Why Is Jewelry So Hard | Precious Stones

Carbon Atom Arrangement
Diamonds are pure carbon, with each carbon atom covalently bonded to four others in a tetrahedral (3D pyramid) setup. This forms a rigid, three-dimensional lattice called diamond cubic structure—imagine a infinite network of interlocked pyramids where every atom pulls equally on its neighbors.

Strength of Covalent Bonds
The bonds are strong sp³ hybrid covalent bonds (sharing electrons tightly between carbons). These are shorter ([ \approx 1.54 \times 10^{-10} ] m) and stronger than bonds in softer carbon forms like graphite (which has flat, slippery layers). Breaking a diamond requires overcoming all four bonds per atom simultaneously, demanding massive energy—about 356 kJ/mol per bond.

No Weak Points
Unlike metals (with movable dislocations) or crystals with cleavage planes, diamond's structure has no easy slip planes. Its isotropic bonding resists deformation from any direction, making scratches or cracks rare unless hit with something equally hard (e.g., another diamond).

Example: A diamond can cut glass because glass's weaker Si-O bonds shatter under the lattice's unyielding pressure, while the diamond tip stays intact.

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