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if the molecule is asymmetric, the bond dipole moments won't "cancel out" and the molecule will have a net dipole moment and the molecule is therefore polar, but if the molecule is symmetric, dipole moments will usually cancel out. hope this helps.
Like stated above, you can cancel the net dipole moments in order to determine if a molecule is polar or not. However, I think just basing it off the Lewis Structure might not be the best. For me, I like to know the shape of the molecule so I can visualize how the atoms are rearranged and how the dipoles can cancel out. Just a tip :)
In order to predict whether a molecule is polar or non polar, we would need to draw the best 3D structure of the molecule to determine the dipole moment. When we draw the best 3D structure, we would also need to know the electronegativity of each atom to draw the bond dipoles. If the bond dipoles do not cancel, then the molecule is polar. If the bond cancels all cancel, the molecule is non polar because there is no overall dipole moment. Remember, a non polar molecule can have polar bonds but still be non polar if there is no dipole moment.
First step in determining if something is polar or nonpolar is drawing the lewis structure. Then you check for electronegativity , as stated below, if it doesn't cancel out then it is polar. It would help to also draw the 3D model to get a more closer look.
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