In a hydrogen atom,the electron makes a transition from the n = 8 to the n = 3 state.The wavelength of the emitted photon is closest to which one of the following values? (c = 3.00 × 10⁸ m/s,1 eV = 1.60 × 10^-19J,h = 6.626 × 10^-34 J ∙ s) A)9.57 × 10^-7 m B)1.13 × 10^-6 m C)3.12 × 10^-7 m D)4.52 × 10^-6 m E)6.34 × 10^-7 m

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Quizplus · Accepted Answer

The wavelength of the emitted photon can be calculated using the Rydberg formula for the energy difference between two hydrogen atom states, which is then converted to wavelength using the relation $E = \frac{hc}{\lambda}$. The energy levels of a hydrogen atom are given by $E_n = -\frac{13.6 \text{ eV}}{n^2}$, where $n$ is the principal quantum number. The energy difference between the $n = 8$ and $n = 3$ levels is calculated and then used to find the wavelength of the emitted photon. The closest value provided is $9.57 \times 10^{-7} \text{ m}$, which corresponds to the typical results of such calculations considering the energy levels involved.

In a Hydrogen Atom,the Electron Makes a Transition from the N