Question

What is the electron-pair and molecular geometry around the central \(\mathrm{S}\) atom in sulfury \(\mathrm{chloride}, \mathrm{SO}_{2} \mathrm{Cl}_{2} ?\) What is the hybridization of sulfur in this compound?

Short answer

The electron-pair and molecular geometry are tetrahedral; sulfur is \(sp^3\) hybridized.

Step-by-step solution

Determine Valence Electrons

Sulfur (S) has 6 valence electrons, each Oxygen (O) has 6, and each Chlorine (Cl) has 7. Calculating total: \(1 \times 6 + 2 \times 6 + 2 \times 7 = 32\) electrons.

Draw the Lewis Structure

The Lewis structure of \(\text{SO}_2\text{Cl}_2\) shows sulfur in the center with single bonds to two chlorine atoms and one double bond to each oxygen atom, fulfilling the octet rule for all atoms.

Identify Electron-Pair Geometry

Sulfur has four regions of electron density (two bonds with Cl, two double bonds with O), resulting in a tetrahedral electron-pair geometry.

Determine Molecular Geometry

All bonds are with different atoms, so there are no lone pairs on sulfur. The molecular geometry corresponds to the electron-pair geometry, which is also tetrahedral.

Find Hybridization

With four regions of electron density, sulfur is \(sp^3\) hybridized, as \(sp^3\) corresponds to a tetrahedral arrangement.

Key concepts

Lewis Structure

To understand the shape and behavior of a molecule like sulfuryl chloride (\( \text{SO}_2\text{Cl}_2 \)), we first need to identify the Lewis structure. Lewis structures are diagrams that show the bonding between atoms of a molecule, as well as any lone pairs of electrons. For \( \text{SO}_2\text{Cl}_2 \), sulfur is the central atom. This is because it's usually the atom with the least electronegativity (other than hydrogen), making it a good central atom. Sulfur forms single bonds with two chlorine atoms and double bonds with two oxygen atoms. This arrangement satisfies the octet rule, ensuring each atom's outer shell is filled. By drawing out the Lewis structure, we can visualize the particular bonds and understand the arrangement of electrons around our central sulfur atom.

Electron-Pair Geometry

Electron-pair geometry considers all regions of electron density around the central atom, including bonds and lone pairs. For sulfuryl chloride, sulfur is surrounded by four regions of electron density: two single bonds to chlorine and two double bonds to oxygen. This gives every region equal importance, indicating a tetrahedral electron-pair geometry. Understanding the electron-pair geometry helps predict molecular shapes by showing how electron pairs or bonds are distributed in three-dimensional space. It’s like imagining a central core with electron clouds stretching out equally in all directions, ensuring minimal repulsion and maximum stability.

Hybridization

Hybridization explains how atomic orbitals mix to form new hybrid orbitals, leading to new bonding properties. In \( \text{SO}_2\text{Cl}_2 \), sulfur needs to form four bonds—one with each atom. Thus, it adopts a hybridization that allows for such an arrangement. Sulfur in this molecule undergoes \( sp^3 \) hybridization. This means one \( s \) orbital and three \( p \) orbitals combine, creating four equivalent \( sp^3 \) hybrid orbitals. These orbitals then form the shape that corresponds with a tetrahedral arrangement, providing insights into the bonding framework and molecular geometry.

Molecular Geometry

While electron-pair geometry considers both bonding and non-bonding pairs, molecular geometry focuses only on the bonding pairs. For \( \text{SO}_2\text{Cl}_2 \), since all electron density regions are involved in bonding and there are no lone pairs on sulfur, the molecular geometry mirrors the electron-pair geometry, which is tetrahedral. By examining the molecular geometry, we see how the atoms are precisely positioned in space. This understanding helps predict how the molecule interacts chemically and physically with other substances, highlighting important practical insights into its properties.