In the following transitions of a hydrogen atom,which one corresponds to the highest frequency of emitted radiation?

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 levels with transitions for an atom are shown in the figure. The transitions corresponding to the emission of radiation of maximum and minimum wavelength are respectively:

When an electron transition takes place from an excited state to the ground state in a hydrogen atom, then:

In a hydrogen atom,the electron makes a transition from the $(n+1)^{\text{th}}$ level to the $n^{\text{th}}$ level. If $n >> 1$,the frequency of the radiation emitted is proportional to:

How much work must be done to pull apart the electron and the proton that make up the Hydrogen atom,if the atom is initially in the state with $n = 2$?