' d xy ' orbital can not form bond with which of the following orbital (If overlapping axis is either ' x ' or ' y ' or ' z ')

Question

' d xy ​ ' orbital can not form bond with which of the following orbital (If overlapping axis is either ' x ' or ' y ' or ' z ')

TestHub · Accepted Answer

For effective bonding, orbitals must have proper symmetry and overlap. The $d_{x y}$ orbital has lobes in the xy-plane. A $p_{z}$ orbital has lobes along the z-axis. With overlapping axes restricted to x, y, or z, there is no effective overlap between $d_{x y}$ and $p_{z}$ due to their orthogonal orientations.

Concepts: Orbital overlap, symmetry, bonding.

The $d_{x y}$ orbital cannot form a bond with the $p_{z}$ orbital due to orthogonal symmetry and no effective overlap along x, y, or z axes.

Chemistry - CHEMICAL BONDING Question with Solution | TestHub

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