Editing Openai/676d4bd2-a748-800d-9b9c-e8c54c96b975 (section)

===== 1. Quantized Orbits: - Electrons revolve around the nucleus in specific, discrete orbits called "energy levels" or "shells." - These orbits correspond to fixed energy states and are represented by integer quantum numbers (n = 1, 2, 3, ...). =====
# Energy Transitions: - Electrons can move between these quantized orbits by absorbing or emitting energy in the form of photons. - The energy difference between two levels determines the frequency of the emitted or absorbed radiation: E=hνE = h \nuE=hν Where EEE is the energy difference, hhh is Planck's constant, and ν\nuν is the frequency of light.
# Centripetal Force: - The force that keeps electrons in their orbits is provided by the electrostatic attraction between the negatively charged electrons and the positively charged nucleus.
# Angular Momentum Quantization: - Bohr introduced the concept that the angular momentum of an electron is quantized and given by: L=nℏ=nh2πL = n\hbar = n\frac{h}{2\pi}L=nℏ=n2πh Where nnn is the principal quantum number, hhh is Planck's constant, and ℏ\hbarℏ is the reduced Planck's constant.
# Hydrogen Atom Focus: - The Bohr Model primarily applies to the hydrogen atom, where it successfully explains the observed spectral lines in its emission spectrum (e.g., the Balmer series).