Lab 5 Emission Spectroscopy

Lab 5 Emission Spectroscopy - Emission Spectroscopy- Lab 5...

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Emission Spectroscopy- Lab 5 Author: Holly Polk Lab Partners: Jim Hernandez, Vanessa Jordan, and Dominic Pisciotta Instructor: Yisheng Xu Chemistry Lab 151, Section 001 Date Work Performed: February 25, 2008 Date Report Submitted: February 25, 2008 Abstract: In this experiment, line emission wavelength spectrums for Helium, Hydrogen, several metal cations, and sparklers were recorded. The helium wavelengths were used to calibrate the spectrometer, and the Hydrogen wavelengths were used to evaluate the accuracy of the Rydberg equation. In an evalution of theoretical versus observed experimental wavelengths, helium had a 1.04 % for an average relative deviation of wavelength (nm). Hydrogen had a 1.68 % average relative deviation of wavelength (nm) in a comparison of observed wavelengths to wavelengths calculated by the Rydberg equation. The metal cation wavelengths observed in the green sparkler were Copper (II) Chloride, Barium, Borate and Na+, and there was Li++ in the yellow/gold sparkler.
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Introduction This experiment uses the OOI spectrometer to view various light sources in order to record a line emission wavelength spectrum for each light source. In order to do so, one must point an optical cable at the light source, and then adjust the integration time control to see the spectrum on the screen. Spectrums and wattage values are then saved and studied. In this lab, helium emission lines in the visible spectrum will be identified and used to calibrate the spectrometer. Hydrogen emission line wavelengths in the visible region will also be identified. Flame emission spectroscopy will also be used in the lab to identify the characteristic emissions of metal ion salts and to identify the metal ions responsible for the color of sparklers. All elements have a unique spectra because of their chemical structure. The energy of the photon may be found with the equation E=hc/ λ . E is the energy of the photon, λ is its wavelength, h is the Planck constant (6.62607 x 10 -34 J*s) and C is the speed of light (2.99792 x 10 8 M/s). The shorter the wavelength, the higher the energy of the photon because the energy of the photon is inversely related to its wavelength. The energy of photons determines the effect of the photon when it interacts with matter. Bohr’s theory is a major component in the background of the experiment. In the Bohr model of the hydrogen atom the negatively charged electron confined to an atomic shell encircles a small positively charged atomic nucleus, and an electron jump between orbits will emit an absorbed amount of electromagnetic energy hν. Rydberg’s equation is used with the Bohr model to describe the energies of transitions or quantum jumps between one orbital energy level, and another. Another equation used throughout this lab is the Rydberg equation which is used
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This note was uploaded on 12/08/2009 for the course CHEM 151 taught by Professor Staff during the Fall '08 term at University of Arizona- Tucson.

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Lab 5 Emission Spectroscopy - Emission Spectroscopy- Lab 5...

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