The molecular geometry of SCl4 sulfur tetrachloride can be determined using the VSEPR Valence Shell Electron Pair Repulsion theory. First, let's determine the central atom, which is sulfur S in this case. Next, we need to find the number of valence electrons for sulfur and chlorine. Sulfur has 6 valence electrons, and chlorine has 7 valence electrons. Since there are 4 chlorine atoms, the total number of valence electrons in the molecule is 6 + 4 7 = 34.Now, we'll distribute these electrons in the molecule. Sulfur will form single bonds with each of the 4 chlorine atoms, using 8 electrons. This leaves 26 electrons, which will be distributed as lone pairs on the chlorine atoms. Each chlorine atom will have 3 lone pairs, using up 24 electrons, and the remaining 2 electrons will be a lone pair on the sulfur atom.Considering the lone pairs and bonding pairs around the central sulfur atom, we have a total of 5 electron groups 4 bonding pairs and 1 lone pair . According to the VSEPR theory, this arrangement corresponds to a trigonal bipyramidal electron geometry. However, since there is a lone pair on the sulfur atom, the molecular geometry will be "see-saw" or "distorted tetrahedral" shape.To determine the polarity of SCl4, we need to consider the electronegativity difference between sulfur and chlorine. Chlorine is more electronegative than sulfur, so the S-Cl bonds are polar. However, due to the see-saw molecular geometry, the bond dipoles do not cancel each other out, resulting in a net molecular dipole moment. Therefore, SCl4 is a polar molecule.