(C) The number of dark lines in an absorption spectrum is given by $(n - 1)$,where $n$ is the principal quantum number of the highest excited state re

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(C) The number of dark lines in an absorption spectrum is given by $(n - 1)$,where $n$ is the principal quantum number of the highest excited state reached by the atoms.Given that there are $5$ dark lines,we have $n - 1 = 5$,which implies $n = 6$.When these atoms return to the ground state,the number of bright lines in the emission spectrum is given by the formula $\frac{n(n - 1)}{2}$.Substituting $n = 6$ into the formula,we get $\frac{6(6 - 1)}{2} = \frac{6 \times 5}{2} = 15$.Therefore,the number of bright lines in the emission spectrum is $15$.

Class 12 Physics Atoms Electron Energy and Electron Energy Levels in Hydrogen Atom

Medium

In a sample of hydrogen-like atoms,all of which are in the ground state,a photon beam containing photons of various energies is passed. In the absorption spectrum,five dark lines are observed. The number of bright lines in the emission spectrum will be (assume that all transitions take place).

A
$5$
B
$10$
C
$15$
D
None of these

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Electron Energy and Electron Energy Levels in Hydrogen Atom

The diagram shows the energy levels for an electron in a certain atom. Which transition shown represents the emission of a photon with the most energy?

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In a hydrogen atom,the electron makes a transition from the $(n+1)^{\text{th}}$ level to the $n^{\text{th}}$ level. If $n >> 1$,the frequency of the radiation emitted is proportional to:

DifficultJEE MAIN 2020

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Energy of a stationary electron in the hydrogen atom is $E = -\frac{13.6}{n^2} \text{ eV}$. Calculate the energies required to excite the electron in a hydrogen atom to $(a)$ its second excited state and $(b)$ its ionized state,respectively.

MediumAP EAMCET 2022

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$A$ hypothetical atom has only three energy levels. The ground level has energy,$E_1 = -8 \ eV$. The two excited states have energies,$E_2 = -6 \ eV$ and $E_3 = -2 \ eV$. Which of the following wavelengths will $NOT$ be present in the emission spectrum of this atom (in $nm$)?

MediumAIEEE 2012

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In a sample of hydrogen-like atoms,all of which are in the ground state,a photon beam containing photons of various energies is passed. In the absorption spectrum,five dark lines are observed. The number of bright lines in the emission spectrum will be (assume that all transitions take place).

Similar Questions

The diagram shows the energy levels for an electron in a certain atom. Which transition shown represents the emission of a photon with the most energy?

Explain the formulas for the energy of an electron in an atom revolving around the nucleus in different orbits.

In a hydrogen atom,the electron makes a transition from the $(n+1)^{\text{th}}$ level to the $n^{\text{th}}$ level. If $n >> 1$,the frequency of the radiation emitted is proportional to:

Energy of a stationary electron in the hydrogen atom is $E = -\frac{13.6}{n^2} \text{ eV}$. Calculate the energies required to excite the electron in a hydrogen atom to $(a)$ its second excited state and $(b)$ its ionized state,respectively.

$A$ hypothetical atom has only three energy levels. The ground level has energy,$E_1 = -8 \ eV$. The two excited states have energies,$E_2 = -6 \ eV$ and $E_3 = -2 \ eV$. Which of the following wavelengths will $NOT$ be present in the emission spectrum of this atom (in $nm$)?

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