An ionic bond is formed when atoms transfer electrons from one to another, leading to the formation of ions. The attraction between these oppositely charged ions—cations (positively charged) and anions (negatively charged)—is what holds them together in an ionic bond.
When an atom loses an electron, it becomes positively charged, while an atom that gains an electron becomes negatively charged. This transfer of electrons typically occurs between metals and non-metals. For example, sodium (a metal) loses an electron to become Na+, while chlorine (a non-metal) gains an electron to become Cl–.
The electrostatic force of attraction between these charged ions is quite strong and is the primary reason why ionic compounds tend to form stable structures. This attraction not only influences how these compounds behave in various conditions but also affects their melting and boiling points, solubility, and electrical conductivity. Overall, the essential driving force behind the formation of ionic bonds is the balance of electrical charges that leads to stability within the resulting compound.