Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 11.6 and 11.7. a. COCl2 (carbon is the central atom)

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Identify the central atom in the molecule COCl_2, which is carbon.

Determine the number of valence electrons for each atom: Carbon (4), Oxygen (6), and Chlorine (7 each).

Draw the Lewis structure for COCl_2, ensuring that all atoms satisfy the octet rule where possible.

Determine the steric number of the central carbon atom by counting the number of atoms bonded to it and the number of lone pairs on it. This will help identify the hybridization.

Based on the steric number, assign the hybridization of the central carbon atom. For example, a steric number of 3 corresponds to sp^2 hybridization.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of COCl2, the central carbon atom undergoes sp2 hybridization, resulting in three equivalent hybrid orbitals that can form sigma bonds with the two chlorine atoms and the oxygen atom.

Bonding and Molecular Geometry

Bonding refers to the interactions between atoms that result in the formation of molecules. The molecular geometry of COCl2 is determined by the arrangement of the bonded atoms and lone pairs around the central carbon atom, which influences the overall shape of the molecule. In this case, the geometry is trigonal planar due to the sp2 hybridization.

Orbital Overlap

Orbital overlap is a key concept in understanding how atoms bond together. It occurs when atomic orbitals from different atoms come close enough to allow their electron clouds to interact, leading to the formation of sigma and pi bonds. In COCl2, the overlap of the sp2 hybrid orbitals of carbon with the p orbitals of chlorine and oxygen results in the formation of sigma bonds, while any remaining p orbitals can participate in pi bonding if applicable.

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