9701 · 3.2
Ionic bonding
This lesson explores ionic bonding, the electrostatic force of attraction between oppositely charged ions. We will examine how ions are formed through electron transfer, how they assemble into giant ionic lattices, and how this structure dictates their unique physical properties.
Need to know
What you need to know
- The formula of an ionic compound (e.g., MgCl₂) is an empirical formula, showing the simplest ratio of ions needed for overall electrical neutrality (one Mg²⁺ ion for every two Cl⁻ ions).
- The coordination number indicates how many ions of opposite charge surround a central ion. In the sodium chloride (NaCl) lattice, both Na⁺ and Cl⁻ have a coordination number of 6.
- The structure is a crystal lattice, which accounts for the regular, crystalline shapes of ionic solids like salt cubes.
Explanation
Ionic bonding
- The formula of an ionic compound (e.g., MgCl₂) is an empirical formula, showing the simplest ratio of ions needed for overall electrical neutrality (one Mg²⁺ ion for every two Cl⁻ ions).
- The coordination number indicates how many ions of opposite charge surround a central ion. In the sodium chloride (NaCl) lattice, both Na⁺ and Cl⁻ have a coordination number of 6.
- The structure is a crystal lattice, which accounts for the regular, crystalline shapes of ionic solids like salt cubes.