Question

Molecular orbitals are formed by the overlap of suitable atomic orbitals from different atoms. Symmetry and energies of the overlapping orbitals and distance between the approaching atoms are crucial for the formation of molecular orbitals. For diatomic molecules, by convention, the internuclear axis is taken to be in the z-direction. Correct statements are:

(1) Overlap of two 2p_x orbitals will always form a stronger bond than overlap of two 2p_z orbitals.

(2) Linear combination of two 2p_z orbitals can produce a σ molecular orbital.

(3) Molecular orbitals formed from 2p_x orbitals are not symmetrical around the internuclear axis.

(4) 2s and 2p_z orbitals can overlap to form a bonding orbital.

Answer 1

(1) As we have given that the internuclear axis in the z-direction

\(\therefore \) So, overlap of 2P_x orbital always form \(\pi\)-bond and we know that \(\pi\)-bond is weaker than \(\sigma \) bonds

(2) Yes - Linear combination of two 2P_z orbital formed one, \(\sigma \) bonding molecular orbital and one \(\sigma \) anti bonding molecular orbital .

(3) As given, The internuclear axis in z-direction 

So, 2P_x always form \(\pi\) bonding and \(\pi\) anti bonding molecular orbital. as we know \(\pi\) - bonds are not symmetrical around \(\sigma \) bond or internuclear axis. so it is also correct statement.

(4)

 

energy of 2s and 2P_z orbitals are almost same so that they can overlap effectively and form bonding orbitals.

Hence, option (2), (3) and (4) are correct statement.