Experiment 8 – SpectroscopyName name Lab Section 432Results and DiscussionTable 1. Data Table 1: Wavelength Calibration of SpectroscopeColor of Line Position on Spectroscope Wavelength (nm)Red 6.35 635nmGreen 5.60 560nmYellow 6.00 600nmBlue 5.00 500nmViolet 4.50 450nmTable 2. Data Table 2: Light SourceLight Source Wavelength Range Region(s) of Maximum IntensityCandle 450nm-700nm GreenIncandescent bulb 450nm-700nm GreenBunsen burner 405nm-610nm BlueTable 3. Data Table 3: Atomic Line Spectra of the Balmer Series of Hydrogen(Chemistry the CentralScience 12th Edition)Color ofLinePosition onSpectroscopeCalculated Wavelength(nm)Literature Wavelength(nm)PercentErrorRed 6.80 680nm 656nm 3.65%Blue 5.00 500nm 486nm 2.88%Teal 4.55 455nm 434nm 4.84%Table 4. Data Table 4: Determination of Electron Transitions Color of Line Wavelength Frequency Energy Transition(nm) (Hz) (J)Red 680nm 4.41*1014 Hz 2.92*10-19 J 32Blue 500nm 6.00*1014 Hz 3.98*10-19 J 42Teal 455nm 6.59*1014 Hz 4.37*10-19 J 52Table 5. Data Table 5: Flame Emission SpectraElement Color of Flame Color of Emission Lines Position WavelengthSodium Orange Orange 6.10 610nmCopper Green and blue Green 5.50 550nmLithium Red Red 6.50 650nmIron Orange Orange 6.00 600nmPotassium Peach Orange 6.15 615nmTable 6. Data Table 6: Unknown SubstanceColor of Flame Color of Emission Lines Position WavelengthElements inUnknown MixtureTeal, green, red,orangeRed, yellow, green Red=6.80Yellow=6.00Green=5.50680nm600nm550nmLithium, Copper,SodiumConclusion: This experiment was supposed to show you how to use the spectroscope to compare various continuous emission sources, get the atomic line spectra of light emitted from discharge tubes, and to calculate the photon wavelengths, frequencies, and energies from the line spectra data. This experiment did all of that and we were able to learn about all of those things through the various experiments. Students are able to compare the calculated vs the literature values for the wavelengths which do have some differences. For example, there was a 3.65% error for red, 2.88% error for blue, and 4.84% error for teal. Also, in our results we calculated the frequency and energy for each color using the c=wavelength*v and E=hv. Also, for the most part the calculated wavelengths for each color tends to fall within the range for that color. With Table 5 you also learn what color flame and emission each of the elements have and for the most partthe color of the flame matched the color of the emission lines except for potassium where the color of the flame was peach and the color of the line was orange. Furthermore, we observe different light sources and their wavelengths. It might be surprising that both the candle and light bulb are the same along with the same color and the Bunsen burner however was different in wavelength and color. As the temperature of the solid is raised, more of the radiation is emitted at shorter wavelengths. Also, the unknown substance was the most colorful and consisted of various elements to create the various colors. The results from this experiment appear accurate and we did do what the objectives of the experiment were. They help the students learn more about how to calculate the wavelengths, frequencies, andenergies. It also shows the importance of knowing the wavelengths, frequencies sand energies. In addition,students do learn about the Bohr model of the hydrogen atom and also learn about transitions which is accompanied by emission or absorption of a discrete amount of energy. Also, the wavelengths and colors help us identify different elements. This could also help us identify different chemicals. It helps us understand energy levels better as well. Plus, spectroscopy is used in astronomy and telescopes as well as in other things. An issue that we had with the experiment was that we had issues with the unknown substance. There were two bottles and we were only supposed to have one? Also we aren’t 100% sure on the elements in the unknown substance however we got lithium, copper, and sodium. Furthermore, it was hard at times to see the wavelengths but for the most part it was fine. But overall the experiment taught a lot about the wavelengths, frequencies, and