1. Excitation:
* When sodium atoms are heated or exposed to a high-energy source like a flame or an electric discharge, their electrons gain energy.
* These electrons jump from their ground state (lowest energy level) to higher energy levels, becoming *excited*.
2. Relaxation:
* Excited electrons are unstable and quickly fall back down to their ground state.
* As they transition back down, they release the excess energy they absorbed in the form of light.
3. Specific Wavelengths:
* Because the energy levels in an atom are quantized (meaning they can only exist at specific, discrete energy levels), the energy released during these transitions is also quantized.
* This means that sodium atoms emit light at specific, discrete wavelengths, creating the characteristic bright lines in the emission spectrum.
In summary:
The bright line emission spectrum of sodium is produced when its electrons are excited to higher energy levels and then release specific amounts of energy as they fall back down to their ground state, emitting light at specific wavelengths.
