Science, Tech, Math › Science Antibonding Orbital Definition Share Flipboard Email Print CCoil/CC BY-SA 3.0/Wikimedia Commons 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 November 04, 2019 An antibonding orbital is a molecular orbital containing an electron outside the region between the two nuclei. As two atoms approach each other, their electron orbitals begin to overlap. This overlap forms a molecular bond between the two atoms with its own molecular orbital shape. These orbitals follow the Pauli exclusion principle in the same way as atomic orbitals. No two electrons in an orbital can have the same quantum state. If the original atoms contain electrons where a bond would violate the rules, the electron will populate the higher energy antibonding orbital. Antibonding orbitals are denoted by an asterisk symbol next to the associated type of molecular orbital. σ* is the antibonding orbital associated with sigma orbitals and π* orbitals are antibonding pi orbitals. When speaking of these orbitals, the word 'star' is often added to the end of the orbital name: σ* = sigma-star. Examples H2- is a diatomic molecule containing three electrons. One of the electrons is found in an antibonding orbital. Hydrogen atoms have a single 1s electron. The 1s orbital has room for 2 electrons, a spin "up" electron and a spin "down" electron. If a hydrogen atom contains an extra electron, forming an H- ion, the 1s orbital is filled. If an H atom and H- ion approach each other, a sigma bond will form between the two atoms. Each atom will contribute an electron to the bond filling the lower energy σ bond. The extra electron will fill a higher energy state to avoid interacting with the other two electrons. This higher energy orbital is called the antibonding orbital. In this case, the orbital is a σ* antibonding orbital. Sources Atkins P.; de Paula J. (2006). Atkins Physical Chemistry (8th ed.). W.H. Freeman. ISBN:0-7167-8759-8.Orchin, M.; Jaffe, H.H. (1967). The Importance of Antibonding Orbitals. Houghton Mifflin. ISBN:B0006BPT5O.