In a hydrogen atom,when an electron jumps from the second to the first orbit,the energy emitted is:

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

An electron collides with a fixed hydrogen atom in its ground state. The hydrogen atom gets excited and the colliding electron loses all its kinetic energy. Consequently,the hydrogen atom may emit a photon corresponding to the largest wavelength of the Balmer series. The minimum kinetic energy $(K.E.)$ of the colliding electron will be.....$eV$.

The diagram shows different transitions across the energy levels for an electron in a certain atom. Among these,which transition represents the emission of a photon with the most energy?

The kinetic energy of an electron in the $n^{th}$ orbit of a hydrogen-like species with atomic number $Z$ is $13.6 \frac{Z^2}{n^2} \ eV$. The potential energy of this electron in the same orbit will be:

Some of the wavelengths observed in the emission spectrum of neutral hydrogen gas are $912, 1026, 1216, 3646, 6563 \, \mathring{A}$. If broadband light is passing through neutral hydrogen gas at room temperature,then the wavelength that will not be absorbed strongly is .................. $\mathring{A}$.