Light, energy, and emission spectra
Light travels as waves whose speed equals frequency times wavelength (c = frequency x wavelength), so a higher-frequency light has a shorter wavelength. Light also comes in packets of energy called photons, and a photon's energy is proportional to its frequency (E = hf, where h is Planck's constant), so violet light carries more energy per photon than red light. When atoms absorb energy, such as from heat or electricity, their electrons jump to higher energy levels; when the electrons fall back, they give off photons with only certain specific energies. Each element therefore emits its own pattern of colored lines, its emission spectrum, like a fingerprint. The fact that only certain lines appear is evidence that the energy of electrons in atoms is quantized, limited to specific levels.
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