1. The Lewis structure:To draw the Lewis structure for SF4, we first need to determine the total number of valence electrons. Sulfur S has 6 valence electrons, and each of the four fluorine F atoms has 7 valence electrons. So, the total number of valence electrons is 6 + 4 7 = 34.The Lewis structure for SF4 can be drawn as follows: F |S - F - S - F | FSulfur is the central atom, surrounded by four fluorine atoms. Sulfur has an expanded octet, with 10 electrons around it 2 electrons in each of the four single bonds and one lone pair . Each fluorine atom is connected to the sulfur atom with a single bond and has three lone pairs.2. The molecular geometry:The molecular geometry of SF4 can be determined using the VSEPR Valence Shell Electron Pair Repulsion theory. The central sulfur atom has a total of five electron groups four single bonds to fluorine atoms and one lone pair . According to VSEPR theory, these electron groups will arrange themselves to minimize repulsion. In this case, the molecular geometry is "see-saw" or "distorted tetrahedral."3. The polarity of the molecule:To determine the polarity of the molecule, we need to consider the electronegativity difference between the atoms and the molecular geometry. Fluorine is more electronegative than sulfur, so the S-F bonds are polar. However, due to the see-saw molecular geometry, these bond dipoles do not cancel each other out, resulting in a net molecular dipole moment. Therefore, the SF4 molecule is polar.