(Polar molecules, Non-polar molecules, etc.)
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Also, if you're dealing with water, the shape is also bent but the bond angle would be 104 degrees due to the presence of 2 lone pairs, which pushes the bonded atoms even closer together, further reducing the bond angle.
The way I always remember it is by determining the electron geometries by observing the molecule by its areas of election density. This means that if a molecule has two bonds and two lone pairs, the electron geometry is tetrahedral because it has four areas of electron concentration. If the molecule has three areas of electron density, with two bonds and one lone pair, then I would consider the electron geometry to be trigonal planer. We know that the shape of a tetrahedral has bond angles of 109.5, while for trigonal planer, the bond angles are 120. Because there are lone pairs, we know the shape of the molecules aren't tetrahedral and trigonal planer but bent for both molecules, which means that the bond angles for the respective molecules are less than 109.5 and 120. Hopefully that makes sense.
If there are 2 lone pairs, then it would be less than 109.5 degrees. If there is 1 lone pair, then it would be less than 120 degrees. Both are bent shape, but the bond angles differ depending on the amount of lone pairs.
If there are 2 lone pairs, then it would be less than 109.5 degrees. If there is 1 lone pair, then it would be less than 120 degrees. Bent shape simply means that there are lone pairs that create a repulsion that allows the bonds to come closer together, allowing for the angles to decrease.
It really depends on how many lone pair the molecule have. If there is only one lone pair, then the angle will be slightly-less-than 120 degrees, if there are two lone pairs, then the angle will be slighty-less-than 109.5 degrees.
This depends on whether the atom has one or two lone pairs, in addition to its two bond pairs. If it has one lone pair, the bond angle will be < 120 degrees, however, if it has two lone pairs, it will have a bond angle << 109.5 degrees (ex. Water has a bond angle of approx. 104.5 degrees)
This depends on the vsepr formula of the molecule. there can be a bent shape in both AX2E2 and AX2E but the angles will be different in these two cases. In AX2E2 there will be more electron repulsion (its electron geometry is tetrahedral) so it will be slightly less than 109.5. In AX2E, the electron geometry is trigonal planar, and thus the bond angle will be slightly less than 120.
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