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Energy levels are the fixed ranges between which electrons can orbit. We have different orbits in which electrons revolve. By combining the energy quanta of Planck’s concept with Rutherford’s model of atoms of electrons orbiting the nucleus, Bohr arrived at his model.By combining energy quanta of Planck’s concept with Rutherford’s model of atom of electrons orbiting the nucleus, Bohr got at his model.An electron would receive energy in the form of photons to be driven to a higher energy state, as per Bohr’s model, as provided as the photon’s intensity was equal to the energy difference between both the original and final energy state.
Bohr’s Model
The atom progressed from the indivisible spheres’ theory of Dalton to the plum pudding model of JJ Thomson to the atom theory of Rutherford. In addition to carrying out the spectacular investigation that revealed the presence of the atomic nucleus, Rutherford postulated that the electrons encircled the nucleus in a planetary movement. Scientists were drawn to the solar system or planetary model of the atom because it was related to something that they were previously familiar with – the solar system.
However, the planetary model had a severe weakness. It was previously understood that as a charged particle (such as an electron) moves in a curved route, it emits light and loses energy. After all, this is how we make TV signals. If an electron orbiting an atom’s nucleus loses energy, it will have to travel a little closer to the nucleus as it loses energy, finally colliding with the nucleus. However, Rutherford’s model was unable to explain how electrons emit light, resulting in the distinct atomic spectra of each element. These concerns threw a cloud over the idea of a planet, implying that it will have to be changed at some point.
In 1913, Niels Bohr, a Danish physicist, suggested the concept of an atom’s electron cloud, in which electrons orbit around the nucleus and form atomic spectra. Knowing Bohr’s model necessitates familiarity with electromagnetic radiation.
Stationary States Or Energy Levels
In his concept of the atom, Bohr’s main notion was that electrons occupy certain orbitals that require the electron to have a certain amount of energy. An electron must be from one of the permitted orbitals and have the appropriate energy required for that orbit to be in the electron-dense cloud of an atom. An electron would need less energy to orbit closer to the nucleus, while an electron would need more energy to orbit farther from the nucleus.
Energy levels or stationary states refer to all of the potential orbits. We have different orbits in which electrons revolve around the orbits. One of Bohr’s models’ flaws was that he couldn’t explain why just particular energy levels or orbits were permitted. As per Bohr, electrons could only lose or gain energy by shifting from one energy level to another, acquiring or dropping precise quantities of energy. Quantized energy levels indicate that only particular amounts are possible.
It’d be like a stairwell, with only rungs at specific heights. The only way to get on the ladder would be to stand on one of the rungs and the only way to move up the ladder would be to switch to another rung. Assume we have a ladder with ten rungs. In the regular state, only one person can be on each level and the ladder occupants must be on the lowest rung accessible. They would be on the bottom five rungs of the ladder if there were five persons on it. No one could move down in this case because all of the lower rungs are occupied. In his model, Bohr devised restrictions for the most number of electrons that could be in each energy level, requiring that an atom in its normal state (ground state) has all electrons in the least energy state. We have different orbits in which electrons revolve. No electron can decrease energy under these conditions because no electron can reach the least energy level. Bohr’s concept explained why electrons surrounding the nucleus did not emit energy and spiralled back into the nucleus in this fashion.
Bohr’s Model And Atomic Spectra
The atomic spectra provided evidence to back up Bohr’s theory. He proposed that the electrons in an atom move through energy levels to create an atomic spectrum. The ground state is the least energy state in which electrons can exist. The electrons in an atom can absorb energy by moving to a higher energy level or excited state, if they are supplied with energy (via heat, electricity, light or other means). We have different orbits in which electrons revolve. The electrons then release the energy they have received in the form of a photon, allowing them to return to a low energy state. Because the disparities in energy levels are accurate, the energy emitted by electrons falling to lower energy levels is always the precise quantity of energy. When looking at an atomic spectrum, this explains why you see certain lines of light—each line belongs to a particular “step down” that an electron in that atom can take. This also explains why each element’s atomic spectrum is unique. Because each element’s electrons have various allowable energy levels, the electrons of each element can travel different paths than those of other elements.
Conclusion
It can be concluded that according to Bohr’s concept, every atom has a series of unchanging energy levels and electrons in the atom’s electron cloud have to be in one of them. It claims that atoms’ atomic spectra are created by electrons acquiring energy from a source, rising to a higher energy level and then lowering down to a lower energy level and emitting the energy difference between them. The existence of atomic spectra lends credence to Bohr’s atomic hypothesis. Only the hydrogen atom’s energy levels were calculated successfully using Bohr’s model.
