The geometry of the SiCl4 Silicon tetrachloride molecule is tetrahedral. In a tetrahedral molecular geometry, a central atom is located at the center with four substituents in this case, four chlorine atoms that are located at the corners of a tetrahedron. The bond angles in a tetrahedral molecule are approximately 109.5 degrees.As for the polarity of SiCl4, it is a nonpolar molecule. Although the Si-Cl bond is polar due to the difference in electronegativity between Silicon 1.90 and Chlorine 3.16 , the overall molecule is nonpolar. This is because the four polar bonds are symmetrically arranged around the central silicon atom, and their dipoles cancel each other out, resulting in a net dipole moment of zero.