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# Atomic Emission Spectra

## Light emitted by an element when electricity is run through it.

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Atomic Emission Spectra

Atomic Emission Spectra

The electrons in an atom tend to be arranged in such a way that the energy of the atom is as low as possible. The ground state of an atom is the lowest energy state of the atom. When those atoms are given energy, the electrons absorb the energy and move to a higher energy level. These energy levels of the electrons in atoms are quantized, meaning again that the electron must move from one energy level to another in discrete steps rather than continuously. An excited state of an atom is a state where its potential energy is higher than the ground state. An atom in the excited state is not stable. When it returns back to the ground state, it releases the energy that it had previously gained in the form of electromagnetic radiation.

So how do atoms gain energy in the first place? One way is to pass an electric current through an enclosed sample of a gas at low pressure. Since the electron energy levels are unique for each element, every gas discharge tube will glow with a distinctive color depending on the identity of the gas (see Figure below).

Credit: User:Jurii/Wikimedia Commons, Heinrich Pniok (Wikimedia: Alchemist-hp)
Source: http://commons.wikimedia.org/wiki/File:Glowing_noble_gases.jpg

Gas discharge tubes are enclosed glass tubes filled with a gas at low pressure through which an electric current is passed. Electrons in the gaseous atoms first become excited, and then fall back to lower energy levels, emitting light of a distinctive color in the process. Shown are gas discharge tubes of helium, neon, argon, krypton, and xenon. [Figure1]

“Neon” signs are familiar examples of gas discharge tubes. However, only signs that glow with the red-orange color seen in the figure are actually filled with neon. Signs of other colors contain different gases or mixtures of gases.

Scientists studied the distinctive pink color of the gas discharge created by hydrogen gas. When a narrow beam of this light was viewed through a prism, the light was separated into four lines of very specific wavelengths (and frequencies since \begin{align*}\lambda\end{align*} and \begin{align*}v\end{align*} are inversely related). An atomic emission spectrum is the pattern of lines formed when light passes through a prism to separate it into the different frequencies of light it contains. The Figure below shows the atomic emission spectrum of hydrogen.

Credit: CK-12 Foundation - Christopher Auyeung, using emission spectra available in the public domain
Source: H spectrum: http://commons.wikimedia.org/wiki/File:Emission_spectrum-H.svg; visible spectrum: http://commons.wikimedia.org/wiki/File:Linear_visible_spectrum.svg; He spectrum: http://commons.wikimedia.org/wiki/File:Helium_Emission_Spectrum.svg; Fe spectrum: http://commons.wikimedia.org/wiki/File:Emission_spectrum-Fe.svg

When light from a hydrogen gas discharge tube is passed through a prism, the light is split into four visible lines. Each of these spectral lines corresponds to a different electron transition from a higher energy state to a lower energy state. Every element has a unique atomic emission spectrum, as shown by the examples of mercury (Hg) and strontium (Sr). [Figure2]

Classical theory was unable to explain the existence of atomic emission spectra, also known as line-emission spectra. According to classical physics, a ground state atom would be able to absorb any amount of energy rather than only discrete amounts. Likewise, when the atoms relaxed back to a lower energy state, any amount of energy could be released. This would result in what is known a continuous spectrum, where all wavelengths and frequencies are represented. White light viewed through a prism and a rainbow are examples of continuous spectra. Atomic emission spectra were more proof of the quantized nature of light and led to a new model of the atom based on quantum theory.

#### Summary

• Atomic emission spectra are produced when excited electrons return to ground state.
• The emitted light corresponds to energies of the specific electrons.

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