Final answer:
SCl2 has a Lewis structure with a steric number of 4, a VSEPR formula AX2E2, a tetrahedral electron pair geometry, bent molecular shape, bond angle less than 109.5 degrees, and is polar due to its asymmetrical shape and polar bonds.
Step-by-step explanation:
To understand the molecule SCl2, first, draw the Lewis structure. Sulfur (S) has six valence electrons and forms two single bonds with two chlorine (Cl) atoms, each of which also has seven valence electrons. This results in S having two lone pairs and a steric number of 4.
Using VSEPR theory, the number of regions of electron density around the sulfur atom is four (two bonding regions and two lone pairs). Therefore, the VSEPR formula for SCl2 is AX2E2.
The electron pair geometry is tetrahedral because there are four regions of electron density. However, due to the two lone pairs, the molecular shape is bent or angular. The bond angle is approximately < 109.5 degrees, typically around 104 degrees due to the repulsion caused by the lone pairs.
The polarity of the molecule is determined by the presence of polar bonds and the molecule's asymmetrical shape. SCl2 has polar bonds and an asymmetric shape, indicating that SCl2 is a polar molecule.