Hybridisation involves .

Options

A. Orbitals of same atom with slightly different energies .
B. Orbitals of different atom but with equal energies .
C. Orbitals of different atoms with exactly equal energies .
D. Orbitals of same atoms with exactly equal energies .

Answer

**Step-by-Step Solution:**

1. **Understanding Hybridization**: Hybridization is a concept in chemistry where atomic orbitals mix to form new hybrid orbitals. These hybrid orbitals have different shapes and energies compared to the original atomic orbitals.

2. **Identifying the Orbitals Involved**: Hybridization involves the mixing of atomic orbitals from the same atom. These orbitals are typically of similar energy levels but not necessarily equal in energy.

3. **Examples of Hybridization**: For instance, in the formation of methane (CH₄), the carbon atom undergoes hybridization. The carbon atom has the electron configuration of 1s² 2s² 2p². To form bonds, the carbon atom promotes one of its 2s electrons to the 2p orbital, resulting in four unpaired electrons.

4. **Formation of Hybrid Orbitals**: The 1s orbital and the three 2p orbitals mix to form four equivalent sp³ hybrid orbitals. These sp³ orbitals have the same energy, which is a key characteristic of hybrid orbitals.

5. **Conclusion**: Therefore, hybridization involves the mixing of orbitals of the same atom that have slightly different energies, resulting in the formation of new orbitals that are equivalent in energy.

**Final Answer**: Hybridization involves orbitals of the same atom with slightly different energies.

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