ANT100Y1 Lecture Notes - Valence Bond Theory, Valence Electron, Atomic Orbital

• School: UTSG
• Department: Anthropology
• Course: ANT100Y1
• Professor: Doug Thomson

Document Summary

The three different p orbitals within a given shell are oriented in space along mutually perpendicular directions, denoted px, py and pz. Each p orbital is separated by a region of zero electron density called a node. Configurations: the lowest-energy arrangement, or ground-state electron configuration of an atom is a listing of the orbitals occupied by its electrons we predict this arrangement via: Rule 1: lowest energy orbitals fill up first, 1s -> 2s -> 2p -> 3s -> 3p -> 4s ->3d, called the aufbau principle. Rule 2: electrons act as if they spin around an axis; this spin can have two orientations, up or down,( ) and only two electrons can occupy an orbital, of opposite spin, called pauli exclusion principle. Rule 3: if two or more empty orbitals of equal energy are available, electrons occupy spins parallel until all orbitals are half-full, called the hund"s rule.