$A$ hydrogen atom absorbs radiation of wavelength $975 \, \text{\AA}$ to transition from the ground state to an excited state. To which energy level will the atom transition?

In the Bohr model of the hydrogen atom,what is the energy required to remove an electron from the ground state $(n = 1)$ (in $eV$)?

An electron in a hydrogen atom first jumps from the third excited state to the second excited state and then from the second excited state to the first excited state. The ratio of the wavelengths $\lambda_1 : \lambda_2$ emitted in the two cases is

If the binding energy of the electron in a hydrogen atom is $13.6 \ eV$,the energy required to remove the electron from the first excited state of $Li^{++}$ is.....$eV$.

The total energy of an electron revolving in the second orbit of a hydrogen atom is

The energy levels of an atom are shown below. When an electron makes a transition from an energy level of $2E$ to an energy level of $E$,the wavelength of the emitted electromagnetic radiation is $\lambda$. What is the wavelength of the emitted photon when the electron makes a transition from an energy level of $4E/3$ to an energy level of $E$?