In propene pi-bond is formed by sideway overlap of:
Correct answer: B. p-orbitals
- A. s-orbitals
- B. p-orbitals
- C. sp3 hybrid orbitals
- D. sp2 hybrid orbitals
Explanation
Each doubly bonded carbon uses three sp2 hybrids for its sigma bonds and keeps one unhybridised p orbital, and the sideways overlap of those two p orbitals above and below the plane forms the pi bond. Hybrid orbitals point along the internuclear axis and so can only make sigma bonds. This is why rotation about the double bond is blocked.
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About Sigma and Pi Bonds
A sigma bond forms by direct end-to-end overlap along the internuclear axis, whereas a pi bond forms by sideways overlap of parallel orbitals. The topic covers single, double and triple bonds, bond composition, restricted rotation and the relation between sigma and pi bonding and orbital hybridisation.
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