Final answer:
Electrons absorb energy and move to an excited state, then release that energy in the form of electromagnetic radiation, primarily light, when returning to the ground state. This release of energy is observed as the atomic emission spectra, with each element producing a unique spectrum based on these electron transitions.
Step-by-step explanation:
When electrons move to higher energy levels and then go back to the ground state, they experience a process known as excitation and de-excitation. In the ground state, an electron in an atom is at its lowest energy level. Upon absorbing energy from an outside source such as heat, electricity, or light, the electron moves to a higher, quantized energy level, known as an excited state. However, this state is unstable, and the electron will eventually return to the ground state by releasing energy in the form of electromagnetic radiation, typically as visible light or ultraviolet photons. This emission of light energy is what creates the atomic emission spectra unique to each element, as each transition corresponds to a specific photon energy and wavelength.
In summary, the process that occurs when an electron jumps to a higher energy level and then falls back to the ground state involves energy absorption followed by the emission of energy that had been absorbed. The law of conservation of energy indicates that the energy released is precisely equal to the energy initially absorbed. This principle is well demonstrated in the example of fireworks, where the absorbed energy is visibly released as vibrant colors of light when the electrons return to their original energy levels.