Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. CCl₄

Verified step by step guidance

1. Identify the central atom in the molecule. In CCl_4, carbon (C) is the central atom.
2. Determine the number of valence electrons for the central atom. Carbon has 4 valence electrons.
3. Count the number of atoms bonded to the central atom. In CCl_4, there are 4 chlorine atoms bonded to carbon.
4. Determine the hybridization of the central atom. Since carbon forms 4 sigma bonds with chlorine, it undergoes sp^3 hybridization.
5. Sketch the molecule: Draw the carbon atom in the center with four sp^3 hybrid orbitals. Each orbital overlaps with a p orbital from a chlorine atom to form a sigma (σ) bond. Label each C-Cl bond as a σ bond.

Key Concepts

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. In the case of CCl4, the carbon atom undergoes sp3 hybridization, resulting in four equivalent hybrid orbitals that arrange themselves in a tetrahedral geometry to minimize electron pair repulsion.

Bonding and Molecular Geometry

Bonding refers to the interactions between atoms that result in the formation of molecules. In CCl4, each of the four sp3 hybrid orbitals of carbon overlaps with the p orbitals of chlorine atoms, forming four sigma (σ) bonds. The molecular geometry is tetrahedral, which is crucial for understanding the spatial arrangement of the atoms and the overall shape of the molecule.

Orbital Overlap Theory

Orbital overlap theory explains how atomic orbitals combine to form bonds in a molecule. In CCl4, the overlap of carbon's sp3 hybrid orbitals with chlorine's p orbitals leads to the formation of sigma bonds. This concept is essential for visualizing the bonding interactions and understanding the strength and characteristics of the bonds formed in the molecule.