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Question

Assuming z-orbital to be the inter-nuclear axis, which of the following overlaps is incorrect?

A
2py+2pyπ2py
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B
2pz+2pzσ2pz
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C
2px+2pxπ2px
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D
1s+2pyπ(1s2py)
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Solution

The correct option is D 1s+2pyπ(1s2py)
2py orbitals of an atom overlaps side by side with 2py orbital of another atom and forms a π bond.
2pz orbitals of an atom overlaps head on with 2pz orbital of another atom and forms a σ bond.
2px orbitals of an atom overlaps side by side with 2px orbital of another atom and forms a π bond.
1s orbital and 2py orbital will never form π bond since s orbital overlapping always forms a sigma bond.

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