Line Spectrum vs Continuous Spectrum
Interactive Simulation of Atomic Emission Spectra
Line Spectrum
DISCRETE
380nm (UV)
500nm
620nm
740nm (IR)
Element Selection
Excitation Level
Continuous Spectrum
CONTINUOUS
380nm (UV)
500nm
620nm
740nm (IR)
Temperature Control
Filament
Star
Sun
Understanding the Difference
This simulation demonstrates the fundamental difference between line spectra (emitted by excited atoms) and continuous spectra (emitted by hot, dense objects).
| Feature | Line Spectrum | Continuous Spectrum |
|---|---|---|
| Source | Excited, low-density gases (atoms/molecules) | Hot, dense objects (solids, liquids, dense gases) |
| Appearance | Discrete colored lines on dark background | Smooth rainbow of colors without gaps |
| Cause | Electron transitions between specific energy levels | Thermal motion of charged particles (blackbody radiation) |
| Dependence | Depends on atomic structure of the element | Depends only on temperature (Planck’s law) |
| Examples | Neon signs, mercury vapor lamps, auroras | Incandescent bulbs, stars, molten metals |
Key Insight: Line spectra reveal the quantum nature of atoms (discrete energy levels), while continuous spectra demonstrate classical thermal radiation properties. This difference was crucial in the development of quantum mechanics.