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 10.6 and 10.7. a. SO₃^2-

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1. Identify the central atom in the molecule or ion. For SO_3^{2-}, the central atom is sulfur (S).
2. Determine the number of valence electrons for the central atom and the surrounding atoms. Sulfur has 6 valence electrons, and each oxygen has 6 valence electrons. The 2- charge adds 2 more electrons, totaling 26 valence electrons.
3. Draw the Lewis structure for the ion, distributing the electrons to satisfy the octet rule for each atom. Place the extra electrons on the central atom if needed.
4. Determine the steric number of the central atom by counting the number of atoms bonded to it and the number of lone pairs. For SO_3^{2-}, sulfur is bonded to three oxygens and has one lone pair, giving a steric number of 4.
5. Based on the steric number, determine the hybridization of the central atom. A steric number of 4 corresponds to sp^3 hybridization. Sketch the structure showing the sp^3 hybrid orbitals on sulfur overlapping with the p orbitals of oxygen, and label the sigma (σ) bonds.

Key Concepts

Hybridization

Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of the sulfate ion (SO3^2-), the central sulfur atom undergoes hybridization to accommodate the bonding with oxygen atoms, typically resulting in sp3 hybridization due to the tetrahedral arrangement of electron pairs.

Bonding and Molecular Geometry

Bonding refers to the interactions between atoms that lead to the formation of molecules or ions. The molecular geometry of SO3^2- is determined by the arrangement of its bonded atoms and lone pairs around the central sulfur atom, which can be predicted using the VSEPR (Valence Shell Electron Pair Repulsion) theory. This results in a trigonal pyramidal shape due to the presence of one lone pair.

Orbital Overlap and Bonding Notation

Orbital overlap is a key concept in understanding how atoms bond together, as it describes the interaction between atomic orbitals of different atoms that leads to the formation of covalent bonds. In the bonding scheme for SO3^2-, it is important to illustrate the overlapping orbitals between sulfur and oxygen atoms, and to label the bonds (single, double) using appropriate notation to indicate the type and strength of the bonds formed.