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Workshop 6: Introduction to Spectroscopy Part I: Interpreting Visible Emission Spectra Street lights in many communities are still using sodium vapor lamps. These lamps have an orange yellow tint. The visible emission spectrum for sodium shows two very close yellow bands (lines) that have wavelengths of about 590 nm. This explains why the light produced from sodium vapor lamps would appear yellow and not white. In comparison, mercury vapor lamps produce a blue colored light due to an intense light emission from the mercury atoms in the visible part of the electromagnetic (EM) spectrum. This line has a wavelength of 434 nm. a) Without doing any math, compare the wavelengths of the photon emitted from these two elements in the visible part of the spectrum. Which element would you expect to produce higher energy photons in the visible part of the spectrum? Discuss this with your group. Write your answer here and briefly explain your reasoning. b) Calculate the energy of the photon emitted by each element in the visible part of the spectrum. Does your answer make sense given your initial expectation? c) In class you have learned that the light emissions from atoms are due to specific electron movements between available energy levels. Would you expect that the size of the atom (the atom's radius) might also undergo changes as the atom releases photons with a specific energy? Discuss this with your group and write the answer below. Justify your answer.

Workshop 6: Introduction to Spectroscopy Part I: Interpreting Visible Emission Spectra Street lights in many communities are still using sodium vapor lamps. These lamps have an orange yellow tint. The visible emission spectrum for sodium shows two very close yellow bands (lines) that have wavelengths of about 590 nm. This explains why the light produced from sodium vapor lamps would appear yellow and not white. In comparison, mercury vapor lamps produce a blue colored light due to an intense light emission from the mercury atoms in the visible part of the electromagnetic (EM) spectrum. This line has a wavelength of 434 nm. a) Without doing any math, compare the wavelengths of the photon emitted from these two elements in the visible part of the spectrum. Which element would you expect to produce higher energy photons in the visible part of the spectrum? Discuss this with your group. Write your answer here and briefly explain your reasoning. b) Calculate the energy of the photon emitted by each element in the visible part of the spectrum. Does your answer make sense given your initial expectation? c) In class you have learned that the light emissions from atoms are due to specific electron movements between available energy levels. Would you expect that the size of the atom (the atom's radius) might also undergo changes as the atom releases photons with a specific energy? Discuss this with your group and write the answer below. Justify your answer.

Chemistry for Engineering Students
Chemistry for Engineering Students
3rd Edition
ISBN:9781285199023
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter6: The Periodic Table And Atomic Structure
Section: Chapter Questions
Problem 6.78PAE
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Workshop 6: Introduction to Spectroscopy Part I: Interpreting Visible Emission Spectra Street lights in many communities are still using sodium vapor lamps. These lamps have an orange yellow tint. The visible emission spectrum for sodium shows two very close yellow bands (lines) that have wavelengths of about 590 nm. This explains why the light produced from sodium vapor lamps would appear yellow and not white. In comparison, mercury vapor lamps produce a blue colored light due to an intense light emission from the mercury atoms in the visible part of the electromagnetic (EM) spectrum. This line has a wavelength of 434 nm. a) Without doing any math, compare the wavelengths of the photon emitted from these two elements in the visible part of the spectrum. Which element would you expect to produce higher energy photons in the visible part of the spectrum? Discuss this with your group. Write your answer here and briefly explain your reasoning. b) Calculate the energy of the photon emitted by each element in the visible part of the spectrum. Does your answer make sense given your initial expectation? c) In class you have learned that the light emissions from atoms are due to specific electron movements between available energy levels. Would you expect that the size of the atom (the atom's radius) might also undergo changes as the atom releases photons with a specific energy? Discuss this with your group and write the answer below. Justify your answer.
Transcribed Image Text:Workshop 6: Introduction to Spectroscopy Part I: Interpreting Visible Emission Spectra Street lights in many communities are still using sodium vapor lamps. These lamps have an orange yellow tint. The visible emission spectrum for sodium shows two very close yellow bands (lines) that have wavelengths of about 590 nm. This explains why the light produced from sodium vapor lamps would appear yellow and not white. In comparison, mercury vapor lamps produce a blue colored light due to an intense light emission from the mercury atoms in the visible part of the electromagnetic (EM) spectrum. This line has a wavelength of 434 nm. a) Without doing any math, compare the wavelengths of the photon emitted from these two elements in the visible part of the spectrum. Which element would you expect to produce higher energy photons in the visible part of the spectrum? Discuss this with your group. Write your answer here and briefly explain your reasoning. b) Calculate the energy of the photon emitted by each element in the visible part of the spectrum. Does your answer make sense given your initial expectation? c) In class you have learned that the light emissions from atoms are due to specific electron movements between available energy levels. Would you expect that the size of the atom (the atom's radius) might also undergo changes as the atom releases photons with a specific energy? Discuss this with your group and write the answer below. Justify your answer.
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