What type of spectrum results from atomic emissions when electrons transition from high to low energy states?

When electrons in an atom transition from a higher energy state to a lower energy state, they release energy in the form of electromagnetic radiation. This radiation corresponds to specific wavelengths, which are unique to the type of atom or molecule emitting it. As a result, the spectrum produced from these transitions consists of distinct lines at particular wavelengths rather than a continuous range of colors.

This distinct appearance is known as a line-emission spectrum. Each line in the spectrum represents a different transition between energy levels, showcasing the quantized nature of electron energy within atoms. Therefore, when we observe the light emitted by an atom, we see a series of sharp lines that indicate the specific energies of the emitted photons. This characteristic makes the line-emission spectrum immensely useful for identifying elements, as each one has a unique line-emission profile based on its electron structure and energy level configurations.