Ionic Bonding

Basic Concepts

Ionic bonding occurs when atoms transfer electrons to achieve a full outer electron shell.
It typically occurs between metals and non-metals where metals lose electrons, and non-metals gain them.
The atom that loses an electron becomes a positively charged ion, or cation.
The atom that gains an electron becomes a negatively charged ion, or anion.
The resulting electrostatic attraction between oppositely charged ions forms the ionic bond.

Properties of Ionic Compounds

Ionic compounds form crystalline structures due to the arrangement of ions in a regular, repeating pattern.
They have high melting and boiling points because of the strong ionic bonds that require significant energy to be broken.
Ionic compounds can conduct electricity when melted or dissolved in water as the ions are free to move.

Formation of Ions

Ions form when an atom loses or gains electrons to gain a stable electronic configuration.
Metals form positive ions by losing electrons, while non-metals form negative ions by gaining electrons.

Examples of Ionic Bonding

An example of an ionic bond is seen in sodium chloride, NaCl, where sodium (Na) loses an electron to chlorine (Cl).
This forms a positive sodium ion, Na+, and a negative chloride ion, Cl-, which are attracted to each other to form an ionic bond.

Stability in Ionic Bonding

The transfer of electrons during ionic bonding leads to a more stable electron configuration for both ions.
Stable electron configurations are often achieved when an atom has a full outermost energy level, typically with eight valence electrons.
This stability explains why elements tend to form ions in the first place, contributing to the formation of ionic compounds.

Familiarity with the process and properties of ionic bonding is key to understanding many chemical phenomena. Learning these points helps to build foundational knowledge in chemistry.