Question

Explain the formation of line spectrum of hydrogen based on Bohr's atomic theory

Answer 1

Answer:

Niels Bohr proposed a theory of atomic structure known as Bohr's atomic model, which depicts an atom as a tiny, positively charged nucleus surrounded by electrons that move in a circular orbit around the positively charged nucleus like planets circle the sun in our solar system.

Explanation:

According to Bohr, the electrons in the hydrogen atom may only occupy distinct orbits around the nucleus that are free of energy radiation.

These orbits must be at definite, quantized positions or radial distances from the nucleus rather than at any distance from it.

The electron emits or absorbs photons with energies that perfectly match the distance between the energies of the allowed orbits when it transitions from one to the other (emission/absorption spectrum).

These photons are visible to us as black lines during absorption or lines of colored light during emission (the Balmer Series, for instance).

Or we can say that,

In an atom, negatively charged electrons travel in fixed circular paths, known as orbits or shells, around the positively charged nucleus. These circular orbits are referred to as orbital shells because each orbit or shell has defined energy.

By making the assumption that the electron traveled in circular orbits and that only orbits with specific radii were permitted, Niels Bohr was able to explain the line spectra of the hydrogen atom.

The most stable ground state of an atom was represented by the orbit that was closest to the nucleus; the orbits that were farther away represented higher-energy excited states.

Hence, the formation of the line spectrum of hydrogen based on Bohr's atomic theory is explained above.

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