Name: 7. Aufbau Principle and Atomic Orbitals (Intro to Solid-State Chemistry)
Duration: 50 min
Description: A full lecture from Jeffrey Grossman's MIT 3.091, Introduction to Solid-State Chemistry, devoted to the Aufbau principle and atomic orbitals: section 3's building-up procedure at university pace. Whenever orbitals are being filled, predict the next step yourself with the n + l rule first, remembering that 4s comes before 3d.

In the course

Supports Chapter 18

18Unit 4 · Atoms, Spin & IdentityPauli Exclusion & the Periodic Table

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10 videos · 4 h 20 min

Lecture · MIT
L22.4 Identical particles and exchange degeneracy
MIT OpenCourseWare · Barton Zwiebach
A 20-minute MIT 8.06 segment in which Barton Zwiebach introduces identical particles and the exchange degeneracy they create: when particles cannot be told apart, a two-particle state has no unique label. It is rigorous background to section 2's minus-sign callout; later segments of the same course (L23.4 on symmetric and antisymmetric states of N particles, then the symmetrization postulate) resolve the ambiguity, which chapter 19 takes up.
- Ch 18
Lecture · MIT
Lecture 19: Identical Particles
MIT OpenCourseWare · Allan Adams · 2013
The lecture from MIT 8.04 Quantum Physics I (Allan Adams, 2013) that goes with Chapter 18. The whole course is in the Lecture Hall.
- Ch 18
Lecture · MIT
23. Many-Electron Atoms
MIT OpenCourseWare · Robert Field · 2017
The lecture from MIT 5.61 Physical Chemistry (Robert Field, 2017) that goes with Chapter 18. The whole course is in the Lecture Hall.
- Ch 18
Course · MIT
Quantum Physics I
MIT OpenCourseWare · Allan Adams · 2013
Allan Adams' celebrated course starts from superposition and the experimental facts, builds the wavefunction, operators and the Schrödinger equation, then tours scattering, hydrogen, identical particles and band structure before closing on entanglement and Bell's theorem. Calculus and a little linear algebra are enough to keep up.
- Ch 01
- Ch 04
- and 14 more chapters
Course · MIT
Physical Chemistry
MIT OpenCourseWare · Robert Field · 2017
Quantum mechanics as chemists use it, taught by the spectroscopist Robert Field: the photoelectric effect and Compton scattering, boxes and oscillators, hydrogen and many-electron atoms. Strong on spectroscopy, the experimental face of quantization.
- Ch 02
- Ch 04
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Explainer · YouTube
How Quantum Mechanics Predicts All The Elements
Arvin Ash
A clear, animated overview of how the quantum numbers, and the rules for filling the states they label, organise electrons into shells and reproduce the layout of the periodic table. Use it for the big picture; the lesson then works through each rule, and its exceptions, one at a time.
- Ch 18
Lecture · YouTube
Why can't you walk through walls? The Pauli Exclusion Principle Explained
Physics Explained
A long, mathematically honest lecture: it builds two-particle wavefunctions in a box, separates fermions from bosons, derives the exclusion principle, and then calculates the quantum pressure that makes solids resist compression. Ideal after the lesson, when you want the reasoning behind sections 2 and 6.
- Ch 18
Explainer · YouTube
How Electron Spin Makes Matter Possible
PBS Space Time
Matt O'Dowd connects the spin you met in chapter 17 to the fact that all electrons are identical, and shows why that combination keeps you from falling through your chair. A good bridge into next chapter's bosons and fermions.
- Ch 18
Explainer · YouTube
Was Brian Cox wrong? - Sixty Symbols
Sixty Symbols
Brian Cox ruffled feathers with a TV lecture that touched on the Pauli exclusion principle, and two of the channel's scientists weigh in. Use it to test section 1's fine print: 'the same quantum state' means the complete state, spatial wavefunction and spin together, so ask how far the rule really reaches between electrons in different atoms.
- Ch 18
Explainer · YouTube
The Basic Math that Explains Why Atoms are Arranged Like They Are: Pauli Exclusion Principle
Parth G
Parth G sets out the basic mathematics behind why electrons are arranged in shells, with the exclusion principle doing the work: the seat-counting at the heart of section 2. As he counts, check his numbers against 2 × (2l + 1) electrons per subshell and 2n² per shell.
- Ch 18