Jöns Jakob Berzelius, detected the presence of a new element while analyzing petalite ore.This element formed compounds similar to those of sodium and potassium, though its carbonate and hydroxide were less soluble in water and more alkaline. Berzelius gave the alkaline material the name "lithos", from the Greek word λιθoς (transliterated as lithos, meaning "stone"), to reflect its discovery in a solid mineral, as opposed to sodium and potassium, which had been discovered in plant tissues. The name of this element was later standardized as "lithium". Arfwedson later showed that this same element was present in the minerals spodumene and lepidolite. In 1818, Christian Gmelin was the first man to observe that lithium salts give a bright red color in flame.However, both Arfwedson and Gmelin tried and failed to isolate the element from its salts. This element, lithium, was not isolated until 1821, when William Thomas Brande isolated the element by performing electrolysis on lithium oxide, a process that had previously been employed by the chemist Sir Humphry Davy to isolate the alkali metals potassium and sodium. Brande also described some pure salts of lithium, such as the chloride, and he performed an estimate of its atomic weight. In 1855, larger quantities of lithium were produced through the electrolysis of lithium chloride by Robert Bunsen and Augustus Matthiessen. The discovery of this procedure henceforth led to commercial production of lithium metal, beginning in 1923, by the German company Metallgesellschaft AG, which performed an electrolysis of a liquid mixture of lithium chloride and potassium chloride.

Because of its specific heat capacity, the highest of all solids, Lithium (CAS NO.7439-93-2) is often used in coolants for heat transfer applications.
In the later years of the 20th century Lithium became important as an anode material. Used in Lithium-ion batteries because of its high electrochemical potential, a typical cell can generate approximately 3 volts, compared with 2.1 volts for lead/acid or 1.5 volts for zinc-carbon cells. Because of its low atomic mass, it also has a high charge- and power-to-weight ratio.
 Lithium is also used in the pharmaceutical and fine-chemical industry in the manufacture of organolithium reagents, which are used both as strong bases and as reagents for the formation of carbon-carbon bonds. Organolithiums are also used in polymer synthesis as catalysts/initiators in anionic polymerization of unfunctionalised olefins. Lithium-6 is valued as a source material for tritium production and as a neutron absorber in nuclear fusion. Natural lithium contains about 7.5 percent lithium-6. Large amounts of lithium-6 have been produced by isotope separation for use in nuclear weapons. Lithium-7 gained interest for use in nuclear reactor coolants.
 Lithium salts were used during the 19th century to treat gout. Lithium salts such as lithium carbonate (Li₂CO₃), lithium citrate, and lithium orotate are mood stabilizers. They are used in the treatment of bipolar disorder since, unlike most other mood altering drugs, they counteract both mania and depression.  Lithium continues to be the gold standard for the treatment of bipolar disorder. It is also helpful for related diagnoses, such as schizoaffective disorder and cyclic major depression.

Reported in EPA TSCA Inventory.

A very dangerous fire hazard when exposed to heat or flame. The powder may ignite spontaneously in air. The solid metal ignites above 180°C. It will burn in oxygen, nitrogen, or carbon dioxide, and will continue to burn in sand or sodium carbonate. The use of most types of fire extinguishers (e.g., water, foam, carbon dioxide, halocarbons, sodium carbonate, sodium chloride, and other dry powders) may cause an explosion. Molten lithium is extremely reactive and attacks such otherwise inert materials as sand, concrete, and ceramics.
Explosive reaction with bromobenzene, carbon + lithium tetrachloroaluminate + sulfinyl chloride, diazomethane. Forms very friction- and impact-sensitive explosive mixtures with halogens (e.g., bromine, iodine (above 200°C)), halocarbons (e.g., bromoform, carbon tetrabromide, carbon tetrachloride, carbon tetraiodide, chloroform, dichloromethane, diiodomethane, fluorotrichloromethane, tetrachloroethylene, trichloroethylene, 1,1,2-trichloro-trifluoroethane).
Violent reaction with acetonitrile, sulfur, mercury (potentially explosive), metal oxides (e.g., chromium(III) oxide (at 185°C), molybdenum trioxide (at 180°C), niobium pentoxide (at 320°C), titanium dioxide (at 200–400°C), tungsten trioxide (at 200°C), vanadium pentoxide (at 394°C)), iron(II) sulfide (at 260°C), manganese telluride (at 230°C), hot water, bromine pentafluoride (may ignite with lithium powder), platinum (at about 540°C), trifluoromethyl hypofluorite (at about 170°C), arsenic, beryllium, maleic anhydride, carbides, carbon dioxide, carbon monoxide + water, chlorine, chromium, chromium trichloride, cobalt alloys, iron sulfide, diborane, manganese alloys, nickel alloys, nitric acid, nitrogen, organic matter, oxygen, phosphorus, rubber, silicates, NaNO₂, Ta₂O₅, Fe alloys, V, ZrCl₄, CHI₃, trifluoromethylhypofluorite.
Ignition on contact with carbon + sulfinyl chloride (when ground), nitric acid (becomes violent), viton poly(1,1-difluorethylene-hexafluoropropylene), chlorine tri- and penta-fluorides (hypergolic reaction), diborane (forms a complex that is pyrophoric), hydrogen (above 300°C).
Incandescent reaction with ethylene + heat, nitrogen + metal chlorides (e.g., chromium trichloride, zirconium tetrachloride, nitryl fluoride (at 200°C)). Incompatible with atmospheric gases, bromine pentafluoride, diazomethane, metal chlorides, metal oxides, nonmetal oxides.
When burned it emits toxic fumes of LiO₂ and hydroxide. Reacts vigorously with water or steam to produce heat and hydrogen. Can react vigorously with oxidizing materials. To fight fire, use special mixtures of dry chemical, soda ash, graphite. NOTE: Water, sand, carbon tetrachloride, and carbon dioxide are ineffective.
Hazard Codes  Xi,C,F
Risk Statements  36/38-34-14/15-23 
R36/38:Irritating to eyes and skin. 
R34:Causes burns. 
R14 :Reacts violently with water. 
R15:Contact with water liberates extremely flammable gases. 
R23 :Toxic by inhalation.
Safety Statements  8-43-45-43C-36/37/39-26 
S8:Keep container dry. 
S43:In case of fire use ... (there follows the type of fire-fighting equipment to be used.) 
S45:In case of accident or if you feel unwell, seek medical advice immediately (show the label whenever possible.) 
S36/37/39:Wear suitable protective clothing, gloves and eye/face protection. 
S26: In case of contact with eyes, rinse immediately with plenty of water and seek medical advice.
RIDADR  UN 3264 8/PG 3
WGK Germany  2
RTECS  OJ5540000
F  10
HazardClass  4.3
PackingGroup  I

DOT Classification:  4.3; Label: Dangerous When Wet

For occupational chemical analysis use NIOSH: Elements (ICP), 7300.

  Lithium (CAS NO.7439-93-2), its Synonyms are Lithium, elemental ; Lithium, metallic . It is soft silvery metal that is normally grayish white due to oxide formation. Spontaneous ignition is likely if heated to melting point.