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Because a sample of hydrogen contains a large number of atoms, the intensity of the various lines in a line spectrum depends on the number of atoms in each excited state. At the temperature in the gas discharge tube, more atoms are in the n = 3 than the n ≥ 4 levels.
1. Determine the wavelength, frequency, and energy of the bright lines for the spectrum of several nonmetal, gaseous elements. 2. Use the activity data and observations to justify Bohr’s atomic model. Next Generation Science Standards* (NGSS) PE HS-PS4-1. Use mathematical representations to support a claim regarding relationships
The brightline spectrum for each element is unique and can be used to identify that element. In this lab you will observe and sketch emission spectra for several known elements.
The charts will be used to draw your observed bright line spectra and the tables will be used to write in your answers for the multiple sets of calculations of wavelength, frequency, and energy of photons.
The discrete energies (lines) in the spectra of the elements result from quantized electronic energies. Of these features, the most important is the postulate of quantized energy levels for an electron in an atom.
Bright Line Spectra of various elements. This work is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License.
23 Σεπ 2024 · Determine the wavelength, frequency, and energy of the bright lines for the spectrum of several nonmetal, gaseous elements. Use the activity data and observations to justify Bohr’s atomic model.
