The energy \(E\) of the emitted photon is given by:
\(E=\frac{h c}{\lambda}\)...(i)
Here, \(h\) is Planck's constant, \(c\) is the speed of light and \(\lambda\) is the wavelength of the photon emitted.
The energy \(E_{n}\) of the electron in the nth energy level is given by
\(E_{n}=-\frac{13.6}{n^{2}} {eV}\)...(ii)
The change in angular momentum \(\Delta L\) of an atom is given by
\(\Delta L=\left(n_{1}-n_{2}\right) \frac{h}{2 \pi} \ldots \ldots(iii)\)
Here, \(n_{1}\) is the initial energy level, \(n_{2}\) is the final energy level and \(h\) is the Planck's constant.
We have given that the wavelength of the photon emitted by the hydrogen atom is \(1027 \stackrel{\circ}{{A}} . \lambda=1027 \stackrel{\circ}{{A}}\).
Substitute \(6.626 \times 10^{-34} {~J} \cdot {s}\) for \(h, 3 \times 10^{8} {~m} / {s}\) for \(c\) and \(1027 \stackrel{0}{{~A}}\) for \(\lambda\) in equation (i)
\(E=\frac{\left(6.626 \times 10^{-34} {~J} \cdot {s}\right)\left(3 \times 10^{8} {~m} / {s}\right)}{1027 \stackrel{\circ}{{A}}}\)
\(E=\frac{\left(6.626 \times 10^{-34} {~J} \cdot {s}\right)\left(3 \times 10^{8} {~m} / {s}\right)}{1027 \times 10^{-10} {~m}}\)
\(E=19.35 \times 10^{-19} {~J}\)
Convert this value of energy of the hydrogen atom into electronvolt.
\(\Delta E=\frac{19.35 \times 10^{-19} \mathrm{~J}}{1.6 \times 10^{-19} \mathrm{C}} \)
\(\Delta E=12.1 {eV}\)
Hence, the energy of the photon emitted from the hydrogen atom is \(12.1 \mathrm{eV}\).
Let us calculate the energy difference between the first and third energy level of the hydrogen atom using equation (ii).
\(E_{3}-E_{1}=\left(-\frac{13.6}{(3)^{2}} {eV}\right)-\left(-\frac{13.6}{(1)^{2}} {eV}\right)\)
\(E_{3}-E_{1}=(-1.5 {eV})-(-13.6 {eV})\)
\(E_{3}-E_{1}=12.1 {eV}\)
From the above calculations, it is clear that the electron in the hydrogen atom jumps from third energy level to the first energy level.Let us now calculate the change in angular momentum of the hydrogen atom using equation (3).
Substitute 3 for \(n_{1}\) and 1 for \(n_{2}\) in equation (3).
\(\Delta L=(3-1) \frac{h}{2 \pi} \)
\(\Delta L=(2) \frac{h}{2 \pi}\)
\(\Delta L=\frac{h}{\pi}\)
Therefore, the change in angular momentum of the hydrogen atom is \(\frac{h}{\pi}\)