Chemistry, asked by nbais4529, 1 year ago

Limitations of baher theory

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Answered by Gouthami03
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▪ 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 Plank’s equation.
ΔE = E2-E1 = hv
▪ 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, but 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.

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