Consider the given list of molecules: XeF ₂ , ClF ₃ , SF ₄ , PCl ₅ , BrF ₅ , XeF ₄ How many of these molecules possess a permanent dipole moment?

Step-by-step solution

The dipole moment of a molecule depends on its geometry and the presence of lone pairs. XeF ₂ : The central Xe atom has 3 lone pairs and 2 bond pairs ( sp^3d hybridization). It has a linear shape with lone pairs at equatorial positions. The bond dipoles cancel out, so = 0 . ClF ₃ : The central Cl atom has 2 lone pairs and 3 bond pairs ( sp^3d hybridization). It has a T-shape. The bond dipoles do not cancel out, so 0 . SF ₄ : The central S atom has 1 lone pair and 4 bond pairs ( sp^3d hybridization). It has a see-sa