Practice Evidence For The Quantized Electronic Energy Levels: Atomic Spectra (2.3.3)

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6 sample questions

Question 1.
What is an emission spectrum?
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Think of it as the light released by excited atoms.
Question 2.
Name the series of lines in hydrogen's emission spectrum that fall into the visible range.
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This series includes transitions to n=2.
3Question 3.
What is the relationship between energy levels and atomic spectra?
- Energy levels are continuous
- Energy levels are quantized
- Energy levels do not exist
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Consider the distinct lines seen in the spectra.
4Question 4.
True or False: The emission spectrum of an element is the same as its absorption spectrum.
- True
- False
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Think about what happens during absorption versus emission.
Question 5.
Calculate the wavelength of light emitted when an electron in hydrogen transitions from n=3 to n=2.
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Remember to use the relationship between energy and wavelength.
Question 6.
Discuss the implications of unique atomic spectra for chemical analysis.
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Reflect on how spectroscopy assists in understanding the universe.

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