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1. On the chart below, arrange the following regions of the electromagnetic spectrum in order of decreasing wavelength: infrared, ultraviolet, green, blue, red, and x-rays. (long) - ) ) ( ( energy per photon ( ) Label the proper ends of the frequency line “high" and "low," and indicate with arrow heads which is the higher end. Color Violet Also label the proper ends of the energy line "high" and "low," again indicating with arrow heads which is the higher end. wavelength frequency 2. A typical value for the wavelength of violet light is 400.0 nm and a typical value for the wavelength of red light is 700.0 nm. Using these wavelength values, complete the following table: Wavelength Red 400.0 nm 700.0 nm Show calculations for violet light here: (short) Frequency J/photon ·( Energy ) kJ/mol photons

1. On the chart below, arrange the following regions of the electromagnetic spectrum in order of decreasing wavelength: infrared, ultraviolet, green, blue, red, and x-rays. (long) - ) ) ( ( energy per photon ( ) Label the proper ends of the frequency line “high" and "low," and indicate with arrow heads which is the higher end. Color Violet Also label the proper ends of the energy line "high" and "low," again indicating with arrow heads which is the higher end. wavelength frequency 2. A typical value for the wavelength of violet light is 400.0 nm and a typical value for the wavelength of red light is 700.0 nm. Using these wavelength values, complete the following table: Wavelength Red 400.0 nm 700.0 nm Show calculations for violet light here: (short) Frequency J/photon ·( Energy ) kJ/mol photons

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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1. On the chart below, arrange the following regions of the electromagnetic spectrum in order of decreasing wavelength: infrared, ultraviolet, green, blue, red, and x-rays. (long) wavelength frequency energy per photon ) Label the proper ends of the frequency line "high" and "low," and indicate with arrow heads which is the higher end. Atomic Emission Spectra Also label the proper ends of the energy line "high" and "low," again indicating with arrow heads which is the higher end. Color 2. A typical value for the wavelength of violet light is 400.0 nm and a typical value for the wavelength of red light is 700.0 nm. Using these wavelength values, complete the following table: Violet Red Wavelength 400.0 nm 700.0 nm a. UV spectrum b. Visible spectrum c. IR spectrum_ Frequency n=6 n=5 Show calculations for violet light here: 3. According to the Bohr model of the hydrogen atom, the electron can be excited to only certain higher levels above the ground state (n=1). When the excited electron returns home, it gives off energy in the form of radiation. Decide where in the electromagnetic spectrum each of the "return home" trips shown at the right will be. n=4 n=3 n=2 n=1 J/photon A B (short) ) Energy C kJ/mol photons E| F
Transcribed Image Text:1. On the chart below, arrange the following regions of the electromagnetic spectrum in order of decreasing wavelength: infrared, ultraviolet, green, blue, red, and x-rays. (long) wavelength frequency energy per photon ) Label the proper ends of the frequency line "high" and "low," and indicate with arrow heads which is the higher end. Atomic Emission Spectra Also label the proper ends of the energy line "high" and "low," again indicating with arrow heads which is the higher end. Color 2. A typical value for the wavelength of violet light is 400.0 nm and a typical value for the wavelength of red light is 700.0 nm. Using these wavelength values, complete the following table: Violet Red Wavelength 400.0 nm 700.0 nm a. UV spectrum b. Visible spectrum c. IR spectrum_ Frequency n=6 n=5 Show calculations for violet light here: 3. According to the Bohr model of the hydrogen atom, the electron can be excited to only certain higher levels above the ground state (n=1). When the excited electron returns home, it gives off energy in the form of radiation. Decide where in the electromagnetic spectrum each of the "return home" trips shown at the right will be. n=4 n=3 n=2 n=1 J/photon A B (short) ) Energy C kJ/mol photons E| F
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