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    For each of the following, determine if the molecule would have a dipole moment (polar or nonpolar):

    1. Draw the Lewis Dot Structure for each

    2. Determine the Electron Arrangement

    3. Draw the Molecular Geometry

    4. Find the electronegativities for each atom and draw an arrow along the bond toward the most electronegative element

    5. If the arrows cancel each other out, the molecule/ ion is nonpolar (no dipole moment). If the arrows do not cancel, the molecule/ ion is polar (has a dipole moment)

    PF5 No dipole CS2 No dipole BrO3- Dipole
    NH4+ No dipole SCl4 Dipole BrF5 Dipole
    BF3 No dipole SCl6 No dipole PH3 Dipole
    NF3 Dipole SO42- No dipole CO32- No dipole
    SiCl4 No dipole ClO3- Dipole CH2O Dipole
    NO3- No dipole O3 Dipole CCl4 No dipole
    AlH3 No dipole SO2 Dipole SO3 No dipole
    CO Dipole CHCl3 Dipole BrF3 Dipole
    H2S Dipole I3- No dipole H3O+ Dipole

    This page titled Solutions is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Mark Draganjac via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request.