Question

question 7 of 10
how does the shape of a molecule affect the polarity of the molecule?

a. a molecule that has a symmetrical shape will be a nonpolar
molecule.

b. a molecule that is symmetrical in shape will have nonpolar bonds.

c. a molecule with polar bonds will be polar, regardless of its shape.

d. a molecule that is not symmetrical will be a nonpolar molecule.

Explanation:

• Option A: If a molecule has a symmetrical shape, the dipole moments of its polar bonds (if any) tend to cancel out, resulting in a nonpolar molecule. For example, in \( \text{CO}_2 \) (linear and symmetrical), the polar \( \text{C}=\text{O} \) bonds' dipoles cancel, making it nonpolar.
• Option B: Symmetry of the molecule doesn't determine if bonds are nonpolar. A symmetrical molecule can have polar bonds (e.g., \( \text{CO}_2 \) has polar \( \text{C}=\text{O} \) bonds but is symmetrical).
• Option C: A molecule with polar bonds isn't always polar. If the shape is symmetrical, the dipoles can cancel (e.g., \( \text{BF}_3 \) has polar \( \text{B}-\text{F} \) bonds but is nonpolar due to trigonal planar symmetry).
• Option D: A nonsymmetrical molecule with polar bonds will likely be polar (e.g., \( \text{H}_2\text{O} \) is bent and polar), so this is incorrect.

Answer:

A. A molecule that has a symmetrical shape will be a nonpolar molecule.