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All of those transitions are definitely happening when we place H\(_2\) into the spectrum tube—but we don’t see all of those transitions and that has to do with the limited wavelengths that human eyes can see. Now I want you to determine which transitions were associated with the visible spectrum. Use the formulas \(E = h\nu\) and \(c = \lambda \nu\) to convert those energy values into wavelengths (in nanometers). (E is the energy in J, h is Planck’s Constant \(6.63 \times 10^{-34} \, \text{J}\cdot\text{s}\), and c is the speed of light \(3.00 \times 10^8 \, \text{m/s}\). Again I have done the first one so you can make sure you are doing this correctly. | \(\lambda \, (\text{nm})\) | |-----------------------------| | \(\begin{array}{c|c|c|c|c|c} n_{\text{initial}} \downarrow & 1 & 2 & 3 & 4 & 5 \\ \hline 6 & & & & & & 93.8 \, \text{nm} \\ 5 & & & & & & \\ 4 & & & & & & \\ 3 & & & & & & \\ 2 & & & & & & \\ \end{array}\) 1. Indicate the energy level transitions that correspond to the visible spectral lines by highlighting each appropriate cell in yellow. 2. Indicate the energy level transitions that correspond to infrared light by highlighting each appropriate cell in red. 3. Indicate the energy level transitions that correspond to ultraviolet light by highlighting each appropriate cell in blue.

All of those transitions are definitely happening when we place H\(_2\) into the spectrum tube—but we don’t see all of those transitions and that has to do with the limited wavelengths that human eyes can see. Now I want you to determine which transitions were associated with the visible spectrum. Use the formulas \(E = h\nu\) and \(c = \lambda \nu\) to convert those energy values into wavelengths (in nanometers). (E is the energy in J, h is Planck’s Constant \(6.63 \times 10^{-34} \, \text{J}\cdot\text{s}\), and c is the speed of light \(3.00 \times 10^8 \, \text{m/s}\). Again I have done the first one so you can make sure you are doing this correctly. | \(\lambda \, (\text{nm})\) | |-----------------------------| | \(\begin{array}{c|c|c|c|c|c} n_{\text{initial}} \downarrow & 1 & 2 & 3 & 4 & 5 \\ \hline 6 & & & & & & 93.8 \, \text{nm} \\ 5 & & & & & & \\ 4 & & & & & & \\ 3 & & & & & & \\ 2 & & & & & & \\ \end{array}\) 1. Indicate the energy level transitions that correspond to the visible spectral lines by highlighting each appropriate cell in yellow. 2. Indicate the energy level transitions that correspond to infrared light by highlighting each appropriate cell in red. 3. Indicate the energy level transitions that correspond to ultraviolet light by highlighting each appropriate cell in blue.

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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All of those transitions are definitely happening when we place H\(_2\) into the spectrum tube—but we don’t see all of those transitions and that has to do with the limited wavelengths that human eyes can see. Now I want you to determine which transitions were associated with the visible spectrum. Use the formulas \(E = h\nu\) and \(c = \lambda \nu\) to convert those energy values into wavelengths (in nanometers). (E is the energy in J, h is Planck’s Constant \(6.63 \times 10^{-34} \, \text{J}\cdot\text{s}\), and c is the speed of light \(3.00 \times 10^8 \, \text{m/s}\). Again I have done the first one so you can make sure you are doing this correctly. | \(\lambda \, (\text{nm})\) | |-----------------------------| | \(\begin{array}{c|c|c|c|c|c} n_{\text{initial}} \downarrow & 1 & 2 & 3 & 4 & 5 \\ \hline 6 & & & & & & 93.8 \, \text{nm} \\ 5 & & & & & & \\ 4 & & & & & & \\ 3 & & & & & & \\ 2 & & & & & & \\ \end{array}\) 1. Indicate the energy level transitions that correspond to the visible spectral lines by highlighting each appropriate cell in yellow. 2. Indicate the energy level transitions that correspond to infrared light by highlighting each appropriate cell in red. 3. Indicate the energy level transitions that correspond to ultraviolet light by highlighting each appropriate cell in blue.
Transcribed Image Text:All of those transitions are definitely happening when we place H\(_2\) into the spectrum tube—but we don’t see all of those transitions and that has to do with the limited wavelengths that human eyes can see. Now I want you to determine which transitions were associated with the visible spectrum. Use the formulas \(E = h\nu\) and \(c = \lambda \nu\) to convert those energy values into wavelengths (in nanometers). (E is the energy in J, h is Planck’s Constant \(6.63 \times 10^{-34} \, \text{J}\cdot\text{s}\), and c is the speed of light \(3.00 \times 10^8 \, \text{m/s}\). Again I have done the first one so you can make sure you are doing this correctly. | \(\lambda \, (\text{nm})\) | |-----------------------------| | \(\begin{array}{c|c|c|c|c|c} n_{\text{initial}} \downarrow & 1 & 2 & 3 & 4 & 5 \\ \hline 6 & & & & & & 93.8 \, \text{nm} \\ 5 & & & & & & \\ 4 & & & & & & \\ 3 & & & & & & \\ 2 & & & & & & \\ \end{array}\) 1. Indicate the energy level transitions that correspond to the visible spectral lines by highlighting each appropriate cell in yellow. 2. Indicate the energy level transitions that correspond to infrared light by highlighting each appropriate cell in red. 3. Indicate the energy level transitions that correspond to ultraviolet light by highlighting each appropriate cell in blue.
Expert Solution
Step 1

Rydberg equation is given by,

1λ=1.0967757×107×(1nf2-1ni2) m-1

 

Range of visible spectral lines is 400 nm to 700 nm

Range of infrared light is 800 nm to 1 mm

Range of ultraviolet light is 100 nm 400 nm

 

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