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. d. I3–

Key Concepts

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 I3–, the central iodine atom undergoes sp3 hybridization, which allows it to form bonds with the surrounding iodine atoms while accommodating lone pairs of electrons.

Bonding and Molecular Geometry

Bonding refers to the interactions between atoms that lead to the formation of molecules. The molecular geometry of I3– can be determined using the VSEPR theory, which predicts that the arrangement of electron pairs around the central atom will minimize repulsion, resulting in a linear shape due to the presence of three bonding pairs and two lone pairs.

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 covalent bonds. In I3–, the overlap of the hybridized orbitals of iodine atoms facilitates the formation of sigma bonds, while any remaining p orbitals can participate in pi bonding if applicable.