Summary
Ionic bonding involves the transfer of electrons between atoms, resulting in the formation of ions with opposite charges that attract each other to form a compound.
- Ionic Bonding — the strong electrostatic attraction between oppositely charged ions. Example: In sodium chloride (NaCl), sodium loses an electron to become Na+ and chlorine gains an electron to become Cl-.
- Ionization — the process of an atom losing or gaining electrons to form ions. Example: Sodium loses one electron to form Na+.
- Lattice Structure — a regular arrangement of ions in a solid, held together by strong electrostatic forces. Example: Sodium chloride forms a lattice structure requiring a lot of energy to break.
- Ionic Radius — the size of a charged ion, influenced by electron number and nuclear charge. Example: As you move down a group, ionic radius increases due to more electron shells.
- Polarisation — distortion of the electron cloud in ionic bonds, influenced by ion charge and size. Example: A smaller, highly charged cation can distort an anion's electron cloud more easily.
Exam Tips
Key Definitions to Remember
- Ionic Bonding: The strong electrostatic attraction between oppositely charged ions.
- Ionization: The process of losing or gaining electrons to form ions.
- Lattice Structure: Regular arrangement of ions in a solid.
- Ionic Radius: Size of a charged ion.
- Polarisation: Distortion of the electron cloud in ionic bonds.
Common Confusions
- Confusing ionic bonding with covalent bonding, which involves sharing electrons.
- Misunderstanding the effect of ionic radius on the strength of ionic bonds.
Typical Exam Questions
- What is ionic bonding? Ionic bonding is the electrostatic attraction between oppositely charged ions.
- How does ionic radius change across a period? It decreases as the positive charge increases, pulling electrons closer.
- What is an example of polarisation in ionic bonds? A small, highly charged cation distorting an anion's electron cloud.
What Examiners Usually Test
- Understanding of how ionic bonds form between metals and non-metals.
- Ability to explain the concept of ionic radius and its trends in the periodic table.
- Knowledge of lattice structures and their properties.