What type of spectrum occurs when an electron moves from high to low energy?

When an electron transitions from a higher energy level to a lower energy level, it emits energy in the form of light. This process is what creates an emission spectrum. The emitted light corresponds to specific wavelengths, which are characteristic of the element involved, allowing us to observe discrete lines in the spectrum.

The emission spectrum results from these transitions where the energy lost by the electron as it drops to a lower state is released in the form of photons of light. Each line in the emission spectrum correlates with a specific change in energy levels within the atom, making these spectra unique to each element.

In contrast, an absorption spectrum occurs when electrons absorb energy to move from a lower energy level to a higher one, resulting in dark lines or bands where specific wavelengths of light are absorbed. Reflection and transmission spectra involve different processes and do not specifically relate to the transitions of electrons between energy levels in the same way that emission and absorption spectra do. Thus, the movement of an electron from high to low energy directly correlates with the formation of an emission spectrum.