Can orbitals present in the 2p sub-shell hybridized alone ?

Answer

### Step-by-Step Solution:

1. **Understanding Hybridization**: Hybridization is the process of combining different types of atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of an atom.

2. **Identifying the 2p Sub-shell**: The 2p sub-shell consists of three orbitals: 2p_x, 2p_y, and 2p_z. These orbitals can hold a maximum of six electrons (two in each orbital).

3. **Requirement for Hybridization**: For hybridization to occur, there must be a mixing of different types of orbitals. This means that a p orbital cannot hybridize with itself; it requires at least one other type of orbital (such as s or d orbitals) to mix with.

4. **Example of Hybridization**: Consider the example of methane (CH₄). The central carbon atom has the electron configuration of 1s² 2s² 2p². In its ground state, carbon has two unpaired electrons in the 2p orbitals. However, to form four equivalent bonds with hydrogen, one of the 2s electrons is promoted to the 2p orbital, resulting in four unpaired electrons.

5. **Formation of Hybrid Orbitals**: The carbon atom then undergoes hybridization, mixing one 2s orbital with three 2p orbitals to form four equivalent sp³ hybrid orbitals. These sp³ hybrid orbitals are used to form sigma bonds with hydrogen atoms.

6. **Conclusion**: Since the 2p orbitals cannot hybridize alone and require the presence of other orbitals (like the 2s orbital in this case), the answer to the question is that the orbitals in the 2p sub-shell cannot hybridize by themselves.