Science, Tech, Math › Science Delocalized Electron Defined in Chemistry It's an electron not associated with a single atom or covalent bond Share Flipboard Email Print Anne Helmenstine Science Chemistry Chemical Laws Basics Molecules Periodic Table Projects & Experiments Scientific Method Biochemistry Physical Chemistry Medical Chemistry Chemistry In Everyday Life Famous Chemists Activities for Kids Abbreviations & Acronyms Biology Physics Geology Astronomy Weather & Climate By Anne Marie Helmenstine, Ph.D. Chemistry Expert Ph.D., Biomedical Sciences, University of Tennessee at Knoxville B.A., Physics and Mathematics, Hastings College Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels. our editorial process Facebook Facebook Twitter Twitter Anne Marie Helmenstine, Ph.D. Updated January 23, 2020 A delocalized electron is an electron in an atom, ion, or molecule not associated with any single atom or a single covalent bond. In a ring structure, delocalized electrons are indicated by drawing a circle rather than single and double bonds. This means the electrons are equally likely to be anywhere along the chemical bond. Delocalized electrons contribute to the conductivity of the atom, ion, or molecule. Materials with many delocalized electrons tend to be highly conductive. Examples In a benzene molecule, for example, the electrical forces on the electrons are uniform across the molecule. The delocalization produces what is called a resonance structure. Delocalized electrons are also commonly seen in solid metals, where they form a "sea" of electrons that are free to move throughout the material. This is why metals are typically excellent electrical conductors. In the crystal structure of a diamond, the four outer electrons of each carbon atom participate in covalent bonding (are localized). Contrast this with bonding in graphite, another form of pure carbon, where only three of the four outer electrons are covalently bonded to other carbon atoms. Each carbon atom has a delocalized electron that participates in chemical bonding but is free to move throughout the plane of the molecule. While the electrons are delocalized, graphite is a planar shape, so the molecule conducts electricity along the plane, but not perpendicular to it.