How do covalent compounds conduct electricity?

Covalent compounds are substances in which atoms are joined by covalent bonds—formed when two non-metals (often with similar electronegativities, sometimes the same element) share pairs of valence electrons rather than transfer them.

Key properties (typical of simple molecular covalent substances):

1. Strong covalent bonds hold atoms together within each molecule.
2. These bonds require significant energy to break at the atomic level, though values vary by bond/type.
3. Many simple covalent compounds have low melting and boiling points (weak intermolecular forces).
4. They usually have low enthalpies of fusion and vaporization.

Electrical conduction: Because covalent compounds lack free ions or mobile electrons in the liquid/solid state, they do not conduct electricity (exceptions exist in special cases, e.g., graphite).

Pure covalent compounds are generally non-conductors of electricity.