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Absorption
For an atom to emit light, the electrons of the atom must become excited and move to a higher energy level. To do this, the electron must absorb energy. Energy sources that can trigger an electron to move to a higher energy level include electricity, heat and light energy. When light energy is used to excite electrons, only certain frequencies are absorbed by the electrons as they move into higher energy states. Each electron present in the atom has many energy levels the electron may move to as it becomes more excited.
Emission
The excited states of the electron do not last forever. The electron will move back toward its natural energy state eventually. To be able to accomplish this, the electron must release energy. The energy released from the electron comes in the form of light. The frequency of the light emitted from the electron is the same as the frequency of light absorbed by the atom as it became excited.
Atomic Spectrum
Each element of the Periodic Table has a different amount of protons, neutrons and electrons that make up the atom. Because of these differences in atomic makeup, each element absorbs and emits different frequencies of light as the electrons are excited or move back down to lower energy levels. When atoms are observed through a spectroscope, the result is that each atom has a specific pattern of frequencies of light creating an atomic spectrum. The atomic spectrum is one way in which elements can be identified.
How the Atomic Spectrum Is Used
The atomic spectrum is a useful tool to study far off places. Scientists use the atomic spectrum to determine the elemental composition of stars by examining the color of light that is emitted. In addition, since each element only emits certain colors or frequencies of light, the different elements can be used to produce electric lights. For example, neon lighting utilizes the element neon and other elements in the gas state to produce the bright colored signs seen at many business locations.