Final answer:
SCl₂ has two lone pairs and a bent or V-shaped molecular geometry, similar to a trigonal planar arrangement with one vertex missing.
Step-by-step explanation:
The number of lone pairs around the central atom in SCl₂ is two. This is because the central sulfur atom has six valence electrons and forms two single bonds with two chlorine atoms, leaving two pairs of non-bonding electrons, which are lone pairs. The presence of these lone pairs means there are four electron pairs around the central atom. As such, the molecular geometry of SCl₂ is described as bent or V-shaped, similar to that of water (H₂O), with a bond angle slightly less than 109.5° due to lone pair-bond pair repulsion. This bent shape can also be thought of as a trigonal planar arrangement with one vertex missing, where the lone pairs occupy one of the positions.
Each chlorine atom adds seven valence electrons to the six valence electrons of sulfur. The following formula is used to get the total amount of valence electrons:
6(S)+2×7(Cl)=20.
In the Lewis structure, one pair of electrons is used for each S-Cl bond (2×2=4 electrons), leaving 20−4=16 electrons for lone pairs. The lone pairs are accommodated on the sulfur atom.