LITHIUM METAL

LITHIUM METAL = METALLIC LITHIUM 

CAS-No. : 7439-93-2
EC-No. : 231-102-5
MDL number: MFCD00134051
Formula : Li

Lithium is a chemical element with the symbol Li and atomic number 3. 
Lithium metal is a soft, silvery-white alkali metal. 
Lithium is the lightest solid element in the periodic table. 
Under standard conditions, Lithium metal is the least dense metal and the least dense solid element. 
Like all alkali metals, lithium is highly reactive, and must be stored in vacuum, inert atmosphere or inert liquid such as purified kerosene or mineral oil. 

When cut, Lithium metal exhibits a metallic luster, but moist air corrodes Lithium metal quickly to a dull silvery gray, then black tarnish. 
Lithium metal 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 Lithium metal's solubility as an ion, Lithium metal 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.
Lithium is usually available in various concentration. 

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 lithium's relative nuclear instability, lithium is less common in the solar system than 25 of the first 32 chemical elements even though lithium's nuclei are very light: lithium is an exception to the trend that heavier nuclei are less common. 
For related reasons, lithium has important uses in nuclear physics. 
The alkali metals are also called the lithium family, after its leading element. 

Like the other alkali metals (which are sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr)), lithium has a single valence electron that is easily given up to form a cation. 
Because of this, lithium is a good conductor of heat and electricity as well as a highly reactive element, though it is the least reactive of the alkali metals. 
Lithium's low reactivity is due to the proximity of its valence electron to its nucleus. 
Molten lithium is significantly more reactive than its solid form.
Lithium metal is soft enough to be cut with a knife. 

When cut, Lithium metal possesses a silvery-white color that quickly changes to gray as it oxidizes to lithium oxide. 
Lithium metal's melting point of 180.50 °C (453.65 K; 356.90 °F) and Lithium metal's boiling point of 1,342 °C (1,615 K; 2,448 °F) are each the highest of all the alkali metals while Lithium metal's density of 0.534  g/cm3 is the lowest.
Lithium has a very low density (0.534 g/cm3), comparable with pine wood. 
Lithium is the least dense of all elements that are solids at room temperature; the next lightest solid element (potassium, at 0.862 g/cm3) is more than 60% denser. 

Apart from helium and hydrogen, as a solid Lithium is less dense than any other element as a liquid, being only two-thirds as dense as liquid nitrogen (0.808 g/cm3). 
Lithium can float on the lightest hydrocarbon oils and is one of only three metals that can float on water, the other two being sodium and potassium
Lithium's coefficient of thermal expansion is twice that of aluminium and almost four times that of iron. 
Lithium is superconductive below 400 μK at standard pressure and at higher temperatures (more than 9 K) at very high pressures (>20 GPa). 

At temperatures below 70 K, lithium, like sodium, undergoes diffusionless phase change transformations. 
At 4.2 K Lithium has a rhombohedral crystal system (with a nine-layer repeat spacing); at higher temperatures Lithium transforms to face-centered cubic and then body-centered cubic. 
At liquid-helium temperatures (4 K) the rhombohedral structure is prevalent. 
Multiple allotropic forms have been identified for lithium at high pressures.
Lithium reacts with water easily, but with noticeably less vigor than other alkali metals. 

The reaction forms hydrogen gas and lithium hydroxide. 
When placed over a flame, lithium compounds give off a striking crimson color, but when the metal burns strongly, the flame becomes a brilliant silver. 
Lithium will ignite and burn in oxygen when exposed to water or water vapor. 
In moist air, lithium rapidly tarnishes to form a black coating of lithium hydroxide (LiOH and LiOH·H2O), lithium nitride (Li3N) and lithium carbonate (Li2CO3, the result of a secondary reaction between LiOH and CO2). 
Lithium is one of the few metals that react with nitrogen gas.

Lithium has a diagonal relationship with magnesium, an element of similar atomic and ionic radius. 
Chemical resemblances between the two metals include the formation of a nitride by reaction with N2, the formation of an oxide (Li2O) and peroxide (Li2O2) when burnt in O2, salts with similar solubilities, and thermal instability of the carbonates and nitrides. 
The metal reacts with hydrogen gas at high temperatures to produce lithium hydride (LiH).
The unique properties of lithium metal allow it to be used in various applications. 
Lithium has an atomic number of 3 and an atomic weight of 6.941. 

Lithium is slightly harder than sodium, but softer than lead, and is extremely light with a density of 0.531 g/cm3, or about half that of water. 
The wide range between the melting point of 180.5°C and the boiling point of 1336°C along with Lithium's excellent heat capacity makes lithium a good medium for heat sink or heat transfer applications. 
Lithium is also a strong reducing agent and reacts readily even with weak oxidizers-reacting with nitrogen at ambient temperature. 
Even though lithium is a powerful reducing agent in many reactions, Lithium is less reactive than the other elements in the alkali metals group.

Lithium metal batteries are one of the more promising alternatives to the lithium-ion architecture commonly used today, with the potential to hold many times the energy. 
The reason lithium-metal batteries hold so much promise is because they seek to use pure lithium metal as the anode material, which can hold as much as 10 times the energy of the graphite used today. 
But lithium metal is reactive and weak, making it extremely difficult to handle and integrate into batteries, especially using state-of-the-art manufacturing equipment.  
Lithium is the only alkali metal that reacts with nitrogen.

Lithium burns red in a flame test.
Lithium was first discovered in the mineral petalite (LiAlSi4O10).
Due to the abundance of lithium in nature, recycling of lithium was not a priority for the many players in the lithium-ion battery, glass, or ceramics industries. 
The recent increase in demand for lithium for electric vehicles has emphasized the importance of recycling and now  both pyrometallurgical and hydrometallurgical flowsheets can recycle lithium from Li-ion battery waste. 
Lithium is a special metal in many ways. 

Lithium's light and soft — so soft that Lithium can be cut with a kitchen knife and so low in density that Lithium floats on water. 
Lithium's also solid at a wide range of temperatures, with one of the lowest melting points of all metals and a high boiling point. 
Like its fellow alkali metal, sodium, lithium reacts with water in showy form. 
The combo of Li and H2O forms lithium hydroxide and hydrogen, which typically bursts into red flame. 

Lithium, as well as the first and second lightest chemical elements (hydrogen and helium, respectively), are the only
elements created at the birth of the universe, according to NASA. 
However, according to the Big Bang Theory, the universe should hold three times as much lithium as can be accounted for in the oldest stars, an issue called the missing lithium problem. 
The least reactive of the alkali metals, lithium is silvery-white, turning yellowish when exposed to moist air. 
Lithium metal does not occur free in nature, but is combined in most igneous rocks and in many mineral springs. 

Lithium has the highest specific heat of any solid element making Lithium metal useful in heat transfer applications. 
With a density only about half that of water, Lithium metal is the lightest solid element.
Lithium is a rare element found primarily in molten rock and saltwater in very small amounts. 
Lithium is understood to be non-vital in human biological processes, although Lithium is used in many drug treatments due to Lithium's positive effects on the human brain.

Lithium was first identified as a component of of the mineral petalite and was discovered in 1817 by Johan August Arfwedson, but not isolated until some time later by W.T. Brande and Sir Humphry Davy. 
In Lithium's mineral forms Lithium accounts for only 0.0007% of the earth's crust. 
Lithium compounds are used in certain kinds of glass and porcelain products. 
More recently lithium has become important in dry-cell batteries and nuclear reactors. 

Some compounds of lithium have been used to treat manic depressives.
Lithium is an alkali metal with the atomic number = 3 and an atomic mass of 6.941 g/mol. 
This means that lithium has 3 protons, 3 electrons and 4 neutrons (6.941 - 3 = ~4). 
Being an alkali metal, lithium is a soft, and highly reactive metal that tends to form hydroxides. 
Lithium also has a pretty low density and under standard conditions, Lithium is the least dense solid element.

Lithium metal is a silvery-shiny material and Lithium metal is the lightest of all metals, with only half the weight of water. 
Like many other elements, lithium metal reacts with air, but opposite to most of those hardly with oxygen, but preferably with nitrogen. 
Thereby Lithium metal quickly forms lithium nitride, Li3N, which makes a dark layer on the otherwise light silver surface. 

USES and APPLICATIONS OF LITHIUM METAL:
-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; Lithium's functions are uncertain. 
Lithium salts have proven to be useful as a mood stabilizer and antidepressant in the treatment of mental illness such as bipolar disorder.

-Lithium has a mass specific heat capacity of 3.58 kilojoules per kilogram-kelvin, the highest of all solids. 
Because of this, lithium metal is often used in coolants for heat transfer applications.
-Because of its reactivity with water, and especially nitrogen, lithium metal is usually stored in a hydrocarbon sealant, often petroleum jelly. 
Although the heavier alkali metals can be stored under mineral oil, lithium is not dense enough to fully submerge itself in these liquids.

-Most lithium is used to make lithium-ion batteries for electric cars and mobile devices.
-Lithium oxide is widely used as a flux for processing silica, reducing the melting point and viscosity of the material and leading to glazes with improved physical properties including low coefficients of thermal expansion. 
Worldwide, this is one of the largest use for lithium compounds. 
Glazes containing lithium oxides are used for ovenware. 
Lithium carbonate (Li2CO3) is generally used in this application because Lithium carbonate converts to the oxide upon heating.

-Lithium became an important component of battery electrolytes and electrodes, because of its high electrode potential. Because of Lithium's low atomic mass, Lithium has a high charge- and power-to-weight ratio. 
A typical lithium-ion battery can generate approximately 3 volts per cell, compared with 2.1 volts for lead-acid and 1.5 volts for zinc-carbon. 
Lithium-ion batteries, which are rechargeable and have a high energy density, differ from lithium batteries, which are disposable (primary) batteries with lithium or its compounds as the anode. 
Other rechargeable batteries that use lithium include the lithium-ion polymer battery, lithium iron phosphate battery, and the nanowire battery.

-The third most common use of lithium is in greases. 
Lithium hydroxide is a strong base and, when heated with a fat, produces a soap made of lithium stearate. 
Lithium soap has the ability to thicken oils, and it is used to manufacture all-purpose, high-temperature lubricating greases.
-Lithium (e.g. as lithium carbonate) is used as an additive to continuous casting mould flux slags where Lithium increases fluidity, a use which accounts for 5% of global lithium use. 
Lithium compounds are also used as additives (fluxes) to foundry sand for iron casting to reduce veining.

-Lithium (as lithium fluoride) is used as an additive to aluminium smelters (Hall–Héroult process), reducing melting temperature and increasing electrical resistance, a use which accounts for 3% of production.
-When used as a flux for welding or soldering, metallic lithium promotes the fusing of metals during the process and eliminates the forming of oxides by absorbing impurities. 
Alloys of the metal with aluminium, cadmium, copper and manganese are used to make high-performance, low density aircraft parts.

-Lithium has been found effective in assisting the perfection of silicon nano-welds in electronic components for electric batteries and other devices.
-Lithium compounds are used as pyrotechnic colorants and oxidizers in red fireworks and flares.
-Lithium chloride and lithium bromide are hygroscopic and are used as desiccants for gas streams. 
Lithium hydroxide and lithium peroxide are the salts most used in confined areas, such as aboard spacecraft and submarines, for carbon dioxide removal and air purification. 
Lithium hydroxide absorbs carbon dioxide from the air by forming lithium carbonate, and is preferred over other alkaline hydroxides for its low weight.

-Metallic lithium and its complex hydrides, such as Li[AlH4], are used as high-energy additives to rocket propellants. Lithium aluminum hydride can also be used by itself as a solid fuel.
-The Mark 50 torpedo stored chemical energy propulsion system (SCEPS) uses a small tank of sulfur hexafluoride, which is sprayed over a block of solid lithium. 
The reaction generates heat, creating steam to propel the torpedo in a closed Rankine cycle.
-Lithium is useful in the treatment of bipolar disorder. 
Lithium salts may also be helpful for related diagnoses, such as schizoaffective disorder and cyclic major depression. 
The active part of these salts is the lithium ion Li+.

-Lithium Metal is available as disc, granules, ingot, pellets, pieces, powder , rod, wire, and sputtering target.
-Lithium is used in heat transfer applications. 
-Lithium is used as an alloying agent, in synthesizing organic compounds, and is added to glasses and ceramics. 
-Lithium's high electrochemical potential makes Lithium useful for battery anodes. 
-Lithium chloride and lithium bromide are highly hygroscopic, so they are used as drying agents. 

-Lithium stearate is used as a high-temperature lubricant. 
-Lithium has medical applications as well.
-Lithium is used extensively in rechargeable battery technology.
-Lithium is used to create the hydrogen isotope tritium through bombardment of neutrons.
-Lithium metal is widely used for Li-ion rechargeable battery R&D.

-The Li-ion battery industry is the largest consumer of lithium worldwide, mainly for the production of active cathode materials, where lithium is used in the form of highly pure lithium carbonate or hydroxide. 
Such batteries power portable devices such as smartphones, tablets, laptops, as well as  electric mobility including electric cars, hybrid vehicles, electric bikes, etc. 
-The third market segment for lithium-ion batteries is Energy Storage Systems. 
-Besides the Li-ion battery industry, lithium has been used for many years in other, more traditional applications such as glass and ceramics, in mold flux powders and in aluminum smelting. 

-Other applications that consume lithium are greases for mechanical systems (e.g gearboxes), catalysts for rubber synthesis (butyllithium), aluminum alloys for airplanes, air cooling systems (lithium bromide) and antidepressants. 
-Lithium metal's used in the manufacture of aircraft and in certain batteries. 
-Lithium metal's also used in mental health: Lithium carbonate is a common treatment of bipolar disorder, helping to stabilize wild mood swings caused by the illness. 
-Lithium-ion batteries are the key to lightweight, rechargeable power for laptops, phones and other digital devices. 

-Aerospace alloys, automobile alloys, battery anodes, catalysts, oxidant/ degasser, precursor.
-When Lithium metal reacts in batteries, the electric charge Lithium metal gives off is of a high voltage which is why these are a preferred metal in many single use and rechargeable power cells. 
-Lithium metal can also be combined with other metals to produce lightweight and strong alloys.
-The element Lithium is also used in medical applications as a mood stabilizer as well as serving many other functions.
-Lithium is able to be used in the function of a Lithium battery in which the Lithium metal serves as the anode. 
Lithium ions serve in lithium ion batteries (chargeable) in which the lithium ions move from the negative to positive electrode when discharging, and vice versa when charging.

-Lithium has the highest specific heat capacity of the solids, Lithium tends to be used as a cooler for heat transfer techniques and applications.
-Lithium metal is often used in disposable and rechargeable batteries, while lithium salts are used in medicine as treatment for mental disorders. 
-Lithium is used in the nuclear field and in the pharmaceutical industry for the vitamin C synthesis. 
-Lithium is also applied in the glass, ceramic and plastic industries.

SOURCES and EXTRACTION OF LITHIUM METAL;
Lithium is most commonly found combined with aluminum, silicon, and oxygen to form the minerals known as spodumene (LiAl(SiO3)2) or petalite/castorite (LiAlSi4O10). These have been found on each of the 6 inhabited continents, but they are mined primarily in Western Australia, China, and Chile. Mineral sources of lithium are becoming less essential, as methods have now been developed to make use of the lithium salts found in saltwater.

LITHIUM SOURCES:
Lithium does not occur free in nature. 
Lithium is found in small amounts in practically all igneous rocks and in the waters of mineral springs. 
The minerals that contain lithium include lepidolite, petalite, amblygonite, and spodumene. 
Lithium metal is produced electrolytically from the fused chloride.

EXTRACTION FROM MINERALS OF LITHIUM METAL:
The mineral forms of lithium are heated to a high enough temperature (1200 K - 1300 K) in order to crumble them and thus allow for subsequent reactions to more easily take place. 
After this process, one of three methods can be applied.
-The use of sulfuric acid and sodium carbonate to allow the iron and aluminum to precipitate from the ore - from there, more sodium carbonate is applied to the remaining material allow the lithium to precipitate out, forming lithium carbonate. 
This is treated with hydrochloric acid to form lithium chloride.

-The use of limestone to calcinate the ore, and then leaching with water, forming lithium hydroxide. 
Again, this is treated with hydrochloric acid to form lithium chloride.
-The use of sulfuric acid, and then leaching with water, forming lithium sulfate monohydrate. 
This is treated with sodium carbonate to form lithium carbonate, and then hydrochloric acid to form lithium chloride.
The lithium chloride obtained from any of the three methods undergoes an oxidation-reduction reaction in an electrolytic cell, to separate the chloride ions from the lithium ions. 
The chloride ions are oxidized, and the lithium ions are reduced.

EXTRACTION FROM SALTWATER OF LITHIUM METAL:
Saltwater naturally contains lithium chloride, which must be extracted in the form of lithium carbonate, then it is re-treated, separated into its ions, and reduced in the same electrolytic process as in extraction from lithium ores. 
Only three saltwater lakes in the world are currently used for lithium extraction, in Nevada, Chile, and Argentina.
Saltwater is channeled into shallow ponds and over a period of a year or more, water evaporates out to leave behind various salts. 
Lime is used to remove the magnesium salt, so that the remaining solution contains a fairly concentrated amount of lithium chloride. 
The solution is then treated with sodium carbonate in order for usable lithium carbonate to precipitate out.

PHYSICAL and CHEMICAL PROPERTIES of LITHIUM METAL:
Molecular weight : 6,94 g/mol
Appearance Form: granular
Odor: No data available
Odor Threshold: No data available
pH: No data available
Melting point/freezing point:
Melting point/range: 180 °C - lit.

Initial boiling point and boiling range: 1.342 °C - lit.
Flash point: Not applicable
Evaporation rate: No data available
Flammability (solid, gas): No data available
Upper/lower flammability or explosive limits: No data available
Vapor pressure: 1 hPa at 723 °C
Vapor density: No data available
Density: 0,534 g/mL at 25 °C - lit.
Relative density: No data available

Water solubility: No data available
Partition coefficient: n-octanol/water: No data available
Autoignition temperature: No data available
Decomposition temperature: No data available
Viscosity 
Viscosity, kinematic: No data available
Viscosity, dynamic: 0,57 mPa.s at 200 °C
Explosive properties: No data available
Oxidizing properties: none
Electrical Resistivity:    8.55 microhm-cm @ 0 °C
Electronegativity: 1.0 Paulings

Heat of Fusion: 1.10 Cal/gm mole;
Heat of Vaporization: 32.48 K-Cal/gm atom at 1342 °C
Specific Heat: 0.85 Cal/g/K @ 25 °C
Tensile Strength: N/A
Thermal Conductivity: 0.848 W/cm/K @ 298-C.2 K
Thermal Expansion: (25 °C) 46 µm·m-1·K-1
Vickers Hardness: N/A

Young's Modulus: 4.9 GPa
Appearance: solid
Color: metallic
Melting point/ range: 180.5 °C at 1,013 hPa
Viscosity, dynamic: 0.57 mPa*s at 200 °C
Boiling point/boiling range ca.: 1,342 °C at 1,013 hPa
Density: 0.534 g/cm3 at 20 °C
Bulk density ca.: 300 kg/m3 

Appearance: soft, silvery-white metal
Isotopes: 8 isotopes [Li-4 to Li-11]. Li-6 (7.59% abundance) and Li-7 (92.41% abundance) are both stable.
Atomic Radius (pm): 155
Atomic Volume (cc/mol): 13.1
Covalent Radius (pm): 163
Ionic Radius: 68 (+1e)
Specific Heat (@20°C J/g mol): 3.489
Fusion Heat (kJ/mol): 2.89

Evaporation Heat (kJ/mol): 148
Debye Temperature (°K): 400.00
Pauling Negativity Number: 0.98
First Ionizing Energy (kJ/mol): 519.9
Oxidation States: 1
Lattice Structure: Body-Centered Cubic
Lattice Constant (Å): 3.490
Magnetic Ordering: paramagnetic
Electrical Resistivity (20°C): 92.8 nΩ·m

Thermal Conductivity (300 K): 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
Young's Modulus: 4.9 GPa
Shear Modulus: 4.2 GPa
Bulk Modulus: 11 GPa
Mohs Hardness: 0.6
Solubility: Lithium dissolves slowly in diluted acids.

ADDITIONAL PHYSICAL PROPERTIES of METALLIC LITHIUM :
401513 Lithium trapezoid ingot of 1,000 g,: 258/284 x 65/90 x 90 mm
401510 Lithium trapezoid ingot of 850 g,: 258/283 x 65/89 x 83 mm
401515 Lithium trapezoid ingot of 430 g,: 126/148 x 65/85 x 81 mm
401503 Lithium trapezoid ingot of 180 g,: 126/137 x 65/76 x 65 mm
401511 Blocks of 100 g,: 165 x 34 x 34 mm
401505 Rods, 10 and 20 mm Ø,: length 250 mm
401514 Granulate,: about Ø 2.5 mm
401518 Pieces: about Ø 10 mm, length 5 mm

FIRST AID MEASURES of METALLIC LITHIUM:
-Description of first-aid measures
*General advice
First aiders need to protect themselves. 
Show this material safety data sheet to the doctor in attendance.
*If inhaled
After inhalation: 
Fresh air. 
Call in physician.
*In case of skin contact: 
Take off immediately all contaminated clothing. 
Rinse skin with water/ shower. 
Call a physician immediately.
*In case of eye contact:
After eye contact: 
Rinse out with plenty of water. 
Immediately call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing: 
Make victim drink water (two glasses at most), avoid vomiting.
Call a physician immediately. 
Do not attempt to neutralise.

ACCIDENTAL RELEASE MEASURES of METALLIC LITHIUM:
-Personal precautions, protective equipment and emergency procedures
Advice for non-emergency personnel: 
Avoid inhalation of dusts. 
Avoid substance contact.
Ensure adequate ventilation. 
-Environmental precautions
Do not let product enter drains. 
-Methods and materials for containment and cleaning up
Cover drains. 
Collect, bind, and pump off spills. 
Observe possible material restrictions. 
Take up dry. 
Dispose of properly. 
Clean up affected area. 
Avoid generation of dusts.

FIREFIGHTING MEASURES of METALLIC LITHIUM:
-Extinguishing media:
Suitable extinguishing media:
Extinguishing media: 
Sodium chloride/hydrogen carbonate or lime stone. 
Special powder against metal fire.
Unsuitable extinguishing media:
Foam Water

-Advice for firefighters
Stay in danger area only with self-contained breathing apparatus. 
Prevent skin contact by keeping a safe distance or by wearing suitable protective clothing.
-Further information:
Prevent fire extinguishing water from contaminating surface water or the ground water system.

EXPOSURE CONTROLS/PERSONAL PROTECTION of METALLIC LITHIUM:
-Control parameters:
Ingredients with workplace control parameters:
-Exposure controls:
Personal protective equipment:

*Eye/face protection:
Use equipment for eye protection tested and approved under appropriate government standards such as NIOSH (US) or EN 166(EU). Tightly fitting safety goggles.
*Skin protection:
This recommendation applies only to the product stated in the safety data sheet, supplied by us and for the designated use. When dissolving in or mixing with other substances and under conditions deviating from those stated in EN374 please
contact the supplier of CE-approved gloves.
Full contact
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min

*Body Protection:
Protective clothing
*Respiratory protection:
Required when dusts are generated.
Our recommendations on filtering respiratory protection are based on the following standards: DIN EN 143, DIN 14387 and other accompanying standards relating to the used respiratory protection system.
Recommended Filter type: Filter type P2
The entrepeneur has to ensure that maintenance, cleaning and testing of respiratory protective devices are carried out according to the instructions of the producer.
These measures have to be properly documented.
*Control of environmental exposure:
Do not let product enter drains. 

HANDLING and STORAGE of METALLIC LITHIUM:
-Precautions for safe handling:
Advice on safe handling:
Keep workplace dry. 
Do not allow product to come into contact with water.
Hygiene measures:
Immediately change contaminated clothing. 
Apply preventive skin protection. 
Wash hands and face after working with substance.
Handling: 
Lithium can be stored min. six months under exclusion of air and humidity (oil cover or argon atmosphere) in approved packing. 

-Conditions for safe storage, including any incompatibilities
Storage conditions:
Store under argon. 
Tightly closed. 

SYNONYMS:
Lithium element 
Lithium atom
Lithium metal 
Lithium granules
Lithium shot
Lithium ingot
Lithium foil 
Lithium wire 
Lithium rod