Define hybridization. Explain `sp^(2)` hybridization with suitable example.

Answer

**Step-by-Step Solution:**

1. **Definition of Hybridization:**
Hybridization is the process of intermixing atomic orbitals of similar energy to form new hybrid orbitals. These hybrid orbitals have the same energy and are used to form chemical bonds in molecules.

2. **Understanding `sp²` Hybridization:**
The `sp²` hybridization involves the mixing of one `s` orbital and two `p` orbitals from the same atom to create three equivalent hybrid orbitals. These orbitals are oriented in a trigonal planar arrangement, which means they are 120 degrees apart.

3. **Example: Boron Trichloride (BCl₃):**
- **Electronic Configuration of Boron:**
The electronic configuration of boron is \(1s^2 2s^2 2p^1\). In the ground state, boron has two electrons in the `1s` orbital, two in the `2s` orbital, and one in the `2p` orbital.
- **Excited State:**
When boron forms BCl₃, one of the `2s` electrons is excited to the `2p` orbital. The excited state configuration becomes \(2s^1 2p^2\).
- **Hybridization:**
The `2s` orbital and two `2p` orbitals combine to form three equivalent `sp²` hybrid orbitals. This results in three hybrid orbitals that are used to form bonds with three chlorine atoms.
- **Bond Formation:**
Each chlorine atom contributes one electron to form a covalent bond with boron, resulting in a total of three bonds in BCl₃.

4. **Characteristics of `sp²` Hybridization:**
- **Geometry:** The geometry of molecules with `sp²` hybridization is trigonal planar.
- **Bond Angles:** The bond angles between the hybrid orbitals are approximately 120 degrees.
- **S and P Character:** In `sp²` hybridization, there is 33% `s` character and 67% `p` character in the hybrid orbitals.