Practice Experimental Observation Of Atomic Spectra (3.3) - Unit 2: Atomic Structure

Practice: Experimental Observation of Atomic Spectra

Lesson 3.3Unit 2: Atomic Structure

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9 questions

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Quiz
3 questions · about 2 min · pass mark 70%. Hints available.
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6 sample questions

Question 1.
What is an emission spectrum?
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Think about what happens when atoms release light.
Question 2.
Name one element and its characteristic flame color in a flame test.
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Recall the example we discussed in class.
3Question 3.
What is the difference between emission and absorption spectra?
- Emission spectra show emitted light while absorption spectra show light that is absorbed.
- Emission spectra show absorbed light while absorption spectra show emitted light.
- There is no difference
- they are the same.
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Think about how each type of spectrum is produced.
4Question 4.
True or False: The flame color of an element can be used to identify that element.
- True
- False
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Recall our discussion about flame tests.
Question 5.
Explain how the Rydberg formula can be used to predict the wavelengths of spectral lines in hydrogen and provide an example of its application.
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Consider how the values of n affect the resulting wavelength.
Question 6.
Using knowledge of the Stark Effect, discuss how external electric fields could manipulate atomic spectra and what that implies for real-world applications.
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Think about how real-world electric fields might impact photon energies.

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