In the compound CO(NH3)6, which hybrid orbitals overlap to form the C–N bond?

• A. sp hybrid orbital of carbon and sp3 hybrid orbital of nitrogen
• B. sp hybrid orbital of carbon and sp2 hybrid orbital of nitrogen
• C. sp3 hybrid orbital of carbon and sp3 hybrid orbital of nitrogen
• D. sp2 hybrid orbital of carbon and sp2 hybrid orbital of nitrogen

Answer: (A)

Verified step by step guidance

1. Identify the central atoms involved in the C–N bond within the compound CO(NH3)6. Here, the bond is between carbon (C) and nitrogen (N).
2. Determine the hybridization of the carbon atom in the compound. Consider the bonding environment of carbon, including the number and types of atoms it is bonded to, and use the steric number (number of sigma bonds + lone pairs) to find the hybridization.
3. Determine the hybridization of the nitrogen atom in the NH3 ligand. Recall that nitrogen in ammonia (NH3) typically has three sigma bonds and one lone pair, which corresponds to sp3 hybridization.
4. Understand that the C–N bond forms by the overlap of the hybrid orbitals from carbon and nitrogen. The type of hybrid orbitals involved depends on the hybridization states determined in the previous steps.
5. Conclude which hybrid orbitals overlap to form the C–N bond by matching the hybridization of carbon and nitrogen. For example, if carbon is sp hybridized and nitrogen is sp3 hybridized, then the bond forms by overlap of carbon's sp orbital with nitrogen's sp3 orbital.