Question

How did bohr use the atomic line spectrum of hydrogen to explain his model of atom.

Answer 1

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 thus emit certain wavelengths used to determine the chemical composition of a gas, star, etc

Complete step-by-step answer:
Bohr explain 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.

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. We see these photons which appear as lines of coloured light, for example Balmer Series, in emission or dark lines in absorption. The Bohr model is originally an atom consisting of a small positively charged nucleus with negatively charged electrons in orbit.

The main points of the model are that:
-Electrons revolve the nucleus in orbits that contain a set size and energy.
-The energy of the orbit is related to the size of it. The least energy is found in the smallest orbit.
-Radiation is emitted or absorbed when an electron jumps from one orbit to another.

Note: 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 . But not so.