Simplified Bohr Model & Energy Levels
Visualizing the quantized orbits and energy transitions of an electron.
Understanding the Bohr Model
The Bohr Model explains that electrons in an atom exist only in specific, stable orbits, each with a fixed energy level. Electrons don't radiate energy while in these orbits.
When an electron jumps from one orbit to another, it either absorbs or emits a tiny packet of light called a photon. The energy of this photon is *exactly* equal to the energy difference between the two orbits. This is why atoms produce distinct "line spectra."
What to look for
- The Atomic View shows the electron (blue dot) moving around the nucleus (yellow dot) in an orbit, leaving a small trail.
- The Energy Level Diagram on the right illustrates these allowed energy levels as horizontal lines, including ionization (n=$\infty$).
- Going up to a higher level absorbs a photon (red pulse); falling down emits one (green pulse).
Controls
Current State
The electron is in the ground state (n=1). Excite it to begin.
Energy Level ($n$): 1
Energy ($E_n$): 0 eV
Last Photon Energy ($\Delta E$): 0 eV
Wavelength ($\lambda$): 0 nm
Frequency ($f$): 0 PHz