7.3 Electron Configuration | High School Chemistry

Описание: 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.

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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

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