Question

question 1
1 pts
cbr₄ select
select
polar molecule
nonpolar molecule
question 2
1 pts
pyramidal molecular geometry select
question 3
1 pts
co₂ select

Explanation:

Question 1

To determine if \( CBr_4 \) is polar or nonpolar, we analyze its molecular geometry and bond polarities. \( CBr_4 \) has a tetrahedral geometry, with carbon at the center and four bromine atoms bonded to it. The \( C - Br \) bonds are polar, but due to the symmetric tetrahedral arrangement, the bond dipoles cancel out, resulting in a nonpolar molecule.

Pyramidal molecular geometry (e.g., \( NH_3 \)) has a central atom with one lone pair and three bonded atoms. The lone pair - bond pair repulsion creates an asymmetric shape, leading to a net dipole moment. Thus, molecules with pyramidal geometry are usually polar.

\( CO_2 \) has a linear molecular geometry (\( O = C = O \)). The polar \( C = O \) bonds are arranged symmetrically, so their dipoles cancel, making \( CO_2 \) a nonpolar molecule.

Answer:

nonpolar molecule

Question 2

(Assuming the options are related to polarity or other molecular properties, but since options aren't provided, we'll focus on pyramidal geometry. Pyramidal molecular geometry (like \( NH_3 \)) has a central atom with a lone pair and three bonded atoms. The lone pair causes a dipole moment, so molecules with pyramidal geometry are typically polar. If options include "polar molecule" as a choice, that would be the answer. However, since the original problem's options for Question 2 aren't fully shown, we'll assume a common context: Pyramidal molecular geometry is associated with polar molecules (due to the lone pair creating an asymmetric charge distribution).)