The energy required to remove an electron from the $n = 10$ state of a hydrogen atom is ....... (in $, eV$)

To excite the spectral line of wavelength $4960 \mathring A$ of an atom,an excitation energy of $7.7 \text{ eV}$ is required. The ground state energy of the atom is $10.5 \text{ eV}$. The energies of the two levels involved in the emission of the $4960 \mathring A$ line are (Assume $hc = 1240 \text{ eV nm}$,where $h$ is Planck's constant and $c$ is the speed of light).

The first excited state of a hydrogen atom is $10.2 \, eV$ above its ground state. The temperature needed to excite hydrogen atoms to the first excited level is

The energy of an electron in the $n^{th}$ orbit of a hydrogen atom is given by $E_n = -\frac{13.6}{n^2} \, eV$. How much energy in $eV$ is required to move an electron from the $n = 2$ orbit to the $n = 3$ orbit?

Which of the following transitions in hydrogen atoms emit photons of highest frequency?

An electron in a hydrogen atom undergoes a transition from an orbit with quantum number $n_i$ to another with quantum number $n_f$. $V_i$ and $V_f$ are respectively the initial and final potential energies of the electron. If $\frac{V_i}{V_f} = 6.25$,then the smallest possible $n_f$ is: