Question

How does the Bohr model of the atom explain the fixed color lines seen in atomic spectra?

Answer 1

Hint: We know that a light spectrum is spectrum that consists of narrow, dark, parallel lines on a background of bright colour, formed from a hot light source surrounded by cooler gases which absorb and when the electron shifts from one allowed orbit to another it absorbs or releases photons of energy which match exactly the separation between the energies of the given orbits.

Complete answer:
Bohr explains to us that the electrons in the Hydrogen atom only occupy distinct orbits around the nucleus (not at any distance from it but at certain specific quantized positions or specific radius each one corresponding to an energetic state of your H atom) where energy is not radiated by them.
Recall Bohr’s atomic model theory. The Bohr Model of the Atom In $$1911$$ at the age of twenty five, Niels Bohr received his hydrogen ion concentration PHD in physics. He was convinced that the atom can be pictured as a tiny low positive nucleus with electrons orbiting around it. The electrons revolve quickly round the nucleus in mounted circular ways known as energy levels or shells. Once associate degree lepton jumps from a lower energy to a better one, some energy is absorbed whereas some energy is emitted. The energy amendment is given by delta $$E={\displaystyle \frac{hc}{wavelength}}.$$
The Bohr model of the atom, at first, looked as if it would be a decent theory, and, indeed, it absolutely was an associate degree advance over what had gone before. However as scientists learned a lot regarding the atom its flaws became evident, and it absolutely was seen to be incorrect, eventually to be outdated by scientific theory.

Note:
Remember that Niels Bohr changed the atomic theory by considering that the electrons did not jump and crash into the nucleus as would be assumed in classical physics. Classical physics states that opposites attract and like repel, so positive nuclei should attract negative electrons.