An atom of Silicon (Si) is predicted to form four covalent bonds.
Silicon, belonging to Group 14 (also known as Group IVA) of the periodic table, has four valence electrons in its outermost shell. To achieve a stable octet configuration similar to that of noble gases, silicon needs to gain or share four more electrons. This is most readily accomplished through covalent bonding, where silicon shares its four valence electrons with other atoms, forming four covalent bonds. Each covalent bond involves the sharing of one electron pair.
For instance, in silicon dioxide (SiO2), each silicon atom forms four single covalent bonds with four oxygen atoms. Another example is in silicon tetrachloride (SiCl4), each silicon atom bonds with four chlorine atoms. This tetravalency is a characteristic property of silicon, enabling it to form a wide array of compounds.
