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Rothiemurchus
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Are integers such as n=1,2,3 etc in Bohr's atomic theory, exactly whole numbers or just very close to being whole numbers?
jtbell said:They are intended to be exact integers.
Please note, however, that Bohr's model with electrons moving in classical circular orbits, and Sommerfeld's version with elliptical orbits, are incorrect and obsolete. They were supplanted by the quantum-mechanical model using the [itex]\Psi[/itex] function, developed by Schrödinger and others in the 1920s. You should consider the Bohr-Sommerfeld model as being of historical interest only.
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Integers play a crucial role in Bohr's atomic theory as they represent the different energy levels of an atom. Each energy level is assigned a unique integer value, with the lowest energy level being assigned the integer 1.
In Bohr's atomic theory, the stability of an atom is determined by the number of electrons in each energy level. The maximum number of electrons that can occupy a particular energy level is given by the corresponding integer value. This ensures that the electrons are arranged in a stable configuration.
The integer 2 in Bohr's atomic theory represents the maximum number of electrons that can occupy the first energy level, also known as the K shell. This is the lowest energy level and is closest to the nucleus, making it the most stable energy level.
According to Bohr's atomic theory, an electron can only exist in certain energy levels around the nucleus. When an electron jumps from a higher energy level to a lower one, it emits a specific amount of energy in the form of light. This energy corresponds to a specific wavelength, resulting in the unique atomic spectra. The integers represent the different energy levels that the electron can occupy.
Yes, the concept of integers in Bohr's atomic theory can be applied to all elements in the periodic table. The number of electrons in each energy level varies for different elements, but the concept of assigning unique integer values to represent the energy levels remains the same.