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.
Which of the following set of orbitals does not produce nodal plane in $xz–$plane?

• A. $d_{yz}+d_{yz}$
• B. $d_{xy}+d_{xy}$
• C. $p_y+d_{xy}$
• D. None of these

Answer 1

The correct option is D None of these

(a) Type of orbital combination- $d_{yz}+d_{yz}$
For $\pi$ bond: Internuclear axis- $y-\text{axis and}z-\text{axis}$ and Nodal plane- $xy\text{and}xz$
For $\sigma$ bond- $x-\text{axis}$ and Nodal plane- $xy\text{and}xz$
(b) Type of orbital combination- $d_{xy}+d_{xy}$
For $\pi$ bond: Internuclear axis- $x-\text{axis and}y-\text{axis}$ and Nodal plane- $xz\text{and}yz$
For $\sigma$ bond- $z-\text{axis}$ and Nodal plane- $xz\text{and}yz$
(c) Type of orbital combination- $p_y+d_{xy}$
For $\pi$ bond: Internuclear axis- $x-\text{axis}$ and Nodal plane- $xz$
For $\sigma$ bond-No delta bond formation.