Question

write the postulates of Bohr's theory of hydrogen atom​

Answer 1

$\huge{\mathfrak{\pink{answer}}}$

Postulate I

In a radical departure from the established principles of classical mechanics and electromagnetism, Bohr postulated that in an atom, electron/s could revolve in stable orbits without emitting radiant energy. Further, he stated that each atom can exist in certain stable states. Also, each state has a definite total energy. These are stationary states of the atom.

Postulate II

Bohr defined these stable orbits in his second postulate. According to this postulate:

An electron revolves around the nucleus in orbits

The angular momentum of revolution is an integral multiple of h/2p – where hàPlanck’s constant [h = 6.6 x 10-34 J-s].

Hence, the angular momentum (L) of the orbiting electron is: L = nh/2p

Postulate III

In this postulate, Bohr incorporated early quantum concepts into the atomic theory. According to this postulate, an electron can transition from a non-radiating orbit to another of a lower energy level. In doing so, a photon is emitted whose energy is equal to the energy difference between the two states. Hence, the frequency of the emitted photon is:

hv = Ei – Ef

(Ei is the energy of the initial state and Ef is the energy of the final state. Also, Ei > Ef).

Answer 2

Explanation:

Postulate I

In a radical departure from the established principles of classical mechanics and electromagnetism, Bohr postulated that in an atom, electron/s could revolve in stable orbits without emitting radiant energy. Further, he stated that each atom can exist in certain stable states. Also, each state has a definite total energy. These are stationary states of the atom.

Postulate II

Bohr defined these stable orbits in his second postulate. According to this postulate:

An electron revolves around the nucleus in orbits

The angular momentum of revolution is an integral multiple of h/2p – where hàPlanck’s constant [h = 6.6 x 10-34 J-s].

Hence, the angular momentum (L) of the orbiting electron is: L = nh/2p

Postulate III

In this postulate, Bohr incorporated early quantum concepts into the atomic theory. According to this postulate, an electron can transition from a non-radiating orbit to another of a lower energy level. In doing so, a photon is emitted whose energy is equal to the energy difference between the two states. Hence, the frequency of the emitted photon is:

hv = Ei – Ef

(Ei is the energy of the initial state and Ef is the energy of the final state. Also, Ei > Ef).