Part 1: Atomic Structure & Quantum Mechanics
Lectures 1–8
This part introduces the quantum mechanical foundations of chemistry. Beginning with early atomic models and the Bohr model of hydrogen, we develop the quantum mechanical description of atoms — quantum numbers, electron orbitals, electron configuration, and the periodic trends that emerge from electronic structure.
Part Overview
The properties of materials are ultimately determined by the behavior of electrons in atoms. Understanding atomic structure requires quantum mechanics: the wave-particle duality of matter, quantized energy levels, and the probabilistic nature of electron position. This part builds from the Bohr model to the full quantum mechanical treatment of the hydrogen atom and multi-electron atoms.
Key Topics
- • Bohr model: quantized orbits and energy levels
- • Hydrogen emission spectrum and spectral series
- • Wave-particle duality and de Broglie wavelength
- • Photoelectric effect and photon energy
- • Quantum numbers (n, l, m_l, m_s) and orbital shapes
- • Aufbau principle, Hund's rule, Pauli exclusion principle
- • Electron configuration and periodic trends
- • Photoelectron spectroscopy (PES)
- • Ionization energies across the periodic table
2 topic pages | 8 lectures | Interactive simulations
Key Equations
Bohr Energy Levels
$$E_n = -\frac{13.6 \text{ eV}}{n^2}$$
Rydberg Formula
$$\frac{1}{\lambda} = R_H\left(\frac{1}{n_1^2} - \frac{1}{n_2^2}\right)$$
de Broglie Wavelength
$$\lambda = \frac{h}{mv}$$
Photoelectric Effect
$$E_k = h\nu - \phi$$
Topics
Atomic Structure & Models
The Bohr model, hydrogen spectrum, de Broglie wavelength, photoelectric effect, and the foundations of quantum mechanics applied to atomic structure. Covers Lectures 1–4.
Quantum Numbers & Electron Configuration
The four quantum numbers, Schrodinger equation solutions for hydrogen, electron configuration rules, photoelectron spectroscopy, and ionization energies. Covers Lectures 5–8.