Niels Bohr Atomic Model And Limitations

Thomsonβs atomic model and Rutherfordβs atomic model failed to answer any questions related to the energy of an atom and its stability.

Bohr’s Theory – Bohrβs Atomic Model

In the year 1913, Niels Bohr proposed an atomic structure model, describing an atomΒ as a small, positively charged nucleusΒ surrounded by electronsΒ that travel in circular orbits around the positively charged nucleus like planets around the sun in our solar system, with attraction provided by electrostatic forces, popularly known as Bohrβs atomic model. It was basically an improved version of Rutherford’s atomic modelΒ overcoming its limitations. On most of the points, he is in agreement with him, like concepts of nucleus and electrons orbiting it. Salient features of Niels Bohr atomic model are:

• Electrons revolve around the nucleus in stable orbits without emission of radiant energy. Each orbit has a definite energy and is called an energy shell or energy level.
• An orbit or energy level is designated as K, L, M, N shells. When the electron is in the lowest energy level, it is said to be in the ground state.
• An electron emits or absorbs energy when it jumps from one orbit or energy level to another. When it jumps from a higher energy level to lower energy level it emits energy while it absorbs energy when it jumps from a lower energy level to a higher energy level.
• The energy absorbed or emitted is equal to the difference between the energies of the two energy levels (E1, E2) and is determined by Plankβs equation.

ΞE = E2-E1 = hπ

Where,

ΞE = energy absorbed or emitted
h= Plankβs constant
π= frequency of electromagnetic radiation emitted or absorbed

• The angular momentum of an electron revolving in energy shells is given by:

mevrΒ =Β nh/2Ο

Where,
n= number of corresponding energy shell; 1, 2, 3 β¦..
me= mass of the electron
v= velocity
h= Plankβs constant

Limitations of Bohr Atomic Model Theory

• It violates the Heisenberg Uncertainty Principle. The Bohr atomic model theory considers electrons to have both a known radius and orbit i.e. known position and momentum at the same time, which is impossible according to Heisenberg.
• The Bohr atomic model theory made correct predictions for smaller sized atoms like hydrogen, butΒ poor spectral predictions are obtained when larger atoms are considered.
• It failed to explain the Zeeman effect when the spectral line is split into several components in the presence of a magnetic field.
• It failed to explain the Stark effect when the spectral line gets split up into fine lines in the presence of an electric field.

Q1

What is the limitation of Bohr Atomic Model Theory?

Bohr Atomic Model Theory fails to explain the effect of magnetic field on the spectra of atoms. It also failed to explain the Stark effect and Heisenberg Uncertainty Principle.

Q2

What is the significance of Bohr Atomic Model Theory?

Bohr was the foremost to find that electrons move around the nucleus in different orbits and we can determine an elementβs properties by the number of electrons in the valence shell.

Q3

How do electrons move in Bohrβs model?

According to Bohr, electrons move around the central nucleus in a fixed circular orbit. These orbits of specific energies and are also referred to as energy shells or energy levels.

Q4

Who was the first scientist to discover electrons?

J. J. Thomson was the first to discover electrons while studying the properties of the cathode ray.

Q5

How many electrons are present in the L shell?

There are 8 electrons in the L shell.

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