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An electron in an atom falls from the second to the first energy level and emits a photon of green light. The same electron is re-excited and then falls from the third to the second energy level. Would the photon emitted in the second case be more likely to be yellow or blue in color? 3.

An electron in an atom falls from the second to the first energy level and emits a photon of green light. The same electron is re-excited and then falls from the third to the second energy level. Would the photon emitted in the second case be more likely to be yellow or blue in color? 3.

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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
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**Topic: The Emission of Photons in Atomic Transitions** **Question:** 3. An electron in an atom falls from the second to the first energy level and emits a photon of green light. The same electron is re-excited and then falls from the third to the second energy level. Would the photon emitted in the second case be more likely to be yellow or blue in color? **Explanation:** In this question, we are exploring the concept of atomic transitions and the emission of photons. When an electron in an atom moves from a higher energy level to a lower one, it releases energy in the form of a photon. The energy of this photon determines its color when it is in the visible spectrum. **Detailed Analysis:** 1. **First Transition:** - The electron falls from the second energy level (n=2) to the first energy level (n=1). - The photon emitted is green in color. - Green light has a specific energy and wavelength associating it with this transition. 2. **Second Transition:** - The electron is re-excited to a higher energy level. - It then falls from the third energy level (n=3) to the second energy level (n=2). - The question asks whether the photon emitted in this transition would be more likely to be yellow or blue. **Explanation of Photon Color:** - The energy difference between the third and second energy levels is less than that between the second and first energy levels since higher energy levels are closer together. - Green light has a wavelength range of approximately 495-570 nm. - Yellow light has a wavelength range of approximately 570-590 nm (it has slightly less energy than green light). - Blue light has a wavelength range of approximately 450-495 nm (it has more energy than green light). Since the energy emitted in the second case is less compared to the first case, the photon would have less energy than that of the green light emitted in the first transition. Therefore, the photon emitted would be likely to have more energy than yellow light but less energy than green light, making it more likely for the photon to be blue in color. In summary, the photon emitted in the second transition (third to second energy level) is more likely to be blue in color.
Transcribed Image Text:**Topic: The Emission of Photons in Atomic Transitions** **Question:** 3. An electron in an atom falls from the second to the first energy level and emits a photon of green light. The same electron is re-excited and then falls from the third to the second energy level. Would the photon emitted in the second case be more likely to be yellow or blue in color? **Explanation:** In this question, we are exploring the concept of atomic transitions and the emission of photons. When an electron in an atom moves from a higher energy level to a lower one, it releases energy in the form of a photon. The energy of this photon determines its color when it is in the visible spectrum. **Detailed Analysis:** 1. **First Transition:** - The electron falls from the second energy level (n=2) to the first energy level (n=1). - The photon emitted is green in color. - Green light has a specific energy and wavelength associating it with this transition. 2. **Second Transition:** - The electron is re-excited to a higher energy level. - It then falls from the third energy level (n=3) to the second energy level (n=2). - The question asks whether the photon emitted in this transition would be more likely to be yellow or blue. **Explanation of Photon Color:** - The energy difference between the third and second energy levels is less than that between the second and first energy levels since higher energy levels are closer together. - Green light has a wavelength range of approximately 495-570 nm. - Yellow light has a wavelength range of approximately 570-590 nm (it has slightly less energy than green light). - Blue light has a wavelength range of approximately 450-495 nm (it has more energy than green light). Since the energy emitted in the second case is less compared to the first case, the photon would have less energy than that of the green light emitted in the first transition. Therefore, the photon emitted would be likely to have more energy than yellow light but less energy than green light, making it more likely for the photon to be blue in color. In summary, the photon emitted in the second transition (third to second energy level) is more likely to be blue in color.
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