Which of the following molecules has a zero dipole moment?

Question

Quizplus · Accepted Answer

To determine the dipole moment, we need to look at the polarity of each molecule. Each molecule has polar covalent bonds, but we also need to take the shape of the molecule into account. A molecule with polar bonds but a symmetrical shape will have a dipole moment of zero. Option A (NCl₃) has trigonal bipyramidal molecular geometry, which is not symmetrical so it is polar. Option B (CO₂) has linear molecular geometry, and the dipole moments of the C=O and C-S bonds cancel each other out due to their oppositely directed polar bonds. Option C (SCl₄) has see-saw molecular geometry which is not symmetrical so it is polar. Option D (H₂O) has bent (V-shaped) molecular geometry which is polar due to electronegativity difference between H and O atoms. Option E (ICl₃) has a symmetrical T-shaped molecular geometry but it is not linear. So it is polar.

Which of the Following Molecules Has a Zero Dipole Moment