Calcium chloride CaCl2 exhibits ionic bonding. This type of bonding occurs between a metal and a non-metal, where one or more electrons are transferred from the metal to the non-metal, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions are then attracted to each other, forming an ionic compound.In the case of calcium chloride, calcium Ca is a metal from Group 2 of the periodic table, and chlorine Cl is a non-metal from Group 17. Calcium has two valence electrons, while chlorine has seven valence electrons. Calcium loses its two valence electrons to achieve a stable electron configuration, forming a Ca2+ cation. Each chlorine atom gains one electron to complete its octet, forming Cl- anions. The resulting compound, CaCl2, consists of one Ca2+ cation and two Cl- anions held together by strong electrostatic forces.The specific characteristics of calcium chloride that support its classification as an ionic compound include:1. High melting and boiling points: Ionic compounds typically have high melting and boiling points due to the strong electrostatic forces between the ions. Calcium chloride has a melting point of 772C 1,422F and a boiling point of 1,935C 3,515F , which are consistent with ionic bonding.2. Solubility in water: Ionic compounds generally dissolve in polar solvents like water, as the polar solvent molecules can surround and separate the ions, overcoming the electrostatic forces holding them together. Calcium chloride is highly soluble in water.3. Conductivity: In the solid state, ionic compounds do not conduct electricity because the ions are held in fixed positions within the crystal lattice. However, when dissolved in water or melted, the ions become free to move, allowing the substance to conduct electricity. Calcium chloride exhibits these properties, further supporting its classification as an ionic compound.