In IF6^- and TeF5^-, sum of axial d-orbitals which are used in hybridisation in both species. — Chemical Bonding Chemistry Question

💡 Solution & Explanation

Step 1: Determine the geometries: XeO4 and CF4 are tetrahedral (non-planar), while SF4 is see-saw shaped (non-planar). Step 2: XeF4 contains sp3d2 hybridization on Xenon with 4 bonding pairs and 2 lone pairs. According to VSEPR, the lone pairs occupy the axial positions to minimize repulsion, leaving the 4 fluorine atoms in a square planar geometry. Step 3: Because of the square planar symmetry, the individual polar Xe-F bond dipoles cancel out perfectly, making the molecule non-polar. Thus, XeF4 is both planar and non-polar, matching option (c).