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### Each compound contains both ionic and covalent bo…

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WM
The University of Alabama

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Problem 74

Determine whether each molecule is polar or nonpolar.
a. SiCl4
b. CF2Cl2
c. SeF6
d. IF5

a. In the Lewis structure, the central Si atom has four electron groups with no lone pairs. So the
geometry of the molecule is tetrahedral. Even though each of the bonds is polar, the molecule is
non polar as the dipole moments cancel each other.
b. The $\mathrm{C}-\mathrm{Cl}$ bonds and the $\mathrm{C}-\mathrm{F}$ bonds have different polarities. So the molecule is polar.
c. In the Lewis structure, the central Se atom has six electron groups with no lone pairs. So the
geometry is octahedral. The Se-Fbonds are polar but the dipole moments cancel each other.
So the molecule is non polar.
d. In the Lewis structure, the central I atom has six electron groups with one lone pair. So the
geometry is square pyramidal. The I-F bonds are polar and so the molecule is polar.

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## Video Transcript

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