The Lewis Structure of SCl2, sulfur dichloride, has a sulfur atom (which brings six valance electrons) bonded two chlorine atoms (which each bring seven valence electrons). By drawing the Lewis Structure accurately, we can determine the shape and hybridization of SCl2 as well.
Since chlorine needs to share just one extra electron to complete its octet, the sulfur is able to share each of its two unpaired electrons to form bonding pairs with chlorine.
Sulfur and Chlorine are both non-metals, which makes these bonds covalent. We can determine the type of covalent bond with a calculation of electronegativity difference: ΔEN = 3.16 – 2.58 = 0.58, which makes the bond polar covalent.
Substances with similar chemical formulas, such as CaBr2, are ionic and so their Lewis Structures are drawn very differently.
The lewis structure is shown here:
The sulfur atom here has two bonding pairs (shown as horizontal lines) and two lone pairs (shown as two dots for each pair). None of these require pi-bonding (which is the method of formation for double and triple bonds). Thus, the hybridization of SCl2 is sp3.
In addition, because there are two bonding pairs and two lone pairs, we can say that the VSEPR notation is AX2E2 and the molecular shape is angular/bent. Indeed, the bond angle is significantly less than it would be in tetrahedral, since the lone pairs take up more space than bonding pairs. The bond angle in SCl2 is 103 degrees (Source).