Certainly! Let's analyze the given options to determine which formula represents a nonpolar molecule containing polar covalent bonds.
1. [tex]\(H - H\)[/tex]:
- The bond [tex]\(H - H\)[/tex] is a bond between two hydrogen atoms.
- Since both atoms are identical and have the same electronegativity, the electrons are shared equally.
- Therefore, the [tex]\(H - H\)[/tex] bond is nonpolar.
2. [tex]\(O = C = O\)[/tex]:
- This is the structural formula for carbon dioxide ([tex]\(\text{CO}_2\)[/tex]).
- In this molecule, there are two double bonds: one between the carbon and each oxygen.
- The bonds between carbon and oxygen are polar covalent bonds due to the difference in electronegativity between carbon and oxygen.
- However, the molecular geometry of [tex]\(\text{CO}_2\)[/tex] is linear, causing the polarities of the two [tex]\(\text{C=O}\)[/tex] bonds to cancel each other out.
- As a result, the overall molecule is nonpolar despite containing polar covalent bonds.
3. (no option given)
4. (no option given)
Considering the options provided, option 2 ([tex]\(O = C = O\)[/tex]) is the correct choice. It represents carbon dioxide, a nonpolar molecule that contains polar covalent bonds.
So, the formula that represents a nonpolar molecule containing polar covalent bonds is:
[tex]\[ \boxed{O = C = O} \][/tex]
