The differences between graphite and diamond 0
Answers
Molecular structure
Diamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.
Graphite: It is also Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.
Hardness
Diamond: Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.
Graphite: Soft. Layers of hexagonally arranged carbon atoms can slide over one another.
Electrical conductivity
Diamond: Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.
Graphite: Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.
Even though they are made of the same element (Carbon), a Diamond differs from Graphite in the atomic structure. In Diamonds, the atoms are closely packed with together with each atom connected to other carbon atoms as compared to Graphite where the bonds between the layers are weak.