7.3 Electron Configuration | High School Chemistry

Chad begins this lesson with an introduction to the s, p, and d atomic orbitals before diving into the rules for determining ground state electron configurations: the Aufbau principle, Hund's rule, and the Pauli exclusion principle. He then goes on to explain how the periodic table itself can be divided into 'blocks' and used as a tool to aid in assigning electron configurations. Chad then presents several examples of both standard electron configurations as well as abbreviated noble gas configurations along with notable exceptions (Cr, Mo, Cu, Ag, Au). He also shows how electrons are added for anions and removed for cations in determining electron configurations and how electrons are removed from the s subshell before the d subshell in the valence shell for transition metal cations. Chad then concludes the less by comparing and contrasting ground state electron configurations with the excited state. If you want all my study guides, quizzes, and practice exams, check out my premium course at https://www.chadsprep.com/high-school... 00:00 Lesson Introduction 00:41 Atomic Orbitals (s, p, and d Orbitals) 04:37 Shells and Subshells of Orbitals 06:16 Aufbau Principle 11:24 Hund's Rule 13:29 Electron Configurations from the Periodic Table 22:08 Noble Gas Configurations 24:34 Electron Configuration Exceptions (Cr, Mo, Cu, Ag, Au) 29:25 Electron Configuration for Cations and Anions 33:41 How to Count the Number of Valence Electrons 37:52 Ground State vs Excited State https://www.chadsprep.com/