logging in or signing up hydrogen spectrum 020804 pisgahchemist Download Post to : URL : Related Presentations : Let's Connect Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Copy embed code: Embed: Flash iPad Dynamic Copy Does not support media & animations Automatically changes to Flash or non-Flash embed WordPress Embed Customize Embed URL: Copy Thumbnail: Copy The presentation is successfully added In Your Favorites. Views: 708 Category: Science & Tech.. License: All Rights Reserved Like it (0) Dislike it (0) Added: March 20, 2010 This Presentation is Public Favorites: 0 Presentation Description No description available. Comments Posting comment... Premium member Presentation Transcript Slide 1: Pisgah High School Chemistry Mike Jones The Hydrogen Spectrum Rev 020804 Canton, NC Slide 2: In this experiment you will measure the wavelengths of the lines in the visible portion of the hydrogen spectrum and compare them to the calculated values predicted by the Bohr Model. Slide 3: This is a spectroscope We can use it to measure the wavelengths of the lines in atomic spectra. Slide 4: A high voltage is applied to a narrow tube filled with hydrogen gas and light is produced. Slide 5: Behind the eyepiece is a transmission diffraction grating which separates the light into its components. Slide 6: The spectral lines produced by the the diffraction grating appear superimposed over the scale. Slide 7: The light from the hydrogen discharge tube passes through a narrow slit. Slide 8: The spectral lines appear superimposed over the scale so that their wavelengths can be determined. Slide 9: The wavelength is the number times 10-7 meters. Or the wavelength is the number times 100 nanometers. Slide 10: 2 3 4 5 6 Light from the spectrum tube coming through the slit Measure the wavelength of each line in meters and nanometers. Actual photograph of hydrogen spectrum. - M. Jones 2/5/04 Slide 11: Now you will predict the wavelength of light emitted as the electron moves from a higher energy level to a lower energy level. You will be given the energy level the electron comes from, and the energy level the electron goes to. Slide 12: Use Bohr’s equation to predict the energy of each allowed state. n is the principal quantum number and has values of 1, 2, 3 … 7 Slide 13: Rh is called the Rydberg Constant, Rh has a value of 2.18 x 10-18 J. Slide 14: Next, find the difference between the two allowed energy states. DE = E final – E initial Then, compute the wavelength. Slide 15: Complete a table like the one below. Slide 16: You will now combine your results with the results of other students to compile a list of all of the possible transitions from a higher energy level to a lower energy level, which give off light. A table like the following one will be on the board. Slide 17: …these lower levels These transitions do not result in an emission. Enter the wavelengths in nanometers here. Slide 18: Finally, compare the wavelengths you measured to the wavelengths predicted by the Bohr model. How do they compare? Were all of these lines visible? In what parts of the electromagnetic spectrum do they appear? Slide 19: Do the results of your experiment support the Bohr Model? Why or why not? What additional experiments could you do in order to further test the model? Slide 20: Send questions, comments, and suggestions to: Mike Jones Pisgah High School 1 Black Bear Drive Canton, NC 28716 828-646-3463 firstname.lastname@example.org You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.