Saint Mary’s College Molecular Geometry Chemistry 8 Steric Bonded Number* Atoms Lone Pairs Molecular Geometry Bond Angle Examples 2 2 0 linear 180° BeCl2 CO2 3 3 0 trigonal planar 120° BF3 NO3− 3 2 1 bent <120° GeF2 SO2 4 4 0 tetrahedral 109.5° CH4 ClO4− Drawing** Hybrid-­‐
ization sp sp2 sp2 sp3 4 3 1 trigonal pyramidal <109.5° (107.3°) NH3 ClO3− 4 2 2 bent <109.5° (104.5°) H2O SCl2 5 5 0 trigonal bipyramidal 90° and 120° PCl5 sp3 sp3 sp3d 5 5 4 3 1 2 seesaw-­‐
shaped <90° and <120° SF4 T-­‐shaped <90° ClF3 sp3d sp3d 5 2 3 linear 180° XeF2 I3− sp3d 6 6 0 octahedral 90° SF6 sp3d2 6 6 5 4 1 2 square pyramidal <90° square planar 90° BrF5 sp3d2 XeF4 sp3d2 * The steric number is the number of electron pairs, i.e., the number of atoms + number of lone pairs ** Only the lone pairs on central atoms are shown. You may be required to show lone pairs on all atoms.