Chapter 5, Problem 5.64CHP

Interpretation Introduction

Interpretation:

The hybridization of each carbon atom and number of sigma bonds and pi bonds present in Cinnamaldehyde has to be identified.

Concept introduction:

Orbital hybridization:

• In hybridization, atomic orbitals are mixed to form new hybrid orbitals.
• The formed hybrid orbitals are having different energies, shapes, etc.,
• The newly formed hybrid orbitals are suitable for the pairing of electrons to give chemical bonds in valence bond theory.
• ${\text{sp}}^{\text{3}}$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.
• ${\text{sp}}^2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.
• $\text{sp }$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma bond:

• Sigma bonds are generated by head-on-overlapping between atomic orbitals.
• Sigma bonds are covalent bonds and are strongest bonds.

Pi bond:

• Pi bonds are generated by two lobes of an atomic orbital on one atom overlap two lobes of an atomic orbital on another atom.
• Pi bonds are covalent bonds and are weakest bonds as compared to the sigma bonds.