How could you describe the changes that happen when carbon changes form from graphite to diamond?

Answer 1

When carbon changes form from graphite to diamond, several significant changes occur.

1. Structure: Graphite has a layered structure, where carbon atoms are bonded together in flat sheets. In contrast, diamond has a three-dimensional network structure, where each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral arrangement.

2. Bonding: In graphite, carbon atoms are bonded through weak van der Waals forces between the layers, allowing the layers to slide over each other easily. On the other hand, diamond consists of strong covalent bonds between carbon atoms in all directions, making it extremely hard and rigid.

3. Optical properties: Graphite is opaque and black, as it absorbs most of the visible light due to its layered structure. Conversely, diamond is transparent and colorless, allowing light to pass through it and refract, creating its brilliant sparkle.

4. Electrical conductivity: Graphite is a good conductor of electricity due to the presence of delocalized π electrons within the layers, which can freely move and carry electric charge. Diamond, with its strong covalent bonds, is an insulator and does not conduct electricity.

5. Hardness: Graphite is relatively soft and has a low hardness due to the weak forces between the layers. In contrast, diamond is the hardest natural material known, as every carbon atom is strongly bonded to its neighbors, making it extremely resistant to scratching or cutting.

6. Density: Graphite has a relatively low density, while diamond is much denser. The tight arrangement of carbon atoms in diamond results in a higher overall mass per unit volume.

Overall, the transformation from graphite to diamond involves rearranging the carbon atoms from a layered, planar structure to a three-dimensional network structure, leading to a range of distinct physical and chemical properties.