The total energy of an electron in the first excited state of the hydrogen atom is $-3.4 \ eV$. Find out its potential energy in this state.

Consider the following electronic energy level diagram of $H-$ atom. Photons associated with shortest and longest wavelengths would be emitted from the atom by the transitions labelled:

Energy levels $A$,$B$ and $C$ of a certain atom correspond to increasing values of energy,i.e.,$E_A < E_B < E_C$. If $\lambda_1$,$\lambda_2$,and $\lambda_3$ are the wavelengths of the photons corresponding to the transitions shown in the figure,then:

The potential energy of the orbital electron in the ground state of a hydrogen atom is $-E$. What is its kinetic energy?

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

If the ionisation energy for the hydrogen atom is $13.6 \ eV$,then the energy required to excite it from the ground state to the next higher state is nearly: (in $eV$)