Ionic bonds

Definition

Ionic bonds are a type of chemical bond formed through the electrostatic attraction between oppositely charged ions. Typically, these bonds form when a metal donates one or more electrons to a non-metal.

5 Must Know Facts For Your Next Test

1. Ionic bonds result from the transfer of electrons from one atom to another, typically between metals and non-metals.
2. Compounds with ionic bonds usually have high melting and boiling points due to strong electrostatic forces.
3. Ionic compounds are often soluble in water and other polar solvents but insoluble in non-polar solvents.
4. In solid form, ionic compounds form crystalline lattice structures that contribute to their hardness and brittleness.
5. When dissolved in water or melted, ionic compounds conduct electricity because the ions are free to move.

Review Questions

• What types of elements typically participate in the formation of ionic bonds?
• How do the properties of ionic compounds differ from those of covalent compounds?
• Why do ionic compounds conduct electricity in aqueous solution but not in solid form?

Related terms

Electron Transfer:

The process by which an electron moves from one atom or molecule to another during the formation of an ionic bond.

Electrostatic Attraction:

The force that draws oppositely charged ions together in an ionic bond.

Crystal Lattice: A repeating three-dimensional arrangement of atoms or ions in an ionic compound that contributes to its structural stability.