IGCSE Chemistry Practice Exam 2026 - Free IGCSE Chemistry Practice Questions and Study Guide

Covalent compounds, such as water (H₂O), do not conduct electricity primarily because there are no charged particles that are free to move. In covalent compounds, atoms share electrons to achieve stable electron configurations. This electron sharing does not create charged species (ions) that are necessary for conducting electricity.

In ionic compounds, on the other hand, the presence of charged ions allows for the movement of electrical current when these compounds are dissolved in water or molten. However, in the case of covalent compounds, the molecular structure does not produce any free ions, even when they are in a liquid state.

While covalent compounds can dissolve in water and may form polar molecules, they do not split into ions, which is a requirement for electrical conductivity. Therefore, the lack of movable charged particles in covalent substances like water is the reason they do not conduct electricity.