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E (J) nfinal:→ 1 4. ninitial 6. 2.12 * 10-18 J 4. 3. 2. 2.

E (J) nfinal:→ 1 4. ninitial 6. 2.12 * 10-18 J 4. 3. 2. 2.

Chemistry
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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**Part B - The Rydberg Equation: What do the Spectral Lines of Hydrogen Tell Us?** Look below at the line spectrum for Hydrogen. Since Hydrogen is such a simple element (having only one electron), we can model and predict its behavior with (relatively) simple equations. --- **Diagram:** - **Spectrum Visualization:** - The spectrum contains several vertical lines at specific wavelengths. Each line corresponds to a wavelength where light is emitted by hydrogen. - **Wavelengths (in nm):** - 410 nm - 434 nm - 486 nm - 656 nm --- **Where** \( R_H = 2.18 \times 10^{-18} \, J \) and \( n_{\text{initial}} \) and \( n_{\text{final}} \) represent the initial and final energy levels of the electron—that is, the electron starts at the \( n_{\text{initial}} \) energy level and relaxes to the \( n_{\text{final}} \) energy level. For instance, the first box in the table represents the energy released when an electron in the 6th shell falls to the 1st shell. Use the Rydberg equation above to complete the following table. I have done the first one so you can make sure you are doing this correctly. --- **Table:** | E (J) | \( n_{\text{final}}: \rightarrow \) | |--------------|---|---|---|---|---| | \( n_{\text{initial}}: \downarrow \) | 1 | 2 | 3 | 4 | 5 | | 6 | 2.12 \( \times \) 10\(^{-18}\) J | | | | | | 5 | | | | | | | 4 | | | | | | | 3 | | | | | | | 2 | | | | | | ---
Transcribed Image Text:**Part B - The Rydberg Equation: What do the Spectral Lines of Hydrogen Tell Us?** Look below at the line spectrum for Hydrogen. Since Hydrogen is such a simple element (having only one electron), we can model and predict its behavior with (relatively) simple equations. --- **Diagram:** - **Spectrum Visualization:** - The spectrum contains several vertical lines at specific wavelengths. Each line corresponds to a wavelength where light is emitted by hydrogen. - **Wavelengths (in nm):** - 410 nm - 434 nm - 486 nm - 656 nm --- **Where** \( R_H = 2.18 \times 10^{-18} \, J \) and \( n_{\text{initial}} \) and \( n_{\text{final}} \) represent the initial and final energy levels of the electron—that is, the electron starts at the \( n_{\text{initial}} \) energy level and relaxes to the \( n_{\text{final}} \) energy level. For instance, the first box in the table represents the energy released when an electron in the 6th shell falls to the 1st shell. Use the Rydberg equation above to complete the following table. I have done the first one so you can make sure you are doing this correctly. --- **Table:** | E (J) | \( n_{\text{final}}: \rightarrow \) | |--------------|---|---|---|---|---| | \( n_{\text{initial}}: \downarrow \) | 1 | 2 | 3 | 4 | 5 | | 6 | 2.12 \( \times \) 10\(^{-18}\) J | | | | | | 5 | | | | | | | 4 | | | | | | | 3 | | | | | | | 2 | | | | | | ---
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