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Sulphur dioxide has only two bonds at 180º so shouldn't the dipole moment of molecule be 0 and as ammonia has 1 lone pair so it's dipole can't be 0 so how Sulphur dioxide has more dipole moment than ammonia?

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    $\begingroup$ Sulphur dioxide isn't linear - also has a lone pair on central atom. $\endgroup$
    – Mithoron
    Oct 8 '20 at 13:56
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I suggest you visit this page. Sulfur dioxide is almost always in this form. Two Oxygens are more electronegative than a single Nitrogen and also S-O bond is longer than N-H bond, though the dipole moment of S-O is more than N-H and despite the lone pair on S, SO2 has a greater dipole moment than NH3.

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