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

In an atom,an electron requires $47.2 \, eV$ of energy to transition from the $n = 2$ orbit to the $n = 3$ orbit. The atomic number $Z$ of the atom is:

For a certain hypothetical one-electron atom,the wavelength (in $\mathring{A}$) for the spectral lines for transition from $n = p$ to $n = 1$ is given by $\lambda = \frac{1500p^2}{p^2 - 1}$ (where $p > 1$). The ionization potential of this element must be ......$V$ (Take $hc = 12420 \text{ eV-} \mathring{A}$).

Out of the following transitions in a hydrogen atom,identify the transition which emits photons of highest frequency.

If an electron in the excited state falls to the ground state,a photon of energy $5 \ eV$ is emitted. The wavelength of the photon is nearly: (in $nm$)

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