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what are the limitations found in Bohr's Theory ????
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Answered by
1
♠ ANSWER :
⏺️BOHR'S ATOMIC THEORY LIMITATIONS
❇ BOHR'S atomic theory was quite successful in explaining the stability of atom and the line spectrum of hydrogen atom. However, several discrepancies were observed in this model.
Some of the limitations of BOHR'S model are:
➊ BOHR'S model of an atom could not account for the finer details ( DOUBLET , two closely spaced lines ) of the hydrogen spectrum observed using sophisticated spectroscopic techniques.
➋ BOHR'S model of an atom could not explain the LINE SPECTRA of atoms containing more than one electron called MULTI ELECTRON atoms.
➌ BOHR'S theory failed to account for the effect of MAGNETIC FIELD on the spectra of atoms or ions. It was observed that when the atom emitting radiations is placed in a strong magnetic field, each spectral line is further split into a number of lines. This phenomenon is known as ZEEMAN'S EFFECT.
➍ BOHR'S theory also could not explain the effect of electric field ( known as STARK EFFECT) on the spectra of atoms.
➎ BOHR'S theory does not provide any clue to explain the shapes of molecules arising out of the directional bonding between atoms.
⏺️BOHR'S ATOMIC THEORY LIMITATIONS
❇ BOHR'S atomic theory was quite successful in explaining the stability of atom and the line spectrum of hydrogen atom. However, several discrepancies were observed in this model.
Some of the limitations of BOHR'S model are:
➊ BOHR'S model of an atom could not account for the finer details ( DOUBLET , two closely spaced lines ) of the hydrogen spectrum observed using sophisticated spectroscopic techniques.
➋ BOHR'S model of an atom could not explain the LINE SPECTRA of atoms containing more than one electron called MULTI ELECTRON atoms.
➌ BOHR'S theory failed to account for the effect of MAGNETIC FIELD on the spectra of atoms or ions. It was observed that when the atom emitting radiations is placed in a strong magnetic field, each spectral line is further split into a number of lines. This phenomenon is known as ZEEMAN'S EFFECT.
➍ BOHR'S theory also could not explain the effect of electric field ( known as STARK EFFECT) on the spectra of atoms.
➎ BOHR'S theory does not provide any clue to explain the shapes of molecules arising out of the directional bonding between atoms.
Answered by
2
Hey friend here is ur query..
==========>>>>>>
Bohr’s theory was able to explain successfully a number of experimental observed facts and
has correctly predicted the spectral lines of neutral hydrogen atom and singly ionized helium
atom, etc. in terms of only principal quantum number n. However, the theory fails to explain
the following facts.
(i)
The theory could not account the spectra of atoms more complex than hydrogen.
(ii) The theory does not give any information regarding the distribution and arrangement of
electrons in atom.
(iii) It does not explain the experimentally observed variations in intensity of the spectral lines of
an element.
(iv) This theory cannot be used to calculate about transitions from one level to another such as the
rate at which they occur or the selection rules which apply to them.
(v)
This theory fails for accounting the fine structure of spectral line. Actually it was found that
when spectral lines emitted by an atom are examined, each line is composed of several lines
closely packed together. Bohr’s theory does not throw any light on it.
(vi) This theory cannot be used for the quantitative explanation of chemical bonding.
(vii) The theory fails to give correct result when an electric or magnetic field is applied to the atom.
<<<<======
Hope this will help you
==========>>>>>>
Bohr’s theory was able to explain successfully a number of experimental observed facts and
has correctly predicted the spectral lines of neutral hydrogen atom and singly ionized helium
atom, etc. in terms of only principal quantum number n. However, the theory fails to explain
the following facts.
(i)
The theory could not account the spectra of atoms more complex than hydrogen.
(ii) The theory does not give any information regarding the distribution and arrangement of
electrons in atom.
(iii) It does not explain the experimentally observed variations in intensity of the spectral lines of
an element.
(iv) This theory cannot be used to calculate about transitions from one level to another such as the
rate at which they occur or the selection rules which apply to them.
(v)
This theory fails for accounting the fine structure of spectral line. Actually it was found that
when spectral lines emitted by an atom are examined, each line is composed of several lines
closely packed together. Bohr’s theory does not throw any light on it.
(vi) This theory cannot be used for the quantitative explanation of chemical bonding.
(vii) The theory fails to give correct result when an electric or magnetic field is applied to the atom.
<<<<======
Hope this will help you
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