Final answer:
Ionic bonds are formed through the transfer of valence electrons between a metal, which becomes a positively charged cation, and a nonmetal, which becomes a negatively charged anion. This transfer adheres to the octet rule, creating strong electrostatic attractions between the ions whose strength depends on their charges and sizes.
Step-by-step explanation:
Ionic Bonding Explained
An ionic bond is a type of chemical bond formed through the transfer of valence electrons between atoms, leading to the creation of ions with opposite charges. This transfer typically occurs between a metal, which becomes a cation (a positively charged ion), and a nonmetal, which becomes an anion (a negatively charged ion). The resulting attraction between these oppositely charged ions holds them together in a compound.
Cations are formed when atoms, such as sodium (Na) or calcium (Ca), lose one or more of their valence electrons. On the other hand, anions are formed when atoms like chlorine (Cl) or oxygen (O) gain one or more electrons. According to the octet rule, atoms tend to transfer electrons in such a way as to achieve a full set of eight valence electrons, resembling the electron configuration of a noble gas.
The strength of ionic bonding depends on the magnitude of the charges on the ions and the sizes of the ions. Ions with greater charges will have a stronger ionic bond. When these ions arrange themselves in a 3D crystal lattice, they do so in a manner that maximizes attractive interactions and minimizes repulsive ones. Ions of the same charge repel each other, while ions with opposite charges attract each other.