(A) For a hydrogen atom, the energy levels are given by $E_n = -\frac{13.6 \text{ eV}}{n^2}$.As the electron transitions from an excited state to the

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Its kinetic energy increases, but potential energy and total energy decrease.

(A) For a hydrogen atom, the energy levels are given by $E_n = -\frac{13.6 \text{ eV}}{n^2}$.As the electron transitions from an excited state to the ground state, $n$ decreases.$1$. Total energy $E_T = -\frac{13.6}{n^2} \text{ eV}$. As $n$ decreases, $E_T$ becomes more negative, so it decreases.$2$. Kinetic energy $E_K = -E_T = \frac{13.6}{n^2} \text{ eV}$. As $n$ decreases, $E_K$ increases.$3$. Potential energy $E_P = 2E_T = -\frac{27.2}{n^2} \text{ eV}$. As $n$ decreases, $E_P$ becomes more negative, so it decreases.

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

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When an electron transition takes place from an excited state to the ground state in a hydrogen atom, then:

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A
Its kinetic energy increases, but potential energy and total energy decrease.
B
Its kinetic energy, potential energy, and total energy decrease.
C
Kinetic energy decreases, potential energy increases, but total energy remains the same.
D
Kinetic energy and total energy decrease, but potential energy increases.

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Electron Energy and Electron Energy Levels in Hydrogen Atom

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Due to transitions among its first three energy levels,a hydrogenic atom emits radiation at three discrete wavelengths $\lambda_1, \lambda_2$ and $\lambda_3$ (where $\lambda_1 < \lambda_2 < \lambda_3$). Then,

MediumKVPY 2011

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The ratio of energies of photons produced due to the transition of an electron in a hydrogen atom from its $(a)$ second to first energy level and $(b)$ highest energy level to the second level is:

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The ionisation energy of a hydrogen atom is $13.6 \, eV$. Following Bohr's theory,the energy corresponding to a transition between the $3^{rd}$ and the $4^{th}$ orbit is.....$eV$.

MediumAIPMT 1992

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When a hydrogen atom transitions from $n=2$ to $n=1$, it emits a photon. The recoil speed of the atom is $\frac{x}{5} \,m/s$. Find the value of $x$. (Use: mass of hydrogen atom $= 1.6 \times 10^{-27} \,kg$)

DifficultJEE MAIN 2024

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Assertion : Between any two given energy levels,the number of absorption transitions is always less than the number of emission transitions.
Reason : Absorption transitions start from the lowest energy level only and may end at any higher energy level. But emission transitions may start from any higher energy level and end at any energy level below it.

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When an electron transition takes place from an excited state to the ground state in a hydrogen atom, then:

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Due to transitions among its first three energy levels,a hydrogenic atom emits radiation at three discrete wavelengths $\lambda_1, \lambda_2$ and $\lambda_3$ (where $\lambda_1 < \lambda_2 < \lambda_3$). Then,

The ratio of energies of photons produced due to the transition of an electron in a hydrogen atom from its $(a)$ second to first energy level and $(b)$ highest energy level to the second level is:

The ionisation energy of a hydrogen atom is $13.6 \, eV$. Following Bohr's theory,the energy corresponding to a transition between the $3^{rd}$ and the $4^{th}$ orbit is.....$eV$.

When a hydrogen atom transitions from $n=2$ to $n=1$, it emits a photon. The recoil speed of the atom is $\frac{x}{5} \,m/s$. Find the value of $x$. (Use: mass of hydrogen atom $= 1.6 \times 10^{-27} \,kg$)

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