Which of the following species has sp^3d^2 hybridization and a non-zero dipole moment?

Step-by-step solution

To determine the hybridization and dipole moment, we first find the steric number (number of bond pairs + lone pairs) for the central atom in each species. BrF₅ : Bromine has 7 valence electrons. It forms 5 single bonds with Fluorine, leaving 1 lone pair. Steric number = 5 + 1 = 6, so hybridization is sp^3d^2 . The shape is square pyramidal, which is asymmetric, leading to a non-zero net dipole moment. XeF₄ : Xenon has 8 valence electrons. It forms 4 single bonds, leaving 2 lone pairs. Steric number = 4 + 2 = 6, so