Final answer:
The hybridization of both sulfur atoms in S2Cl₂ is sp³ due to four regions of electron density, resulting in a bent or V-shaped molecular geometry around each sulfur atom. The chlorine atoms are also sp³ hybridized.
Step-by-step explanation:
Hybridization and Molecular Geometry of S2Cl₂
To determine the hybridization of the sulfur atoms in S2Cl₂, we need to consider the number of regions of electron density around the sulfur atoms. Each sulfur in S2Cl₂ is connected to one sulfur atom and two chlorine atoms, making three regions of electron density from bonding pairs. Additionally, there is a lone pair of electrons on each sulfur, bringing the total to four regions of electron density. According to VSEPR theory, this would result in a tetrahedral electron-pair geometry. However, since one of the positions is occupied by a lone pair, the molecular geometry is ‘bent’ or ‘V-shaped’ around each sulfur atom similar to SO₂ with a modified angle due to the presence of two chlorine atoms. Therefore, the hybridization of the sulfur atoms in S2Cl₂ is sp³.
The chlorine atoms in S2Cl₂ are surrounded by three lone pairs and one bond pair, which is also consistent with an sp³ hybridization state. The geometrical arrangements of these hybrid orbitals support the molecular geometry predicted by VSEPR theory.