In a hydrogen atom, the energy of an electron in the first and third orbits is $E_1$ and $E_3$ respectively. If $E_3 = x E_1$, then the value of $x$ will be:

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

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 $E$?

In a hydrogen atom,which of the following transitions will emit a photon of the highest frequency?

How much energy is needed to release the electron from the second excited state in the hydrogen atom (in $eV$)?

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: