Answer
σ bonds are formed by the head-on overlap of atomic orbitals along the internuclear axis, while π bonds are formed by the side-to-side overlap of p orbitals perpendicular to the internuclear axis.
Work Step by Step
In the molecular orbital model, σ bonds and π bonds have the following characteristics:
σ Bonds:
- σ bonds are formed by the head-on overlap of atomic orbitals along the internuclear axis (z-axis).
- The overlapping atomic orbitals can be s-s, s-p, or p-p orbitals.
- σ bonds are generally stronger and more stable than π bonds.
- Examples of σ bonds include C-C, C-H, and C-O single bonds.
π Bonds:
- π bonds are formed by the side-to-side overlap of p orbitals perpendicular to the internuclear axis (z-axis).
- The overlapping p orbitals must be parallel to each other.
- π bonds are generally weaker and less stable than σ bonds.
- Examples of π bonds include C=C and C=O double bonds, where the π bonds are formed by the side-to-side overlap of p orbitals.
