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(A) For a hydrogen atom, the energy levels are given by $E_n = -\frac{13.6 	ext{ eV}}{n^2}$.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.

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

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

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