What is the Difference Between Carbon and Diamond?

Carbon and diamond are both composed of the chemical element carbon, but they have distinct differences due to their different crystal structures and bonding arrangements. The main differences between carbon and diamond include:

1. Crystal Structure: In diamond, each carbon atom shares electrons with four other carbon atoms, forming four single bonds and creating a strong, rigid three-dimensional structure. In graphite, carbon atoms form sheets of carbon atoms, with each sheet held together by weak forces known as stacking interactions.
2. Hardness and Strength: Diamond is one of the hardest materials known, with a hardness of 10 on the Mohs scale. In contrast, graphite is soft and slippery, with a hardness of 1 to 2 on the Mohs scale.
3. Transparency and Appearance: Diamonds are transparent and typically appear brown, gray, or colorless. Graphite, on the other hand, is opaque and has a dark, metallic-to-earthy appearance.
4. Compressibility: Diamond's tetrahedral structure provides great resistance to compression, making it highly durable.
5. Solubility: Both diamond and graphite are insoluble in water and organic solvents due to the strong attractions between their carbon atoms.

In summary, the key difference between carbon and diamond lies in their crystal structures and bonding arrangements. Diamond's strong, rigid three-dimensional structure gives it extraordinary hardness and durability, while graphite's sheet-like structure makes it soft, slippery, and more prone to cleaving.

Comparative Table: Carbon vs Diamond

Here is a table comparing the differences between carbon and diamond:

Carbon is a chemical element, while diamond is an allotrope of carbon. Allotropes are different forms of an element, and their physical properties vary from each other. In the case of carbon, some allotropes include graphite and diamond.