Periodic Table

Lithium

Alkali Metal

Quick Facts about Lithium

He
  • solid- state of matter at room temperature
  • Stable- has at least one stable isotope
  • +1- common oxidation states in compounds
  • BCC- crystal structure, atomic arrangement in solid form
Be

Lithium (Li) is element 3 on the periodic table. Atomic mass of Li: 6.9400 u. Li is in period 2, group 1. Melting point of Li: 453.65 K.Density of Li: 0.53 g/cm³.

Why Lithium Matters

The lightest metal—powering your phone and treating your mood

In Your Home

  • Rechargeable batteries in phones, laptops, EVs
  • Some ceramics and glass
  • Lithium grease for machinery
  • Mood stabilizer medications

Industry Uses

EnergyLithium-ion batteries in EVs, phones, and grid storage
PharmaLithium carbonate for bipolar disorder treatment
AerospaceLithium-aluminum alloys for aircraft
NuclearLithium-6 for tritium production in fusion research

In Your Body

✗ Not essential

Not essential, but affects brain chemistry. Lithium medications stabilize mood by affecting neurotransmitter signaling. Trace amounts in drinking water may affect mental health.

Safety: Narrow therapeutic window—toxic at levels not much higher than therapeutic dose. Requires regular blood monitoring.

Discovery of Lithium

Discovered by Johann Arfwedson in Sweden, 1817

Name origin: Greek: lithos (stone).

History & Events

1817
Discovery
Johan August Arfwedson discovered lithium in petalite ore while analyzing minerals
1949
Psychiatric Use
John Cade discovered lithium's mood-stabilizing effects, revolutionizing bipolar treatment
1991
Li-ion Battery
Sony released the first commercial lithium-ion battery, enabling portable electronics revolution

About Lithium

Soft silvery metal. First member of group 1 of the periodic table. Lithium salts are used in psychomedicine.

Atomic Properties of Li

Atomic Number of Li
3
Atomic Mass of Li
6.9400 u
Electron Configuration
[He] 2s1
Electronegativity
0.98
Block
s-block
Group
1
Period
2

Physical Properties of Li

Phase (STP)
solid
Melting Point of Li
453.65 K
Boiling Point of Li
1603.00 K
Density of Li
0.5340 g/cm3

Thermal Properties

Heat of Fusion
2.89 kJ/mol
Heat of Vaporization
148.00 kJ/mol
Specific Heat
3.58 J/g·K
Molar Heat Capacity
24.86 J/mol·K
Thermal Conductivity
84.80 W/m·K

Atomic Radii

Calculated
145 pm
Covalent
133 pm
Van der Waals
182 pm
Metallic
123 pm

Common Misconceptions

Wrong:Lithium batteries contain metallic lithium.
Correct:Most 'lithium' batteries use lithium compounds (like LiCoO2). Only lithium primary batteries use lithium metal.
Wrong:Lithium is rare.
Correct:Lithium is fairly abundant (33 ppm in Earth's crust), but economically extractable deposits are limited.
Wrong:Lithium medications make you 'zombie-like'.
Correct:Properly dosed lithium stabilizes mood without sedation. Side effects are usually manageable.

Isotopes of Lithium

Lithium has 2 naturally occurring isotopes.

IsotopeAtomic Mass (u)AbundanceHalf-LifeDecay Mode
63Li (Li-6)Lithium-6 isotope6.0151228877.590%
73Li (Li-7)Lithium-7 isotope7.01600343792.41%

Data source: NIH PubChem (aggregated from IUPAC, NIST)

Isotope Applications

Isotopes of Lithium have important real-world applications in science and industry.

Industrial Applications

7Li, as hydroxide monohydrate (7LiOH•H2O), is used to maintain the pH level of the coolant used in pressurized water reactors in the nuclear power industry [39], [40]. Lithium plays a role in the construction of a thermonuclear bomb, which differs from a fission weapon in that it uses the energy released when two light atomic nuclei (i.e. deuterium (2H) and tritium (3H)) fuse to form helium and a high energy neutronvia this DT reaction. 6Li is used, in the form of 6Li deuteride (6Li 2H), as fusion fuel capable of producing tritium when bombarded with neutrons within the weapon via the reaction 6Li (n, 3H) 4He [41]. Li-based laboratory reagents have found their way into surface water and can be easily identified. Although a military secret in the 1950s, it is now known that substantial amounts of 6Li (normally having an isotopic abundance of 0.076) were removed from chemical reagents to be used in nuclear weapon development. Reagents containing the remaining lithium depleted in 6Li (having an isotopic abundance as low as 0.025) were sold to both chemical manufacturers and to laboratory chemists for their use [42]. The distinctive isotopic signature of depleted 6Li, having a n(7Li)/n(6Li) ratio of 39, compared to a ratio of 12 in naturally occurring terrestrial materials, enables easier detection of this lithium source in polluted waterways and the environment [35], [37].

Medical Applications

7Li is a decay product of the 10B (neutron, alpha) 7Li reaction, which has a peak value for room temperature neutrons. Brain tumor cells are typically found some 5 to 7 cm below the surface of the skull. After 10B has been introduced to or entered the tumor cells, a beam of neutrons of energy slightly above room temperature is introduced to the affected areas. The energy of these neutrons is reduced to room temperature by the time they react with the 10B, which then disintegrates into high energy charged particles (7Li and 4He), which deposit their kinetic energy in nearby (predominately cancerous) cells and destroys them. Any adjacent normal cells are unaffected [43].

Abundance

Earth's Crust
20.0 mg/kg
Seawater
180.00 μg/kg

Uses

Used in batteries. Also for certain kinds of glass and ceramics. Some is used in lubricants.

Sources

Obtained by passing electric charge through melted lithium chloride and from the silicate mineral called spodumene [LiAl(Si2O6)].

Geochemistry

Goldschmidt
litophile
Geochemical Class
alkali metal

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