CHEM I, Discussion 4-1 Atomic Spectra & the Bohr Model

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Presentation transcript:

CHEM I, Discussion 4-1 Atomic Spectra & the Bohr Model Name_____________________ Minitopic 4-1 Atomic Spectra & the Bohr Model

Minitopic 4-1: Atomic Spectra and the Bohr Model 1. How does the emission spectrum relate to the energy levels of Bohr’s atomic model? 2. How can we explain visible light and how it relates to the electromagnetic spectrum? 3. What is the relationship between wavelength and frequency? 4. How do we relate light to energy? 5. How does a spectrophotometer measure the wavelength of light absorbed by a solution?

1. How does the emission spectrum relate to the energy levels of Bohr’s atomic model?

1. How does the emission spectrum relate to the energy levels of Bohr’s atomic model? High E n=6 n=5 n=4 n=3 n=2 Low E n=1 (ground state) (nucleus)

1. How does the emission spectrum relate to the energy levels of Bohr’s atomic model?

2. How can we explain visible light and how it relates to the electromagnetic spectrum?

3. What is the relationship between wavelength and frequency?

3. What is the relationship between wavelength and frequency?

Example 1: What is the frequency of red light with a wavelength of 7 Example 1: What is the frequency of red light with a wavelength of 7.00 x 10-7m?

Example 2: What is the wavelength of a photon of light with a frequency of 8.1 x 1014 s-1?

4. How do we relate light to energy?

Example 3: What is the energy of a photon of violet light whose frequency is 8.90 x 1014s-1?

Example 4: What is the energy of a photon of orange light whose wavelength is 6.00 x 10-7m?

5. How does a spectrophotometer measure the wavelength of light ABSORBED by a solution?

5. How does a spectrophotometer measure the wavelength of light ABSORBED by a solution?

5. How does a spectrophotometer measure the wavelength of light ABSORBED by a solution?