⚛️ Bohr Atomic Model Simulator - Electron Transitions
Atomic StructureWhat's happening? ΔE = 13.6(1/n₂² - 1/n₁²). Electron jumps down = photon emitted. Jumps up = photon absorbed. The photon color depends on energy difference.
Bohr model tested every year for hydrogen spectrum.
JEE asks energy transitions, spectral series, ionization energy. Key: dE = 13.6(1/n1^2 - 1/n2^2) eV.
Key formulas
Bohr Atomic Model Formulas
Energy levels
E_n = -13.6 x Z^2/n^2 eV
For H: E_n = -13.6/n^2. H-like: x Z^2
Rydberg
1/lambda = R(1/n1^2 - 1/n2^2)
R = 1.097x10^7 m^-1
Radius
r_n = n^2/Z x 0.529 A
Bohr radius a_0 = 0.529 Angstrom
Ionization
IE = 13.6 x Z^2 eV
Energy to remove electron from n=1
Step-by-step problem solving
How to solve chemistry problems in JEE
- Identify n1, n2
- Use dE = 13.6(1/n1^2 - 1/n2^2)
- For wavelength: 1/lambda = R(...) or lambda = hc/dE
- n2>n1 = emission, n2
Common JEE mistakes
What students get wrong
Emission vs absorption
Drop down = emission. Jump up = absorption.
Wrong Z
H: Z=1, He+: Z=2, Li2+: Z=3. Square it!
n1 vs n2
n1 = lower, n2 = higher. Balmer: n1=2
Units
Energy in eV, wavelength in nm
FAQs
Bohr Atomic Model Questions
Balmer series?
Transitions ending at n=2. Visible light.
Spectral series?
n1=1: Lyman(UV), n1=2: Balmer(visible), n1=3: Paschen(IR)
Multi-electron atoms?
Bohr only works for H and H-like ions.
Negative energy meaning?
Electron is bound. +13.6 eV frees it.