6. Which photon will correspond with the transition labeled B? a. The absorption of a 248 nm photon. b. The emission of a 155 nm photon. c. The emission of a 487 nm photon. d. The absorption of a 155 nm photon. e. The emission of a 248 nm photon.
6. Which photon will correspond with the transition labeled B? a. The absorption of a 248 nm photon. b. The emission of a 155 nm photon. c. The emission of a 487 nm photon. d. The absorption of a 155 nm photon. e. The emission of a 248 nm photon.
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Chapter1: Units, Trigonometry. And Vectors
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![### Quantum Transitions and Photons
In this exercise, we will analyze transitions between energy levels and their corresponding photon absorptions and emissions.
#### Diagram Explanation:
The diagram provided is an energy level diagram displaying different principal quantum numbers and their corresponding energy levels measured in electron volts (eV).
- **Principal Quantum Numbers (n):** These run along the vertical axis and are marked from n=1 to n=5.
- **Energy Levels:** The energy levels associated with each principal quantum number are marked. For instance:
- n=1 has an energy of -15 eV.
- n=2 has an energy of -8 eV.
- n=3 has an energy of -5 eV.
- n=4 has an energy of -3 eV.
#### Transitions:
- **Transition A:** From n=2 to n=1.
- **Transition B:** From n=3 to n=2.
- **Transition C:** From n=4 to n=3.
- **Transition D:** From n=4 to n=1.
- **Transition E:** From n=3 to n=4.
#### Questions:
**5. Which transition corresponds to the absorption of the photon with the shortest wavelength?**
The photon with the shortest wavelength corresponds to the largest energy difference.
- A. A.
- B. B.
- C. C.
- D. D.
- E. E.
**6. Which photon will correspond with the transition labeled B?**
Transition B is from n=3 to n=2.
- A. The absorption of a 248 nm photon.
- B. The emission of a 155 nm photon.
- C. The emission of a 487 nm photon.
- D. The absorption of a 155 nm photon.
- E. The emission of a 248 nm photon.
To answer these questions correctly, remember that the energy of a photon is inversely proportional to its wavelength. The energy of the transition can be calculated using the formula:
\[ E = \frac{hc}{\lambda} \]
where \( h \) is Planck's constant, \( c \) is the speed of light, and \( \lambda \) is the wavelength. Large energy differences correspond to shorter wavelengths.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0959128f-1417-4f4f-bd20-8f81c7fe5d61%2Fcee87474-8773-4941-a16b-dd16242854ae%2Fwcr41id.png&w=3840&q=75)
Transcribed Image Text:### Quantum Transitions and Photons
In this exercise, we will analyze transitions between energy levels and their corresponding photon absorptions and emissions.
#### Diagram Explanation:
The diagram provided is an energy level diagram displaying different principal quantum numbers and their corresponding energy levels measured in electron volts (eV).
- **Principal Quantum Numbers (n):** These run along the vertical axis and are marked from n=1 to n=5.
- **Energy Levels:** The energy levels associated with each principal quantum number are marked. For instance:
- n=1 has an energy of -15 eV.
- n=2 has an energy of -8 eV.
- n=3 has an energy of -5 eV.
- n=4 has an energy of -3 eV.
#### Transitions:
- **Transition A:** From n=2 to n=1.
- **Transition B:** From n=3 to n=2.
- **Transition C:** From n=4 to n=3.
- **Transition D:** From n=4 to n=1.
- **Transition E:** From n=3 to n=4.
#### Questions:
**5. Which transition corresponds to the absorption of the photon with the shortest wavelength?**
The photon with the shortest wavelength corresponds to the largest energy difference.
- A. A.
- B. B.
- C. C.
- D. D.
- E. E.
**6. Which photon will correspond with the transition labeled B?**
Transition B is from n=3 to n=2.
- A. The absorption of a 248 nm photon.
- B. The emission of a 155 nm photon.
- C. The emission of a 487 nm photon.
- D. The absorption of a 155 nm photon.
- E. The emission of a 248 nm photon.
To answer these questions correctly, remember that the energy of a photon is inversely proportional to its wavelength. The energy of the transition can be calculated using the formula:
\[ E = \frac{hc}{\lambda} \]
where \( h \) is Planck's constant, \( c \) is the speed of light, and \( \lambda \) is the wavelength. Large energy differences correspond to shorter wavelengths.
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