(Polar molecules, Non-polar molecules, etc.)
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You have to be careful because Lewis structures are not meant to be drawn to an accurate representation of the shape of a molecule. Although a Lewis structure may be drawn as symmetrical, we must first consider the VSEPR shape first. If we were to use the shape and symmetry of the VSEPR structure, then we are able to determine the polarity using the shape and symmetry.
Sometimes symmetry alludes to polarity but since most of the time the lewis structure isn't the actual representation you have to base it off of the VSEPR model. A symmetric Lewis structure does not automatically mean the molecule is non polar because the VSEPR model is the actual shape of the molecule. You should base the polarity off of the VSEPR model.
Not really. Although asymmetrical Lewis structures are usually polar, there are many symmetrical Lewis structures that are polar too. Take water for example. It is symmetrical in its Lewis structure and its electron geometry, but it's still polar because the dipoles don't cancel out. Best to just draw the VSEPR model and determine the overall dipole moment.
The Lewis structure won't show you the polarity, but it is helpful in determining the VSEPR model shape of the molecule which will then help determine polarity. If the VSEPR shape allows for dipole moments to cancel and the overall dipole moment to be zero, then the molecule will be nonpolar.
Lewis structures can be deceiving of the actual molecular shape. It is best to use the VSEPR model to se the symmetry of the molecular shape. Then the dipole moments of polar bonds can create partially charged vectors. If, when considering the molecular symmetry and charge of each bond, the vectors cancel out, the molecule is nonpolar. If the vectors do no cancel out, the molecule is polar.
The symmetry of a Lewis Structure can be an indicator of polarity. For example, CCl4 has a carbon atom surrounded by four chlorine atoms of equal electronegativity. Because it is a symmetrical molecule, the dipole moments of the four chlorines cancel and it is a nonpolar molecule. This would not be the case if one of the chlorines was instead a different atom with a different electronegativity, like hydrogen, then it would be polar. However, it is probably best to draw a VSEPR shape to determine polarity instead of relying only on Lewis structures.
Symmetry shouldn't really be what you're looking for to determine polarity but rather use the VSEPR models instead because VSEPR models are the actual representation and Lewis structures are just inaccurate base models.
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