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10 videos · 4 h 50 min
Lecture · MIT
MIT OpenCourseWare · Jeffrey C. Grossman
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.
Lecture · MIT
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.
Lecture · MIT
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.
Course · MIT
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.
Course · MIT
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.
Explainer · YouTube
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.
Lecture · YouTube
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.
Explainer · YouTube
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.
Explainer · YouTube
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.
Explainer · YouTube
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.