key term - Diamond

Definition

Diamond is a crystalline form of carbon in which the carbon atoms are arranged in a tetrahedral lattice structure. This unique arrangement gives diamond its exceptional hardness and optical properties, making it not only a highly sought-after gemstone but also a valuable material in industrial applications. The strong covalent bonds between the carbon atoms in diamond contribute to its stability and resistance to chemical reactions.

5 Must Know Facts For Your Next Test

1. Diamonds are formed under high-pressure, high-temperature conditions deep within the Earth's mantle over millions of years.
2. The hardness of diamond is rated at 10 on the Mohs scale, making it the hardest naturally occurring substance known.
3. Diamonds have a high refractive index, which contributes to their brilliance and sparkle when cut properly for jewelry.
4. In addition to their use in jewelry, diamonds are also utilized in industrial applications for cutting, grinding, and drilling due to their hardness.
5. The unique tetrahedral arrangement of carbon atoms in diamond results in strong covalent bonds that give diamond its stability and durability.

Review Questions

• How does the tetrahedral lattice structure of diamond contribute to its physical properties?
  • The tetrahedral lattice structure of diamond contributes significantly to its physical properties by creating a network of strong covalent bonds between carbon atoms. This arrangement results in an extremely rigid and stable framework, which accounts for diamond's exceptional hardness. Additionally, this specific structure influences other properties such as its high melting point and low electrical conductivity.
• Discuss the differences between diamond and graphite as allotropes of carbon, focusing on their bonding and structural arrangements.
  • Diamond and graphite are both allotropes of carbon but exhibit vastly different properties due to their distinct bonding and structural arrangements. In diamond, each carbon atom is bonded to four others in a three-dimensional tetrahedral lattice, resulting in a very hard material. In contrast, graphite consists of layers of carbon atoms arranged in a planar hexagonal lattice where each atom is bonded to three others; these layers can slide over each other easily, giving graphite its lubricating properties. This difference in structure leads to diamond being hard and transparent while graphite is soft and opaque.
• Evaluate the significance of diamonds in both industrial applications and as gemstones in terms of their unique properties.
  • Diamonds hold significant value both as gemstones and in industrial applications due to their unique properties. Their hardness makes them ideal for cutting, grinding, and drilling tools used in manufacturing and construction, where durability is crucial. As gemstones, diamonds are prized for their brilliance and sparkle, attributed to their high refractive index and ability to disperse light. This dual functionality demonstrates how diamonds' physical characteristics can be harnessed for both aesthetic appeal and practical uses, reflecting their versatility.

Related terms

Covalent Bonding:

A type of chemical bond where pairs of electrons are shared between atoms, which is key to the formation of diamond's strong lattice structure.

Crystal Lattice:

The symmetrical three-dimensional arrangement of atoms within a crystal, which determines the physical properties of the solid, including diamonds.

Allotropes: Different structural forms of the same element, such as diamond and graphite, that have distinct physical properties due to variations in bonding and arrangement.