Chapter 8, Problem 61A

Interpretation Introduction

Interpretation:

The molecule ${\text{CO}}_{\text{2}}$ has two carbon-oxygen double bonds. Describe the bonding and hybridized orbitals involves in the ${\text{CO}}_{\text{2}}$ .

Concept introduction:

When a group of atoms bonded together, they form a molecule. In ${\text{CO}}_{\text{2}}$ , two carbon and oxygen atom are bonded together and forms a double bond.

Answer to Problem 61A

Only one $\text{2s}$ and one $\text{2p}$ orbital need to combine to create two $\text{sp}$ hybrid orbitals on the carbon atom because carbon only needs to form two double bonds with the oxygens.

Explanation of Solution

Only one $\text{2s}$ and one $\text{2p}$ orbital need to combine to form two $\text{sp}$ hybrid orbitals on the carbon atom because carbon only needs to form two double bonds with the oxygens. Between each $\text{O}$ and $\text{C}$ , a single $\text{sp}$ hybrid orbital creates a sigma bond. Unhybridized $\text{2p}$ orbitals then create pi bonds between $\text{C}$ and $\text{O}$ . $$

  

Conclusion

• The hybridization of ${\text{CO}}_{\text{2}}$ molecules is $\text{sp}$ .
• Single $\text{sp}$ hybrid orbital creates a sigma bond.