The ionisation energy of a hydrogen atom is $13.6 \, eV$. Following Bohr's theory,the energy corresponding to a transition between the $3^{rd}$ and the $4^{th}$ orbit is.....$eV$.

In a sample of hydrogen-like atoms,all of which are in the ground state,a photon beam containing photons of various energies is passed. In the absorption spectrum,five dark lines are observed. The number of bright lines in the emission spectrum will be (assume that all transitions take place).

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?

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:

If $n$ is the orbit number of the electron in a hydrogen atom,the correct statement among the following is

What is an emission line?