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

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$A$ hydrogen atom makes a transition from $n = 2$ to $n = 1$ and emits a photon. This photon strikes a doubly ionized lithium atom $(Z = 3)$ in an excited state and completely removes the orbiting electron. The least quantum number for the excited state of the ion for this process is:

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The electron in a hydrogen atom makes a transition from an excited state to the ground state. Which of the following statements is true?

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