Atomic Structure and Spectra

📋 Course Outline

1. Bohr's quantization condition
2. Allowed stationary orbits
3. Energy absorption and emission
4. Hydrogen atom model
5. Energy levels and spectra
6. Hydrogen-like atoms
7. Excitation and ionization energies
8. Limitations of Bohr's theory

📖 1. Bohr's quantization condition

🔑 Key Concepts & Definitions

Bohr's quantization condition:
BOHR (1913): The principle that the angular momentum of an electron in an atom is restricted to discrete, quantized values. Specifically, the angular momentum can only take on values that are integer multiples of ħ, where ħ is the reduced Planck constant. This is expressed mathematically as $m v r = n \hbar$, where $m$ is the mass of the electron, $v$ is its velocity, $r$ is the radius of the orbit, and $n$ is a positive integer called the principal quantum number.

Angular momentum quantization:
The concept that the angular momentum of an electron orbiting the nucleus is not continuous but can only have specific, discrete values. These values are integral multiples of $\hbar$, meaning the electron's angular momentum is quantized.