The diagram shows the energy levels for an electron in a certain atom. Which transition shown represents the emission of a photon with maximum wavelength?

In the above figure,$D$ and $E$ respectively represent:

When an electron in the ground state of a hydrogen atom is given $12.4 \, eV$ of energy,to which orbit will it transition?

$A$ monochromatic light is incident on a hydrogen sample in the ground state. Hydrogen atoms absorb a fraction of light and subsequently emit radiation of six different wavelengths. The frequency of incident light is $x \times 10^{15} \ Hz$. The value of $x$ is (Given $h = 4.25 \times 10^{-15} \ eVs$)

Energy of an electron in $n^{th}$ orbit of hydrogen atom is $\left( {k = \frac{1}{{4\pi {\varepsilon _0}}}} \right)$

The energy required to remove an electron from the $n = 10$ state of a hydrogen atom is ....... (in $, eV$)