In propene pi-bond is formed by sideway overlap of:
- 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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