Quantum Bohr Model – AP Physics 2

Quantized Energy

$$ E_n = -13.6 \frac{Z^2}{n^2}\text{ eV} $$ $$ E_{photon} = \lvert E_f - E_i \rvert $$ $$ \lambda = \frac{1240 \text{ eV}\cdot\text{nm}}{E_{photon}} $$

Series Emissions

Lyman Series ($n_f = 1$): Ultraviolet Light (Invisible). High energy drops back to ground state.

Balmer Series ($n_f = 2$): Visible Light. Drops to the second orbital.

Paschen Series ($n_f = 3$): Infrared Light (Invisible). Low energy transitions.

Tags

quantumatomhydrogenspectroscopy

Emission Spectrometer (100nm to 1000nm)

Transition Data

Initial State ($n_i$):
Final State ($n_f$):

Energy Change ($\Delta E$):
Photon Wavelength ($\lambda$):

Target Isotope

Trigger Transition

Electron Current State

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Target Final State

When an electron drops to a lower energy level ($n_i > n_f$), it emits a photon. If it jumps to a higher level, it absorbs a photon. Emission lines will be logged in the spectrometer below.