CHEM 001 Lecture Notes - Lecture 14: Electron Configuration, Pauli Exclusion Principle

• School: College of The Sequoias
• Department: Chemistry (CHEM)
• Course: CHEM 001
• Professor: guerra

Document Summary

Ground state - all electrons are in the lowest energy orbitals possible. Electron configuration - a notation for distribution of electrons into the orbitals of a ground state atom. The number is n; the letter is l; the superscript is the number of electrons in that sublevel. Orbital diagram - electrons drawn as arrows, orbitals as boxes. Same information as electron configuration plus electron spin. An orbital can hold 0, 1, or 2 electrons. If it holds 2, the spins must be opposed. Aufbau principle - lower energy levels are filled before higher energy levels. Chromium and copper are exceptions to the aufbau principle. Don"t worry about writing electron configurations for lanthanides and actinides - there are too many exceptions. There is a 4th quantum number called the electron spin quantum number (ms) Ms has two values: + and - (or up and down) These values represent an electron"s two spin states.