(B) The energy of an electron in the $n$-th orbit of a hydrogen atom is given by $E_n = -\frac{13.6 \ eV}{n^2}$.For the ground state $(n=1)$, $E_1 = -

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(B) The energy of an electron in the $n$-th orbit of a hydrogen atom is given by $E_n = -\frac{13.6 \ eV}{n^2}$.For the ground state $(n=1)$, $E_1 = -13.6 \ eV$.For the $M$-shell $(n=3)$, the energy is $E_3 = -\frac{13.6 \ eV}{3^2} = -\frac{13.6}{9} \ eV \approx -1.51 \ eV$.To ionize the hydrogen atom from the $M$-state, the atom must be provided with enough energy to reach the ionization limit $(E_{\infty} = 0 \ eV)$.The energy required is $\Delta E = E_{\infty} - E_3 = 0 - (-1.51 \ eV) = +1.51 \ eV$.Therefore, the second electron must transfer at least $+1.51 \ eV$ of energy to the atom.

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

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In an inelastic collision, an electron excites a hydrogen atom from its ground state to an $M$-shell state. $A$ second electron collides instantaneously with the excited hydrogen atom in the $M$-state and ionizes it. At least how much energy must the second electron transfer to the atom in the $M$-state?

WBJEE 2011 All WBJEE

A
$+3.4 \ eV$
B
$+1.51 \ eV$
C
$-3.4 \ eV$
D
$-1.51 \ eV$

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Class 12

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Atoms

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Electron Energy and Electron Energy Levels in Hydrogen Atom

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The ionisation potential of hydrogen atom is $13.6 \ V$. The energy required to remove an electron from the second orbit of hydrogen is......$eV$.

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The energy levels of an atom are shown in the figure. Which one of these transitions will result in the emission of a photon of wavelength $124.1 \, nm$? Given $(h = 6.62 \times 10^{-34} \, Js)$.

MediumJEE MAIN 2023

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$A$ stationary hydrogen atom has an electron that transitions from the fifth energy level to the ground level. The velocity that the atom acquires as a result of photon emission will be: ($m$ is the mass of the atom,$R$ is Rydberg constant,and $h$ is Planck's constant).

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The total energy of an electron in the first excited state of the hydrogen atom is about $-3.4 \; eV.$
$(a)$ What is the kinetic energy of the electron in this state?
$(b)$ What is the potential energy of the electron in this state?
$(c)$ Which of the answers above would change if the choice of the zero of potential energy is changed?

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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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The ionisation potential of hydrogen atom is $13.6 \ V$. The energy required to remove an electron from the second orbit of hydrogen is......$eV$.

The energy levels of an atom are shown in the figure. Which one of these transitions will result in the emission of a photon of wavelength $124.1 \, nm$? Given $(h = 6.62 \times 10^{-34} \, Js)$.

$A$ stationary hydrogen atom has an electron that transitions from the fifth energy level to the ground level. The velocity that the atom acquires as a result of photon emission will be: ($m$ is the mass of the atom,$R$ is Rydberg constant,and $h$ is Planck's constant).

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.

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