(Polar molecules, Non-polar molecules, etc.)
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We base the electron pair geometry on the number of regions of electron density surrounding the central atom (5), so it is trigonal bipyramidal. For the molecular geometry, we look at the bonds specifically. The bonds between the 3 surrounding atoms with the central atom create a T-shaped geometry.
AX3E2 is not linear. It is T-shaped. An example of this VSEPR type is ClF3. It has three fluorine atoms and one Cl atom as the central atom. It has two lone pairs and has three bonds. The three fluorine atoms are arranged around the central Cl atom to form a T-shaped molecule.
AX3E2 is T shaped. There are 5 electron densities regions, so we can see consider it as trigonal pyramidal with 2 bonding pair changed into lone pair. Changing the pairs on the trigonal planar is more stable, hence resulting the T-shaped. I think this picture shows the shape clearly.
- ax3e2.gif (7.91 KiB) Viewed 288 times
AX3E2. From this we can see that the central atom has 5 areas of electron density so the shape is trigonal bipyramidal. Now when it comes to naming the shape only the molecules connected to it count towards its name and we can see that only 3 molecules are attached. Now for a trigonal bipyramidal when you have lone pairs you always remove the equatorial ones first because it interacts with the most molecules ( 4 molecule interactions vs 3 for axial position). Since there are two lone pairs it would be in the equatorial positions and so the shape is a t shape ( with 2 axial molecules and one equatorial molecule with a bond angles of 90 degrees relative to the axial molecules).
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