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[References] Consider only transitions involving the n = 1 through n=4 energy levels for the hydrogen atom (using the diagram below). n=4 n= 3 n= 2 VV n= 1 a. How many emission lines are possible, considering only the four quantum levels? b. Photons of the lowest energy are emitted in a transition from the level with n to a level with n c. The emission line having the shortest wavelength corresponds to a transition from the level with n= to the level with n Submit Answer Try Another Version

[References] Consider only transitions involving the n = 1 through n=4 energy levels for the hydrogen atom (using the diagram below). n=4 n= 3 n= 2 VV n= 1 a. How many emission lines are possible, considering only the four quantum levels? b. Photons of the lowest energy are emitted in a transition from the level with n to a level with n c. The emission line having the shortest wavelength corresponds to a transition from the level with n= to the level with n Submit Answer Try Another Version

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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**Understanding Electron Transitions in Hydrogen Atoms** In this exercise, we'll examine the transitions between quantum energy levels in a hydrogen atom, specifically between the levels \( n = 1 \) through \( n = 4 \). ### Diagram Analysis: - The diagram shows four horizontal lines representing energy levels. - These levels are labeled from top to bottom as \( n = 4 \), \( n = 3 \), \( n = 2 \), and \( n = 1 \). - Arrows pointing downwards indicate possible transitions of an electron moving to a lower energy level, which corresponds to emission of energy. ### Questions: **a. How many emission lines are possible, considering only the four quantum levels?** - To determine this, consider all possible transitions between these levels. **b. Photons of the lowest energy are emitted in a transition from the level with \( n = \_\_\_\_ \) to a level with \( n = \_\_\_\_ \).** - This involves the smallest difference in energy between two levels. **c. The emission line having the shortest wavelength corresponds to a transition from the level with \( n = \_\_\_\_ \) to the level with \( n = \_\_\_\_ \).** - This involves the largest energy difference between two levels. Consider these principles: - Larger energy differences result in shorter wavelengths. - Smaller energy differences result in longer wavelengths. By exploring these questions, you'll gain insights into the behavior of electrons in atoms and how they emit light at specific wavelengths.
Transcribed Image Text:**Understanding Electron Transitions in Hydrogen Atoms** In this exercise, we'll examine the transitions between quantum energy levels in a hydrogen atom, specifically between the levels \( n = 1 \) through \( n = 4 \). ### Diagram Analysis: - The diagram shows four horizontal lines representing energy levels. - These levels are labeled from top to bottom as \( n = 4 \), \( n = 3 \), \( n = 2 \), and \( n = 1 \). - Arrows pointing downwards indicate possible transitions of an electron moving to a lower energy level, which corresponds to emission of energy. ### Questions: **a. How many emission lines are possible, considering only the four quantum levels?** - To determine this, consider all possible transitions between these levels. **b. Photons of the lowest energy are emitted in a transition from the level with \( n = \_\_\_\_ \) to a level with \( n = \_\_\_\_ \).** - This involves the smallest difference in energy between two levels. **c. The emission line having the shortest wavelength corresponds to a transition from the level with \( n = \_\_\_\_ \) to the level with \( n = \_\_\_\_ \).** - This involves the largest energy difference between two levels. Consider these principles: - Larger energy differences result in shorter wavelengths. - Smaller energy differences result in longer wavelengths. By exploring these questions, you'll gain insights into the behavior of electrons in atoms and how they emit light at specific wavelengths.
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