BRAINLIESTHow do you determine if a covalent bond is polar or nonpolar without using electronegativity? How does dipole moment work with covalent bonds?

Use molecular geometries. Some geometries are asymmetrical, so they necessarily are polar. Other molecules are symmetrical, so even though they contain elements of great differences in electronegativities, these molecules are non-polar.

Consider carbon dioxide - which has the elements carbon and oxygen in its composition. The EN of carbon is 2.5; the EN of oxygen is 3.5. Clearly, there is a big difference in electronegativity, which suggests that the oxygens are isolating electron density away from the carbon.

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As we can see in the above picture, the two permanent dipoles cancel each other out since they are equal in magnitude and opposite in direction. So carbon dioxide might have elements of great difference in EN, but is still non-polar.

Now apply this knowledge to your problem. To determine molecular geometries, understand that both electrons and attached atoms influence geometry. Try looking up and applying the AXE method. I will leave my answer at here for now, since you have not shown much work in tackling this problem.

Explanation: