A) Overlap of one s- and \[s{{p}^{2}}\]-hybridized orbitals.
B) Overlap of two \[s{{p}^{2}}\]- hybridized orbitals.
C) Overlap of one p-and one \[s{{p}^{2}}\]-hybridized orbitals.
D) Sideways overlap of two p-orbitals.
Correct Answer: D
Solution :
[d] Rotation around \[\pi \] bond is not possible. If any attempt is made to rotate one of the carbon atoms, the lobes of \[\pi \]-orbital will no longer remain coplanar i.e no parallel overlap will be possible and thus \[\pi \]-bond will break. This is known as concept of restricted rotation. In other words the presence of \[\pi \]-bonds makes the position of two carbon atom.
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