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:

$A$ photon is emitted in transition from $n = 4$ to $n = 1$ level in a hydrogen atom. The corresponding wavelength for this transition is $......... \, nm$ (given,$h = 4 \times 10^{-15} \, eV \cdot s$ and $c = 3 \times 10^8 \, m/s$):

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.....$eV$.

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

$A$ $12.5 \text{ eV}$ electron beam is used to bombard gaseous hydrogen at ground state. The energy level up to which the hydrogen atoms would be excited is:

The maximum wavelength of incident radiation required to ionize a hydrogen atom in its ground state is nearly