* This simulation take the spectral data from NATIONAL INSTITUTE OF STANDARDS AND TECHNOLOGY.
When heat is applied to the atoms, some electrons can have high energy levels and fall to the lower levels. Some electrons emit as much energy as the energy level difference. By measuring the emitted light, we can detect the atoms.
The metal atoms mainly emit visible light. Metal-containing ionic material with gunpowder creates a fantastic fireworks display.
Incandescent bulbs emit light in all visible wavelengths by thermoelectrons. The spectrum’s continuous view is not only because a specific value of energy is emitted but because energy is evenly emitted over the entire visible range.
The continuous spectrum is well observed in a dense state because the atom’s electron orbits interfered with each other and thus did not emit their own light. (E.g., solid or liquid, dense gas)
When looking at the spectrum of light emitted from a fluorescent lamp, sodium lamp, neon sign, or flame test, only distinct wavelengths of light appear. The observed spectrum looks like a bar code.
Line spectra are well observed in lean conditions because the atoms must emit their own light without interfering with each other. (E.g., gas or plasma state)
[…] OPTION 3: VIRTUAL LAB: If you don’t have access to the necessary chemicals, there is a virtual experiment students can do instead. No safety hazards or clean up! (This is also great for lab make-ups when students are absent). I love that it shows the electrons and orbitals for each atom as they go. You can check out the virtual lab here. […]