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Chapter 20: Problem 66

Describe the bonding in \(\mathrm{SO}_{2}\) and \(\mathrm{SO}_{3}\) using the localized electron model (hybrid orbital theory). How would the molecular orbital model describe the \(\pi\) bonding in these two compounds?

Short Answer

Expert verified
In both SO₂ and SO₃, sulfur is the central atom with trigonal planar electron domain geometry. In SO₂, sulfur undergoes sp² hybridization and forms two σ bonds with oxygen atoms, along with two π bonds created by overlapping p-orbitals. In SO₃, sulfur also undergoes sp² hybridization and forms three σ bonds with oxygen atoms, while the π electrons are delocalized over the entire molecule, resulting in resonance structures. In the molecular orbital model, the π bonding in SO₂ comprises one bonding π MO, one non-bonding MO, and one antibonding π* MO. In SO₃, the π bonding involves two bonding π MOs, one non-bonding MO, and one antibonding π* MO, accounting for delocalization and resonance.

Step by step solution

01

Electron Domain Geometry of SO₂

In the SO₂ molecule, the central atom S has 6 valence electrons, and each Oxygen atom contributes 6 valence electrons. Therefore, there are 18 valence electrons in total. The S atom forms two sigma bonds with the 2 O atoms and has one lone pair. So, there are three electron domains, and according to the VSEPR model, the electron domain geometry is trigonal planar.
02

Electron Domain Geometry of SO₃

In the SO₃ molecule, the central atom S has 6 valence electrons, and each Oxygen atom contributes 6 valence electrons. Therefore, there are 24 valence electrons in total. The S atom forms three sigma bonds with the 3 O atoms. So, there are three electron domains, and according to the VSEPR model, the electron domain geometry is trigonal planar. Step 2: Determining the Hybridization of the Central Atom
03

Hybridization of S in SO₂

Since the electron domain geometry of SO₂ is trigonal planar, the central atom S undergoes sp² hybridization, forming 3 sp² hybrid orbitals.
04

Hybridization of S in SO₃

Since the electron domain geometry of SO₃ is trigonal planar, the central atom S undergoes sp² hybridization, forming 3 sp² hybrid orbitals. Step 3: Describing the π Bonding using the Localized Electron Model
05

π Bonding in SO₂

In SO₂, one unhybridized p-orbital from the S and each of the two O atoms are involved in the π bonding. These p-orbitals overlap side-by-side, forming two π bonds.
06

π Bonding in SO₃

In SO₃, one unhybridized p-orbital from the S and each of the three O atoms contribute to the π bonding. The π electrons are delocalized over the entire molecule, resulting in resonance structures with one double bond and two single bonds between S and the O atoms. Step 4: Describing the π Bonding in the Molecular Orbital Model
07

Molecular Orbital Description of π Bonding in SO₂

In the molecular orbital model, the π bonding in SO₂ is described as the overlap of the three p-orbitals (one from S and two from O atoms) to form three molecular orbitals: one bonding π MO (occupied by two electrons), one non-bonding MO (occupied by two electrons), and one antibonding π* MO (occupied by zero electrons).
08

Molecular Orbital Description of π Bonding in SO₃

In the molecular orbital model, the π bonding in SO₃ is described as the overlap of four p-orbitals (one from S and three from O atoms) to form four molecular orbitals: two bonding π MOs (each occupied by two electrons), one non-bonding MO (occupied by two electrons), and one antibonding π* MO (occupied by zero electrons). This accounts for the delocalization and resonance observed in the SO₃ molecule.

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