The binding energy of hydrogen is 13.6 eV.The wavelength of the emission line corresponding to the transition from n = 4 to n = 3 is A)1.9 $\times$ 10^-6 m B)8.2 $\times$ 10^-7 m C)5.3 $\times$ 10⁵ m D)3.0 $\times$ 10^-25 m E)1.6 $\times$ 10¹⁴ m

Question

Quizplus · Accepted Answer

The energy difference between the levels in the hydrogen atom can be calculated using the formula for the energy levels of a hydrogen atom: $E_n = -\frac{13.6 \text{ eV}}{n^2}$, where $n$ is the principal quantum number. For a transition from $n = 4$ to $n = 3$, the energy of the photon emitted can be calculated using the difference in energy levels: $E_{photon} = E_3 - E_4$. The wavelength ($\lambda$) of the emitted photon can then be found using the relation $E = \frac{hc}{\lambda}$, where $h$ is Planck's constant and $c$ is the speed of light. The calculation will show that the wavelength corresponds to the option given in A.

The Binding Energy of Hydrogen Is 13 ×\times× 10-6 M B)8 ×\times×

The Binding Energy of Hydrogen Is 13 $\times$ 10^-6 M
B)8 $\times$