The differences between sigma bond and pie bond are given as follows:
- A sigma bond is formed by the end to end overlap of half-filled atomic orbitals along the internuclear axis.
- Sigma bond-containing compound is less active.
- The molecular orbital is symmetrical about the internuclear axis.
- There can be the free rotation of atoms around the sigma bond.
- The bond may be representing between two atoms either along or pie bond.
- In the formation of sigma bond s-orbital can participate.
- Sigma bond containing compound generally gives substitution reaction.
- In this case, overlapping can take place to a large extent.
- Pie bond is formed by the side wise overlap of two half-filled p-orbitals.
- Pie bond-containing compound is more active.
- The molecular orbital is discontinuous and consists of two charged clouds above and below the plane of atoms.
- Free rotation of atoms around pie bond is not possible.
- The bond is always present between two atoms in addition to sigma bond.
- In the formation of pie bond s-orbital cannot participate.
- Pie bond-containing compound generally gives addition reaction.
- In the formation of pie bond overlapping occurs to a lesser extent.