In the Lewis structure of carbon dioxide (CO_2), which atomic orbitals overlap to form the sigma and pi bonds between carbon and oxygen atoms?

• A. The sigma bonds are formed by the overlap of d orbitals on carbon with p orbitals on oxygen, and the pi bonds are formed by the overlap of s orbitals.
• B. The sigma bonds are formed by the overlap of sp hybrid orbitals on carbon with p orbitals on oxygen, and the pi bonds are formed by the sideways overlap of unhybridized p orbitals.
• C. Both the sigma and pi bonds are formed exclusively by the overlap of s orbitals on carbon and oxygen.
• D. The sigma bonds are formed by the overlap of p orbitals on carbon with s orbitals on oxygen, and the pi bonds are formed by the overlap of sp^2 hybrid orbitals.

Answer: (B)

Verified step by step guidance

1. Recall that in carbon dioxide (CO_2), the central carbon atom forms two double bonds with two oxygen atoms, each double bond consisting of one sigma (σ) bond and one pi (π) bond.
2. Understand that sigma bonds are formed by the head-on (end-to-end) overlap of orbitals, while pi bonds are formed by the sideways (lateral) overlap of orbitals.
3. Recognize that carbon undergoes sp hybridization in CO_2, which means it forms two sp hybrid orbitals and has two unhybridized p orbitals remaining.
4. Identify that the sigma bonds between carbon and oxygen are formed by the overlap of the sp hybrid orbitals on carbon with the p orbitals on oxygen (which are oriented along the bond axis).
5. Note that the pi bonds are formed by the sideways overlap of the unhybridized p orbitals on carbon with the unhybridized p orbitals on oxygen, creating the double bond's pi component.