Linear Trigonal Planar Tetrahedral Trigonal Bipyramid Octahedral Bent

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Linear Trigonal Planar Tetrahedral Trigonal Bipyramid Octahedral Bent

There are only FIVE possible electronic geometries which you establish by counting the number of electron regions surrounding the central atom electron electron electron electron electron 2regions 3regions 4regions 5regions 6regions AX2 AX3 AX4 AX5 AX6 3 sp sp2 sp sp3d sp3d2 linear trigonal planar tetrahedral trigonal bipyramid octahedral note that AX E AX4E the lone 5 AX E .. .. pairs all AX2E .. 3 go in the equatorial position occupied positions .. 1 by a lone pair bent trigonal pyramid see-saw square pyramid Molecular Geometries AX E can be any of the shapes on .. 4 2 AX2E2 .. .. .. the whole page. The .. AX E electronic geometries are only positions occupied 3 2 .. those in the box (and orbital 2 by a lone pair hybridizations). The molecular bent T-shaped square planar geometry will be different from the electronic when there is at least one or more lone pairs AX3E3 on the central atom. Look at the top of the table and go .. DOWN a column. As you change from bonding electrons .. AX E .. positions occupied .. 2 3 .. to lone pair electrons, the molecular shape is now different by a lone pair from the electronic because some of the positions are missing 3 .. atoms. The new shape is then renamed based on the shape of the atoms. linear T-shaped Remember, once you have estabilished the correct electronic geometry, the molecular .... AX2E4 geometry MUST be either the same as the electronic or one of the shapes listed directly positions occupied .. under the electronic geometry. In other words, each shape in a given column here has the 4 by a lone pair .. same electronic geometry given at the top of the column. linear Polarity If all the positions on the electronic geometry are the same (have the same atoms surrounding the central atom), the molecule is NOT polar because of the symmetry. Any of the other molecular geometries (except square planar and linear) under the box will be polar. McCord 10/2005.

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