What is the hybridisation of the following species ?
Diamond, Graphite

Answer

To determine the hybridization of diamond and graphite, we will analyze each allotrope of carbon step by step.

### Step 1: Understanding Diamond
1. **Structure**: Diamond is a crystalline form of carbon where each carbon atom is tetrahedrally coordinated to four other carbon atoms.
2. **Hybridization**: In diamond, the carbon atoms undergo sp³ hybridization. This means that one s orbital and three p orbitals mix to form four equivalent sp³ hybrid orbitals.
3. **Bonding**: Each of these sp³ hybrid orbitals forms a sigma bond with another carbon atom, resulting in a three-dimensional network structure.
4. **Shape**: The overall shape of the diamond structure is tetrahedral, with bond angles of approximately 109.5 degrees.

### Step 2: Understanding Graphite
1. **Structure**: Graphite consists of layers of carbon atoms arranged in a hexagonal lattice. Each carbon atom is bonded to three other carbon atoms in the same plane.
2. **Hybridization**: In graphite, the carbon atoms undergo sp² hybridization. This involves one s orbital and two p orbitals mixing to form three sp² hybrid orbitals.
3. **Bonding**: Each sp² hybrid orbital forms a sigma bond with another carbon atom, while the remaining unhybridized p orbital forms a pi bond with adjacent carbon atoms, leading to delocalized electrons above and below the plane.
4. **Shape**: The arrangement of the carbon atoms in graphite results in a trigonal planar shape with bond angles of approximately 120 degrees.

### Summary of Hybridization
- **Diamond**: sp³ hybridization (tetrahedral shape)
- **Graphite**: sp² hybridization (trigonal planar shape)