The molecular geometry of SiF4 (silicon tetrafluoride) can be predicted using the Valence Shell Electron Pair Repulsion (VSEPR) theory. According to VSEPR theory, the shape of a molecule is determined by the repulsion between the electron pairs in the valence shell of the central atom.
In SiF4, silicon (Si) is the central atom, and it is bonded to four fluorine (F) atoms. Silicon has four valence electrons, and each fluorine atom contributes one electron to form a covalent bond. Therefore, the total number of electron pairs around the silicon atom is four, all of which are bonding pairs.
Since there are no lone pairs on the silicon atom and all four bonds are equivalent, the distribution of electron pairs is symmetrical. This configuration leads to a tetrahedral geometry. The angles between the bonding pairs in a tetrahedral structure are approximately 109.5 degrees.
In summary, based on VSEPR theory, SiF4 exhibits a tetrahedral molecular geometry due to the presence of four bonding pairs of electrons around the central silicon atom, with no lone pairs affecting the shape.