CHEM 14A Lecture Notes - Lecture 7: Trigonal Planar Molecular Geometry, Square Planar Molecular Geometry, Lone Pair

• School: UCLA
• Department: Chemistry and Biochemistry
• Course: CHEM 14A
• Professor: Scerri Eric

Document Summary

There are only five possible electronic geometries which you establish by counting the number of electron regions surrounding the central atom (cid:9)2(cid:9) electron regions. Ax6 sp3d sp3d2 linear(cid:9) trigonal planar(cid:9) tetrahedral(cid:9) trigonal bipyramid(cid:9) octahedral(cid:9) Ax4e note that the lone pairs all go in the equatorial positions. Geometriescan be any of the shapes on the whole page. The electronic geometries are only those in the box (and orbital hybridizations). The molecular positions occupied geometry will be different from by a lone pair. T-shaped(cid:9) the electronic when there is at least one or more lone pairs on the central atom. Look at the top of the table and go. As you change from bonding electrons to lone pair electrons, the molecular shape is now different from the electronic because some of the positions are missing atoms. The new shape is then renamed based on the shape of the atoms. positions occupied by a lone pair.