Answer
See the explanation
Work Step by Step
a. Overlap of 1s atomic orbitals of two hydrogen atoms:
The overlap of 1s atomic orbitals of two hydrogen atoms forms a molecular orbital. This molecular orbital is a sigma (σ) bond, which is a type of bonding orbital. The σ bond is formed by the constructive interference of the wavefunctions of the two 1s atomic orbitals.
b. Overlap of 2p atomic orbitals of two carbon atoms:
The overlap of 2p atomic orbitals of two carbon atoms forms multiple molecular orbitals. These molecular orbitals include:
- Sigma (σ) bonds: Formed by the constructive interference of the wavefunctions of the 2p atomic orbitals along the internuclear axis.
- Pi (π) bonds: Formed by the constructive interference of the wavefunctions of the 2p atomic orbitals perpendicular to the internuclear axis.
c. Overlap of 3d atomic orbitals of two transition metal atoms:
The overlap of 3d atomic orbitals of two transition metal atoms forms multiple molecular orbitals. These molecular orbitals include:
- Sigma (σ) bonds: Formed by the constructive interference of the wavefunctions of the 3d atomic orbitals along the internuclear axis.
- Pi (π) bonds: Formed by the constructive interference of the wavefunctions of the 3d atomic orbitals perpendicular to the internuclear axis.
d. Overlap of 4f atomic orbitals of two lanthanide atoms:
The overlap of 4f atomic orbitals of two lanthanide atoms forms multiple molecular orbitals. These molecular orbitals include:
- Sigma (σ) bonds: Formed by the constructive interference of the wavefunctions of the 4f atomic orbitals along the internuclear axis.
- Pi (π) bonds: Formed by the constructive interference of the wavefunctions of the 4f atomic orbitals perpendicular to the internuclear axis.
