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If a molecule only has non polar bonds, then the it will be non polar. Usually when a molecule has a lone pair, it is polar. However, in molecules like XeF4 (2 lone pairs), the dipole moments and lone pairs cancel out, rendering the molecule non polar. Hope this helps!
Adding to this, make sure to recognize that just because a Lewis structure might look like it's symmetrical, you have to take into account the VSEPR shape to see if the molecule truly is symmetrical (i.e. tetrahedrals such as CH2Cl2 in a Lewis structure looks symmetrical, but in VSEPR, it's not)
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