Ionic bonds typically form between metals and nonmetals. Metals, which are found on the left side of the periodic table, tend to have few electrons in their outer shell and are willing to lose them in order to achieve a stable electron configuration. This loss of electrons results in the formation of positively charged ions, known as cations.
On the other hand, nonmetals, which are located on the right side of the periodic table, have more electrons in their outer shell and tend to gain electrons to fill their outer shell, achieving stability. This process results in the formation of negatively charged ions, known as anions.
The electrostatic attraction between the positively charged cations and negatively charged anions leads to the formation of ionic bonds. Common examples of ionic bonds can be observed in compounds like sodium chloride (NaCl), where sodium (a metal) donates an electron to chlorine (a nonmetal), resulting in a stable ionic compound.