Question

According to VBT any covalent bond will be formed by overlapping of valence atomic orbitals of bonded atoms provided atomic orbitals must be half–filled and electrons be in opposite spin.
According to type of overlapping covalent bonds can be classified as: (a) $\sigma$ bond (b) $\pi$ bond (c) $\delta$ bond.
The combination of orbital that cannot produce non–bonding molecular orbital is:
(internuclear axis is z–axis)

• A. $p_y+d_{x^2-y^2}$
• B. $p_z+d_{yz}$
• C. $s+d_{xz}$
• D. $d_{xy}+d_{xy}$

Answer 1

The correct option is D $d_{xy}+d_{xy}$

(a) $p_y+d_{x^2-y^2}$: can produce non-bonding if internuclear axis is either $x,y$ or $z$ axis.
(b) $p_z+d_{yz}$: can produce non-bonding if internuclear axis is either $x,y$ or $z$ axis.
(c) $s+d_{xz}$: will always form non-bonding irrespective of inter-nuclear axis.
(d) $d_{xy}+d_{xy}$: either form $\pi$ bond if internuclear axis is $\frac{x}{y}$ axis or can also form $\delta bond$ if internuclear axis is $z$ axis.