Question

What is the chemical basis of molecular hybridization?

Short answer

Short Answer: Molecular hybridization is the process where atomic orbitals of an atom combine to create new hybrid orbitals to form chemical bonds in molecules. Different types of hybrid orbitals can be formed, such as sp, sp^2, sp^3, dsp^3, and d^2sp^3. An example of hybridization is in methane (CH4), where the carbon atom forms four single covalent bonds with hydrogen atoms. The carbon combines its 2s and three 2p orbitals to create four sp^3 hybrid orbitals which overlap with the hydrogen's 1s orbitals. This results in a tetrahedral geometry with a bond angle of 109.5 degrees.

Step-by-step solution

1. Define Molecular Hybridization

Molecular hybridization is the process by which atomic orbitals of an atom combine to create new hybrid orbitals. These hybrid orbitals then overlap with other orbitals from neighboring atoms to create chemical bonds, resulting in the formation of molecules. This concept was introduced by Linus Pauling to explain the formation and shape of covalent bonds in polyatomic molecules.

2. Types of Hybrid Orbitals

There are several types of hybrid orbitals, depending on the number and type of atomic orbitals that combine to form the hybrid orbitals: - sp hybridization: one s orbital and one p orbital combine to form two sp hybrid orbitals. - sp^2 hybridization: one s orbital and two p orbitals combine to form three sp^2 hybrid orbitals. - sp^3 hybridization: one s orbital and three p orbitals combine to form four sp^3 hybrid orbitals. - dsp^3 hybridization: one s orbital, three p orbitals, and one d orbital combine to form five dsp^3 hybrid orbitals. - d^2sp^3 hybridization: one s orbital, three p orbitals, and two d orbitals combine to form six d^2sp^3 hybrid orbitals.

3. Example of Molecular Hybridization: Methane (CH4)

Methane (CH4) is a simple example that demonstrates hybridization. In methane, the central carbon atom forms four single covalent bonds with four hydrogen atoms. Carbon has an electron configuration of 1s^2 2s^2 2p^2. To form four covalent bonds, the 2s and the three 2p orbitals of the carbon atom combine to create four equivalent sp^3 hybrid orbitals. These sp^3 hybrid orbitals then overlap with the 1s orbitals of the hydrogen atoms to form four C-H sigma bonds. The resulting CH4 molecule has a tetrahedral geometry with a bond angle of 109.5 degrees.