(Polar molecules, Non-polar molecules, etc.)
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I think he briefly mentioned it but basically electron shape views a lone electron pair the same as any regular bonding pair. For example, SO2 would have a molecular shape of bent (2 bonding regions + 1 lone pair) but electron geometry of trigonal trigonal planar (3 regions of electron density).
The difference between electron geometry and molecular shape is whether the lone pairs are taken into account or not; electron geometry demonstrates the complete positions of all shared or lone pair electrons around the central atom, while the molecular shape depicts the physical appearance of the atoms arranged around the central atom.
I think that knowing how to identify both the electron geometry and molecular shape will be important for the upcoming test. Simply remember that the electron geometry only takes into account all regions of high electron density that includes lone pair and bonded electrons. Also keep in mind that a single unpaired electron on the central atom is treated like a lone pair when determining the electron arrangement.
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