If two different non-axial d-orbitals having | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) The $d-$orbitals having an $xz$ nodal plane are $d_{xy}$ and $d_{yz}$.For a $\pi-$bond to form,the orbitals must overlap laterally.However,two dif

Vedclass · Accepted Answer

They do not form a $\pi-$bond

Vedclass · Answer

(D) The $d-$orbitals having an $xz$ nodal plane are $d_{xy}$ and $d_{yz}$.For a $\pi-$bond to form,the orbitals must overlap laterally.However,two different non-axial $d-$orbitals with the same nodal plane cannot overlap effectively to form a $\pi-$bond along any internuclear axis because their symmetry requirements for $\pi-$bonding are not met.Therefore,they do not form a $\pi-$bond.

If two different non-axial $d-$orbitals having $xz$ nodal plane form $\pi-$bond by overlapping each other,then the internuclear axis will be:

Similar Questions

The total number of lone pairs of electrons in the given molecule is

Arrange the following species in the increasing order of lone pairs of electrons:
$(A)$ $CO$
$(B)$ $NO_2^-$
$(C)$ $NF_3$
$(D)$ $CO_3^{2-}$

Which of the following molecules does not form in the $I^{st}$ excited state of the central atom?

The correct order of increasing bond lengths of $C-H$, $O-H$, $C-C$ and $H-H$ is

The correct order of bond strength for the given species is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module