Describe the common features which can be explained by the theoretical model of Bohr? Briefly write the limitation of this model
Answers
Answered by
10
Limitations of Bohr’s Model of Atom
Unable to explain the spectrum of multi-electron atoms (For example − helium atom which contains two electrons)
Unable to explain splitting of spectral lines in electric field (Stark effect) or in magnetic field (Zeeman effect)
Fails to explain finer details (doublet − two closely spaced lines) of hydrogen atom spectrum
Fails to explain the ability of atoms to form molecules by chemical bonds
Planck’s Quantum Theory of Radiation / quantizations of energy
Main features of Planck’s quantum theory of radiation are as follows:
Radiant energy is not emitted or absorbed in continuous manner, but discontinuously in the form of small packets of energy called quanta.
Each quantum of energy is associated with definite amount of energy.
The amount of energy (E) associated with quantum of radiation is directly proportional to frequency of light (ν).
i.e., E ∝ ν
Or, E = hν
‘h’ is known as Planck’s constant and has the value 6.626 × 10−34 Js
Postulates for Bohr’s model for hydrogen Atom
The electron in the hydrogen atom moves around the nucleus in a circular path of fixed radius and energy. These circular paths are called orbits, stationary states, or allowed energy states.
Energy is absorbed when electron jumps from lower orbit to a higher orbit and is emitted when electron jumps from higher orbit to a lower orbit.
Frequency (ν) of absorbed or emitted radiation is given by,
(Bohr’s frequency rule)
Where, E1 and E2 are the energies of lower and higher allowed energy states respectively
V=∆E/h
Angular momentum (L) of an electron in a stationary state is given by,
MVR=NH/2π n=1,2,3....
Hope this answer helps u and pls mark it as brainliest answer
Unable to explain the spectrum of multi-electron atoms (For example − helium atom which contains two electrons)
Unable to explain splitting of spectral lines in electric field (Stark effect) or in magnetic field (Zeeman effect)
Fails to explain finer details (doublet − two closely spaced lines) of hydrogen atom spectrum
Fails to explain the ability of atoms to form molecules by chemical bonds
Planck’s Quantum Theory of Radiation / quantizations of energy
Main features of Planck’s quantum theory of radiation are as follows:
Radiant energy is not emitted or absorbed in continuous manner, but discontinuously in the form of small packets of energy called quanta.
Each quantum of energy is associated with definite amount of energy.
The amount of energy (E) associated with quantum of radiation is directly proportional to frequency of light (ν).
i.e., E ∝ ν
Or, E = hν
‘h’ is known as Planck’s constant and has the value 6.626 × 10−34 Js
Postulates for Bohr’s model for hydrogen Atom
The electron in the hydrogen atom moves around the nucleus in a circular path of fixed radius and energy. These circular paths are called orbits, stationary states, or allowed energy states.
Energy is absorbed when electron jumps from lower orbit to a higher orbit and is emitted when electron jumps from higher orbit to a lower orbit.
Frequency (ν) of absorbed or emitted radiation is given by,
(Bohr’s frequency rule)
Where, E1 and E2 are the energies of lower and higher allowed energy states respectively
V=∆E/h
Angular momentum (L) of an electron in a stationary state is given by,
MVR=NH/2π n=1,2,3....
Hope this answer helps u and pls mark it as brainliest answer
Similar questions