Giant Covalent Structures of Graphite and Diamond

Graphite:

Graphite is a giant covalent structure composed of layers of carbon atoms arranged in a hexagonal lattice. Within each layer, carbon atoms are bonded to three neighboring carbon atoms through strong covalent bonds, forming a network of hexagons. However, between the layers, there are weak van der Waals forces that allow the layers to slide over each other easily. It should be noted that the covalent bonds between C-C bonds are strong, its the Van Der Waals forces of attraction that are weak.

Relating Structures to Uses:

Due to its layered structure and the weak van der Waals forces between layers, graphite has several unique properties that make it useful in various applications:

• Lubricant: The weak interlayer forces in graphite allow the layers to slide easily, making graphite an effective dry lubricant. It reduces friction and wear between moving parts and is commonly used in applications such as locks, hinges, and mechanical systems.
• Conductor of Electricity: Graphite also exhibits electrical conductivity due to the presence of delocalized electrons within the layers.

• Pencil “Lead”: Graphite is a key component of pencil “lead” due to its softness and ability to leave marks on paper when applied.
• Carbon Brushes: Graphite brushes are commonly used in electric motors and generators to transmit electrical current from stationary to rotating parts due to their electrical conductivity and durability.
• Sporting Goods: Graphite composites are utilized in the production of lightweight and strong materials for sporting goods like tennis rackets, fishing rods, golf clubs, and bicycles.
• Refractories: Graphite’s high melting point and chemical inertness make it a valuable component in refractory materials, which are used in high-temperature applications like furnaces and crucibles.

Diamond:

Diamond is another giant covalent structure made entirely of carbon atoms. In diamond, each carbon atom is bonded to four neighboring carbon atoms in a three-dimensional network. The arrangement of carbon atoms forms a tetrahedral structure, with strong covalent bonds in all directions. This results in an extremely rigid and dense structure.

Relating Structures to Uses:

The rigid and densely packed structure of diamond contributes to its exceptional properties, making it highly valuable in cutting tools and other applications: