AQA GCSE Chemistry Paper 1 Practice Exam 2026 – All-in-One Comprehensive Guide for Exam Success!

The structure of sodium chloride is best described as a giant ionic lattice. This term refers to a three-dimensional arrangement of ions held together by strong electrostatic forces known as ionic bonds. In sodium chloride, sodium ions (Na⁺) and chloride ions (Cl⁻) alternate in a regular repeating pattern, creating a stable and robust structure. This lattice formation contributes to the characteristic properties of sodium chloride, such as its high melting and boiling points, as substantial energy is required to break the ionic bonds in the lattice.

The giant ionic lattice structure explains why sodium chloride forms crystalline solids at room temperature and why it can conduct electricity when dissolved in water or melted, as the ions are then free to move. Other options describe different types of structures; for instance, individual crystals may form from the solid but do not capture the essence of the ionic bonds in a continuous lattice, while a simple molecular structure does not represent how sodium chloride is constructed. A liquid solution characterizes the behavior of sodium chloride when dissolved but does not accurately depict its structural characteristics in the solid state.