Tin(IV) chloride has a tetrahedral shape according to the VSPER theory. The VSEPR theory predicts a molecule's shape based on the available number of bonding electrons available. Those electrons, having negative charges, oppose each other and influence the shape and structure of the molecule. Tin has 4 e- available for bonding in tin (IV). Chlorine has room to accept one electron in it's outer shell, so four chlorine atoms will bond onto the one tin atom. The structure of the resulting molecule, tin(IV) chloride, SnCl4, is tetrahedral, with tin in the very center, a chlorine extending straight up above it, and three other chlorine atoms extending outward and down from the tin, similar to a tripod base.