Chemistry - CHEMICAL BONDING Question with Solution | TestHub

The molecule is of the ${\mathrm{XF}}_4$ type with a zero dipole moment ($\mu =0$). This implies a highly symmetrical structure. To confirm the geometry, knowing the planarity is crucial. If it's planar, it's square planar. If not, other non-polar geometries like tetrahedral (if X has no lone pairs) or see-saw (if X has one lone pair) would be considered, but a zero dipole moment for ${\mathrm{XF}}_4$ strongly suggests square planar geometry. Therefore, planarity is the key additional information.