Ionic bond

Definition

An ionic bond is a type of chemical bond formed through the electrostatic attraction between oppositely charged ions, typically resulting from the transfer of electrons from one atom to another. This process often occurs between metals and nonmetals, where metals lose electrons to become positively charged cations, and nonmetals gain electrons to become negatively charged anions. The strong attraction between these charged ions leads to the formation of ionic compounds.

5 Must Know Facts For Your Next Test

1. Ionic bonds typically form between elements with significantly different electronegativities, such as sodium (Na) and chlorine (Cl).
2. The resulting ionic compounds usually have high melting and boiling points due to the strong forces of attraction between the ions.
3. Ionic compounds are generally soluble in water and conduct electricity when dissolved or melted, as the ions are free to move.
4. The strength of an ionic bond is influenced by the charges of the ions and the distance between them, described by Coulomb's law.
5. Common examples of ionic compounds include table salt (NaCl) and magnesium oxide (MgO), which exhibit distinct crystal lattice structures.

Review Questions

• How do ionic bonds differ from covalent bonds in terms of electron transfer and charge formation?
  • Ionic bonds involve the transfer of electrons from one atom to another, resulting in the formation of charged ions, whereas covalent bonds involve the sharing of electrons between atoms. In ionic bonding, metals typically lose electrons to become cations, while nonmetals gain electrons to become anions. This difference leads to distinct properties for ionic compounds compared to those formed through covalent bonding, including differences in conductivity and melting points.
• Discuss how lattice energy plays a role in the stability of ionic compounds.
  • Lattice energy is a crucial factor that contributes to the stability of ionic compounds. It measures the energy released when gaseous ions form a solid ionic lattice, indicating the strength of the ionic bonds present. A high lattice energy means that a significant amount of energy is required to break apart the ionic compound into its constituent ions, thus providing stability. This energy can also influence properties like melting point and solubility, as compounds with higher lattice energies tend to have higher melting points.
• Evaluate the implications of ionic bonding on the physical properties of ionic compounds compared to molecular compounds.
  • Ionic bonding has significant implications for the physical properties of ionic compounds compared to molecular compounds. Ionic compounds generally exhibit high melting and boiling points due to the strong electrostatic forces between ions, making them solid at room temperature. In contrast, molecular compounds, which rely on weaker van der Waals forces or covalent bonds, tend to be liquids or gases under similar conditions. Additionally, ionic compounds are often soluble in water and conduct electricity in solution due to their ion mobility, while many molecular compounds do not exhibit these characteristics.

Related terms

Cation: A positively charged ion that is formed when an atom loses one or more electrons.

Anion: A negatively charged ion that is created when an atom gains one or more electrons.

Lattice Energy:

The energy released when oppositely charged ions in the gas phase come together to form an ionic solid; it reflects the strength of the ionic bond.