Each energy level corresponds to an exact amount of energy needed by the electron to orbit the nucleus. Transitions from a higher energy level to a lower energy level correspond to the difference in the energy needed for an electron to occupy those two energy levels. This difference creates the emission spectrum.
energy states in the hydrogen atom are quantized.
Niels Bohr studied the emission lines of Hydrogen.
the bohr model for hydrogen is H
In Bohr's model there are stationary orbits in which though the electrons are subjected to centrifugal acceleration, they will not give out any kind radiation. But in Rutherford's model no such stationary orbits. In case Bohr's model, line spectrum is possible. But in Rutherford's model, continuous spectrum is expected. But no such spectrum emitted by atoms especially hydrogen atom
At the simplest level it was the Bohr model.
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Niels Bohr studied the emission lines of Hydrogen.
Niels Bohr in 1913.
it is produced when an electron from a higher energy orbit drops down to a lower level of energy orbit.
It's produced when an electron from a higher energy orbit drops down to a lower level energy orbit
For a detailed explanation on the relation between spectrum lines electron energy check out avogadro.co.uk/light/bohr/spectra.htm
The formula parallel to Rydberg's formula used in Bohr's theory of the emission spectrum of the hydrogen atom is the Balmer Series. See related link for more information.
Bohr
he failed to explain line spectrum of elements except hydrogen.
Bohr.
nies bohr created the theory of the atom. that all atom revolves around dog nucleus
Niels Bohr had the first theoretical explanation. It was based on his very early quantum mechanics - that has now been completely scrapped.
Bohr based his atomic model on the element hydrogen. He applied his model to the hydrogen atom and found that it provided an explanation for its line spectrum.