(A) The energy $E$ of a hydrogen-like atom with atomic number $Z$ and principal quantum number $n$ is given by the formula:$E_n = -13.6 \times \frac{Z

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(A) The energy $E$ of a hydrogen-like atom with atomic number $Z$ and principal quantum number $n$ is given by the formula:$E_n = -13.6 \times \frac{Z^2}{n^2} \, eV$For the $He^+$ ion,the atomic number $Z = 2$.For the first excited state,the principal quantum number $n = 2$.Substituting these values into the formula:$E_2 = -13.6 \times \frac{2^2}{2^2} \, eV$$E_2 = -13.6 \times \frac{4}{4} \, eV$$E_2 = -13.6 \, eV$.

Class 12 Physics Atoms Bohr's Model of Hydrogen Atom

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The energy of a hydrogen atom in the ground state is $-13.6 \, eV$. The energy of the $He^+$ ion in the first excited state will be .... $eV$.

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A
$-13.6$
B
$-27.2$
C
$-54.4$
D
$-6.8$

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The energy of a hydrogen atom in the ground state is $-13.6 \, eV$. The energy of the $He^+$ ion in the first excited state will be .... $eV$.

Similar Questions

Which of the following is a property of the Rydberg constant?

The ground state energy of a hydrogen atom is $-13.6 \text{ eV}$. What is the ratio of the kinetic energy to the potential energy of the electron in this state?

As per the Bohr model,the minimum energy (in $eV$) required to remove an electron from the ground state of a doubly ionized $Li$ atom $(Z = 3)$ is:

The ratio of the velocity of an electron in the ground state of a hydrogen atom to the velocity of light (in $CGS$ units) is:

The angular momentum of an electron in a hydrogen atom is proportional to: (Where $r$ is the radius of the orbit of the electron)

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