Lithium



Symbol-Li



History- Johan August Arfvedson in Stockholm, Sweden in 1817



Lithium was first discovered and defined by J.A. Arfvedson in 1817 when he did an analysis of a mineral he found.



Atomic number-3



Atomic mass-6.94



Melting point- 453.74 K boiling point- 1620 K



Density in natural state- 0.53 g/cm3



Natural abundance-92.5%



It is found in spodumene, ambylgonite, lepidolite, and desert lake brines.



Obtained by passing electric charge through melted lithium chloride.



Structure

#Atomic Radius: 2.05Å

Atomic Volume: 13.1cm3/mol

Covalent Radius: 1.23Å

Cross Section: 71barns

Crystal Structure: Cubic body centered

Electron Configuration: 1s2 2s1

Electrons per Energy Level: 2,1

Ionic Radius: 0.76Å

Filling Orbital: 2s 1

Number of Electrons (with no charge): 3

Number of Neutrons (most common/stable nuclide): 4

Number of Protons: 3 Oxidation States: 1

Valance Electrons: 2s 1

List of isotopes- 6Li and 7Li



Chemical properties/reaction tendencies

Reaction of lithium with air

The silvery surface tarnishes because of reaction with oxygen and moisture from the air. When lithium is burned in air, the main product is the white oxide lithium oxide, Li2O.

4Li(s) + O2(g) 2Li2O(s)

2Li(s) + O2(g) 2Li2O2(s)



Reaction of lithium with water

Lithium metals reacts slowly with water to form a colourless solution of lithium hydroxide (LiOH) and hydrogen gas (H2).

2Li(s) + 2H2O 2LiOH(aq) + H2(g)



Reaction of lithium with the halogens

Lithium metal reacts with all the halogens to form lithium halides.

2Li(s) + F2(g) LiF(s)

2Li(s) + Cl2(g) LiCl(s)

2Li(s) + Br2(g) LiBr(s)

2Li(s) + I2(g) LiI(s)



Reaction of lithium with acids

Lithium metal dissolves readily in dilute sulphuric acid to form solutions containing the aquated Li(I) ion together with hydrogen gas, H2.

2Li(s) + H2SO4(aq) 2Li+(aq) + SO42-(aq) + H2(g)



Reaction of lithium with bases

Lithium metals reacts slowly with water to form a colourless solution of basic lithium hydroxide (LiOH) and hydrogen gas (H2).

2Li(s) + 2H2O 2LiOH(aq) + H2(g)



Common compounds

Lithium carbonate or lithium citrate are mood stabilizers.

Lithium chloride and lithium bromide are used as desiccants.

Lithium stearate is an all-purpose high-temperature lubricant.

Lithium hydroxide is used to extract carbon dioxide from the air.