Draw an orbital diagram of the following molecules. Indicate the hybridization of each atom and indicate the orbitals used for each sigma and pi bond. Assign formal charged to each atom.

VSEPR Geometry and Molecular Geometry of OH-

D a Given that the spatial requirement of a lone pair is greater than that of a bond pair, explain why XeF2 has a linear molecular structure and not a bent one. The four lone pairs of XeF2 occupy the equatorial positions. The angles between lone pairs are 60°, so there is less lone pair/lone pair repulsion with this arrangement. O The two lone pairs of XeF2 occupy the equatorial positions. The angle between lone pairs is 180°, so there is less lone pair/lone pair repulsion with this arrangement. O The two lone pairs of XeF2 occupy the equatorial positions. The angle between lone pairs is 60°, so there is less lone pair/lone pair repulsion with this arrangement. O The three lone pairs of XeF2 occupy the equatorial positions. The angles between lone pairs are 120°, so there is less lone pair/lone pair repulsion with this arrangement. Submit

Explain, why CH3Cl has higher dipole moment than CH3F?