Identify each of the following molecules as polar or nonpolar:
a. ${\mathrm{SeF}}_2$
b. ${\mathrm{PBr}}_3$
c. ${\mathrm{SiF}}_4$
d. ${\mathrm{SO}}_2$

We have to identify the ${\mathrm{SeF}}_2$molecules as polar or nonpolar.

${\mathrm{SeF}}_2$has polar properties.
It has a bent shape because it has two lone pairs and two bond pairs.

We have to identify the following molecules as polar or nonpolar.

Because of its asymmetrical form, ${\mathrm{PBr}}_3$ (phosphorus tribromide) is a polar molecule.
The difference in electronegativity is more than $0.5$, making the $\mathrm{P}-\mathrm{Br}$ bonds polar.
However, it is classified as a polar molecule due to its asymmetrical form.

We have to identify the ${\mathrm{PBr}}_3$molecules as polar or nonpolar.

Because the fluorine atoms are organised in a tetrahedral molecule around the centre silicon atom, all of the negative charge regions cancel each other out, ${\mathrm{SiF}}_4$is a nonpolar molecule.

We have to identify the${\mathrm{SiF}}_4$ molecules as polar or nonpolar.

Sulfur dioxide ${\mathrm{SO}}_2$ is a polar substance.
Because of its bent molecular shape, the molecule exhibits a nonzero dipole moment.