How to determine the Lewis dot structure of O2?
The Lewis dot, or bonding, diagram is traditionally created with two bonded atoms to represent a chemical bond. A line may be trailed off to mean one of three things: the atom in the tail has only one valence electron, so it’s a metal; that atom has more than two electrons and can’t form bonds and requires an element found on the far right column of its respective table; or it’s not its atomic number. Every connection shown is made with single electrons except for double connections, which are made with either two shared pairings (which results in no overall charge), formation of a large ionic bond between large ions represented by smaller symbols as well as color changes on some bonds before resonance forms between them or 1.5 electrons, which is assumed to happen by having both atoms share one electron.
Oxygen’s molecular orbital diagram is displayed differently with three long-range order parameters that are computed from the real three-dimensional orbitals. To represent their contribution, the lobes are color-coded in the same way as 3c-2e molecular orbitals. The orbital diagram clearly shows that oxygen has three unpaired electrons in its valence shell, which accounts for the paramagnetism and high electronegativity.