(A) represents the excitation of an electron from the $n=2$ orbit to the $n=4$ orbit,which corresponds to an absorption line in the Balmer series.$E$

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Absorption line of Balmer series and the ionization potential of hydrogen

(A) represents the excitation of an electron from the $n=2$ orbit to the $n=4$ orbit,which corresponds to an absorption line in the Balmer series.$E$ represents the transition of an electron from the $\infty$ orbit to the $n=1$ orbit,which corresponds to the energy released equal to the ionization potential of hydrogen $(13.6 \ eV)$.

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

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In the above figure,$D$ and $E$ respectively represent:

A
Absorption line of Balmer series and the ionization potential of hydrogen
B
Absorption line of Balmer series and the wavelength lesser than lowest of the Lyman series
C
Spectral line of Balmer series and the maximum wavelength of Lyman series
D
Spectral line of Lyman series and the absorption of greater wavelength of limiting value of Paschen series

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Electron Energy and Electron Energy Levels in Hydrogen Atom

In the hydrogen atom,if the reference level of potential energy is assumed to be zero at the ground state level,choose the incorrect statement.

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Energy of an electron (in $eV$) in the $2^{nd}$ orbit of a $He^{+}$ ion is (in $.6$)?

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The energy levels of an electron in an atom are shown. Which transition of the electron represents the emission of a photon with the highest energy?

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An electron makes a transition from an excited state to the ground state of a hydrogen-like atom. Out of the following statements,which one is correct?

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In the above figure,$D$ and $E$ respectively represent:

Similar Questions

In the hydrogen atom,if the reference level of potential energy is assumed to be zero at the ground state level,choose the incorrect statement.

In an atom, the difference between two energy levels is $3.31 \ eV$. The wavelength of the radiation emitted when the transition takes place between these levels is nearly: (in $Å$)

Energy of an electron (in $eV$) in the $2^{nd}$ orbit of a $He^{+}$ ion is (in $.6$)?

The energy levels of an electron in an atom are shown. Which transition of the electron represents the emission of a photon with the highest energy?

An electron makes a transition from an excited state to the ground state of a hydrogen-like atom. Out of the following statements,which one is correct?

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