When a hydrogen atom is raised from the ground state to the excited state,

An electron in the $n = 1$ orbit of a hydrogen atom is bound by $13.6 \, eV$. If a hydrogen atom is in the $n = 3$ state,how much energy is required to ionize it?

The $1^{st}, 2^{nd},$ and $3^{rd}$ energy levels of an atom are $E, 4E/3,$ and $2E$ respectively. If a wavelength $\lambda$ is emitted during the transition $3 \to 1$,what is the wavelength emitted during the transition $2 \to 1$?

The energy of a hydrogen atom in its ground state is $-13.6 \,eV$. The energy of the level corresponding to $n=7$ is ...... $eV$.

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 ratio of energies of photons produced due to transition of an electron in a hydrogen atom from the second energy level to the first energy level and from the fifth energy level to the second energy level is: