Which of the following will not form sigma bond after overlapping?? A) s orbital and s orbital B) s orbital and pz orbital C) pz orbital and pz orbital D) px orbital and px orbital Ans is d anyone plz explain why px not overlap?

Question

Answer

During formation of sigma a bond ,the orbitals overlap axially (head on overlapping) which is firmly bonding.now p orbitals overlapping cant done headon so they have only one option to overlap sideways, perpendicular to plane.since pie bonds is form by sideways overlaping so they are ealy to break.

Answer

Two px orbitals overlap sidewise to form a pi bond which is weaker than a sigma bond (formed by head on overlapping of either two sigma or one sigma and one pi bond). So, option d is correct.

Answer

Explanation:

Sigma bonds are formed by the overlapping of atomic orbitals end to end along the internuclear axis. The orbitals that participate in the formation of sigma bonds should have sufficient overlap and energy similarity. The options given are:

A) s orbital and s orbital: S orbitals can form sigma bonds by overlapping end to end along the internuclear axis.

B) s orbital and pz orbital: S orbital and pz orbital can overlap end to end along the internuclear axis to form sigma bond.

C) pz orbital and pz orbital: Two pz orbitals can overlap along the internuclear axis to form a sigma bond.

D) px orbital and px orbital: Px orbitals cannot overlap end to end along the internuclear axis to form sigma bonds. Px orbitals are perpendicular to the internuclear axis, and thus, they cannot overlap end to end along the axis.

Therefore, the correct answer is option D) px orbital and px orbital.

Summary:
- Sigma bonds are formed by the overlapping of atomic orbitals end to end along the internuclear axis.
- Px orbitals cannot overlap end to end along the internuclear axis to form sigma bonds.
- The correct answer is option D) px orbital and px orbital.

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