I couldn't fit both parts of the question into one picture so please answer both sections. Thank you. **Photon Emission in Hydrogen Atom Transition**Calculate the energy of a photon emitted when an electron in a hydrogen atom undergoes a transition from \( n = 6 \) to \( n = 1 \).**Energy Emitted:**[Text Box for Input] \( \text{J} \)---This process involves using the Rydberg formula to calculate the photon energy released during the electron transition. The energy associated with the transition can be calculated using the formula: \[ E = -R_H \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) \]Where:- \( E \) is the energy of the photon emitted,- \( R_H \) is the Rydberg constant (\(2.18 \times 10^{-18}\) J),- \( n_1 \) and \( n_2 \) are the principal quantum numbers of the initial and final states. Here, \( n_1 = 1 \) and \( n_2 = 6 \).When an electron falls to a lower energy level, it releases energy in the form of a photon, which can be quantified using this formula. **Problem Statement**Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level \( n = 7 \) to the level \( n = 1 \).\[ \lambda = \boxed{} \, \text{nm} \]

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Calculate the energy of a photon emitted when an electron in a hydrogen atom undergoes a transition from n = 6 to n = 1. energy emitted:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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