Lithium

Lithium is an alkali metal with the atomic number 3 and an atomic mass of 6.941 g/mol. It consists of 3 protons, 3 electrons, and approximately 4 neutrons. Lithium is an alkali metal characterised by its softness, flammability, and high reactivity, readily forming hydroxides. Its low density makes it the least dense solid element at standard conditions.

1.0Introduction 

Lithium was first discovered in the mineral petalite by Johan August Arfwedson in 1817, with Sir Humphry Davy and W.T. Brande later isolating the element. Though rare, lithium constitutes about 0.0007% of the Earth's crust in its mineral form. Its compounds have long been used in specific types of glass and porcelain. In recent years, lithium has gained increased importance for its role in dry-cell batteries and nuclear reactors. Additionally, certain lithium compounds are prescribed to treat bipolar disorder.

2.0Physical Properties of Lithium

3.0Chemical Properties Of Lithium

Because of its  reactivity, lithium reacts both with organic and inorganic substances. Because of its placement in Group 1 of the periodic table, lithium has a high degree of reactivity, particularly when it comes to non-metals like oxygen, nitrogen, and halogens, as seen by the following reactions.

• Reaction with Air: Lithium burns bright red when it comes into contact with air (O₂); the main byproduct is lithium monoxide.(Li₂O).

           4Li + O₂ -> 2Li₂O

• Reaction with Acids: Lithium oxide (LiO) and acids such as hydrochloric acid (HCl) combine to produce water and lithium chloride (LiCl).

           Li₂O → 2LiCl + H₂O + 2HCl

• Reaction with Water: Lithium hydroxide (LiOH) and hydrogen gas are also produced when lithium oxide (Li2O) and water combine.

          4LiOH + H₂ = 2Li₂O + 2H₂O

• Reaction with Nitrogen: Lithium is the only alkali metal that directly reacts with nitrogen (N₂) to form lithium nitride (Li₃N).

           6Li + N₂ → 2Li₃N

• Reaction with Hydrogen: Lithium reacts quickly with hydrogen gas (H₂) to produce lithium hydride (LiH). 2Li + H₂ → 2LiH
• Reaction with Carbon: When lithium reacts with carbon dioxide (CO₂), it forms lithium carbide (Li₂C₂) and lithium oxide (Li₂O).10Li + 2CO₂ → Li₂C₂ + 4Li₂O
• Reaction with Halogens: Due to the small size of its cation (Li⁺), lithium reacts with halogens (X₂, where X can be fluorine, chlorine, bromine, or iodine) to form ionic halides (LiX).2Li + X₂ → 2LiX (X = F, Cl, Br, I)

4.0Uses of Lithium

• Lithium-ion batteries:

Rechargeable batteries, which power gadgets like cell phones, computers, digital cameras, and electric cars, are the main application for lithium.

Non-rechargeable batteries for gadgets like toys, clocks, and heart pacemakers also include lithium.

• Alloys:

Lithium-Aluminum Alloys: Used in high-speed trains, bicycle frames, and airplanes, these alloys increase the strength and decrease the weight of aluminum.

Magnesium-lithium alloys: Armour plating is done using magnesium-lithium alloys that have been strengthened.

• Ceramics and Glass:

Lithium oxide enhances the qualities of unique glasses and glass ceramics.

• Materials that Hygroscopic:

One of the materials that is most hygroscopic is lithium chloride (LiCl). It is utilized in industrial drying systems and air conditioning systems.

• Lubricants:

Lithium Stearate: This lubricant can be used for any purpose and works especially well at high temperatures.

• Applications in Medicine:

Lithium carbonate is a common ingredient in drugs used for  treatment of  bipolar disorder and manic depression.

• Storage of Hydrogen:

Lithium Hydride (LiH): A fuel source that can be utilized to store hydrogen.