(Solved): 16. Calculate the energy (J) released when an electron in the hydrogen atom transitions from energy ...

16. Calculate the energy $$(\mathrm{J})$$ released when an electron in the hydrogen atom transitions from energy level $$n=3$$ to energy level $$n=2$$ using the Bohr model. Use the following equation to calculate the energy released during the transition of an electron from an upper orbital to lower orbital (after a nearly instantaneous energy absorption) $$\begin{array}{l}{E}_{\text{photon }}=??E_{\text{atom }}\\ E_{\text{photon }}=2.18\times 10^{?18}\mathrm{J}?\left[\frac{1}{n_{f^2}^2}?\frac{1}{n_i^2}\right]\\ \text{ recall }{E}_{\text{photon }}=hv=\frac{hc}{?}\\ \text{ where }h=6.626\times 10^{?34}\mathrm{J}?\sec \left(\frac{\mathrm{kg}?{\mathrm{m}}^2}{\sec }\right)\text{ and }\mathrm{c}=3.0\times 10^8\mathrm{m}/\sec \end{array}$$ Will the emitted photon be visible? (hint: calculate $$?$$ in $$\mathrm{nm}$$ )