Ionic bond

Definition

An ionic bond is a type of chemical bond that forms when electrons are transferred from one atom to another, resulting in the formation of charged ions. This bond typically occurs between metals, which lose electrons and become positively charged cations, and nonmetals, which gain electrons to become negatively charged anions. The electrostatic attraction between these oppositely charged ions leads to the formation of a stable compound.

5 Must Know Facts For Your Next Test

1. Ionic bonds are generally strong due to the significant electrostatic forces between the charged ions, resulting in high melting and boiling points for ionic compounds.
2. When ionic compounds dissolve in water, they dissociate into their constituent ions, making them good conductors of electricity in solution.
3. Ionic bonds are often formed between elements from groups 1 and 2 of the periodic table (metals) and groups 16 and 17 (nonmetals).
4. The formation of ionic bonds often leads to the creation of crystalline structures, such as sodium chloride (table salt), which can be observed as a repeating pattern in solid form.
5. The ability of metals to lose electrons and nonmetals to gain them is influenced by their positions on the periodic table and their electronegativities.

Review Questions

• How does the difference in electronegativity between two elements influence the formation of an ionic bond?
  • The difference in electronegativity between two elements is crucial in determining whether an ionic bond will form. When one element has a significantly higher electronegativity than another, it will attract electrons more strongly. This results in the transfer of electrons from the less electronegative atom (usually a metal) to the more electronegative atom (usually a nonmetal), leading to the formation of cations and anions. The resulting electrostatic attraction between these oppositely charged ions creates a stable ionic bond.
• Compare and contrast ionic bonds with covalent bonds, highlighting their formation and properties.
  • Ionic bonds form through the transfer of electrons from one atom to another, resulting in the creation of charged ions that attract each other due to electrostatic forces. In contrast, covalent bonds are formed when two atoms share electrons, leading to the formation of molecules. Ionic compounds typically have high melting and boiling points, are usually soluble in water, and conduct electricity when dissolved or melted. Covalent compounds often have lower melting and boiling points and can be either soluble or insoluble in water depending on their polarity.
• Evaluate the role of lattice energy in determining the stability of ionic compounds and their physical properties.
  • Lattice energy plays a significant role in determining both the stability and physical properties of ionic compounds. It represents the amount of energy released when gaseous ions come together to form a solid lattice structure. Higher lattice energy indicates stronger ionic bonds, which correlate with higher melting and boiling points. The stability imparted by high lattice energy also affects solubility; compounds with lower lattice energy tend to dissolve more readily in solvents. Therefore, understanding lattice energy helps explain why certain ionic compounds are more stable and have distinct physical characteristics compared to others.

Related terms

covalent bond: A covalent bond is a type of chemical bond where two atoms share one or more pairs of electrons, allowing them to attain stable electron configurations.

electronegativity: Electronegativity is the tendency of an atom to attract electrons towards itself in a chemical bond, influencing the type of bonding that occurs between atoms.

lattice energy: Lattice energy is the energy released when ions in the gas phase combine to form an ionic solid; it reflects the strength of the ionic bonds in a crystalline lattice.