Back to the atomic emmission spectrum and the atomic theory.
in the 1900s, scientists observed that when a gaseous element, such as hydrogen was subjected to an electric discarge that the atoms emitted electromagnetic radiation. The light emmitted could be separated into component frequencies which forms a continuous spectrum. The atoms emit only certain wavelenghs. Each atom has its own atomic energy spectrum.
In 1913, Bohr proposed that electrons revolve around the nucleus in fixed path. These energylevels are called the principal quantum number. Bohr's study with hydrogen matched the calculated wavelengths with the wavelengths of the specified lines.
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Yes, that explanation provides some key points about the atomic emission spectrum and the atomic theory. However, I can expand on it further to provide a more thorough explanation.
The atomic emission spectrum refers to the unique pattern of electromagnetic radiation (light) emitted by an atom when its electrons transition from higher energy levels to lower energy levels. This phenomenon was observed by scientists in the 1900s when they subjected gaseous elements, such as hydrogen, to an electric discharge.
When atoms emit light, the emitted radiation can be separated into different component frequencies, which form a spectrum. In the case of a continuous spectrum, all frequencies of light are present, blending into each other without any distinct lines. However, in the case of atomic emission spectra, only certain wavelengths or frequencies of light are emitted. This results in a discontinuous spectrum consisting of distinct lines.
Each atom has its own unique set of energy levels or orbitals, and these energy levels are responsible for producing specific wavelengths of light. When an atom is excited (for example, by applying an electric discharge), its electrons move from lower energy levels to higher energy levels. However, these excited electrons are unstable and tend to move back to their original energy levels. As they do so, they release energy in the form of photons (particles of light), which corresponds to specific wavelengths or frequencies.
In 1913, the Danish physicist Niels Bohr proposed a model for the atom that explained the observed atomic emission spectra. Bohr suggested that electrons revolve around the nucleus of an atom in fixed paths or orbits, also referred to as energy levels or shells. These energy levels are sometimes represented by the principal quantum number.
According to Bohr's model, electrons can only exist in certain discrete energy states corresponding to these energy levels. When excited, electrons move to higher energy levels, and when they return to their original energy levels, they release photons with energies corresponding to the energy difference between the levels. This energy difference determines the wavelength or frequency of the emitted light.
Bohr's model successfully explained the observed atomic emission spectra, particularly for hydrogen. The wavelengths of the emitted lines in the hydrogen spectrum matched the calculated wavelengths based on the energy differences between Bohr's energy levels. This agreement between theory and observation provided strong evidence for the existence of discrete energy levels in atoms and laid the foundation for further development of atomic theory.
In summary, the atomic emission spectrum is the pattern of light emitted by atoms as their electrons transition between energy levels. Each atom has its own unique set of energy levels, which correspond to specific wavelengths or frequencies of light. Niels Bohr's model of the atom in 1913 proposed that electrons revolve around the nucleus in fixed paths or energy levels, and these energy levels explain the observed patterns in the atomic emission spectrum.