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Atoms of individual elements emit light at only specific wavelengths, producing a line spectrum rather than the continuous spectrum of all wavelengths produced by a hot object. Niels Bohr explained the line spectrum of the hydrogen atom by assuming that the electron moved in circular orbits and that orbits with only certain radii were allowed.
ΔE = hf. Only certain frequency lines are present in the spectrum as only certain high to low energy level transitions are possible within the atom. The emitted light are analyzed with a spectrometer and discrete bright lines in a dark background are observed.
The line spectrum is like a fingerprint and is specific for each element. If you have ever let food boil over when cooking, you will notice the gas flame will turn a bright yellow-orange. This is due to the electrons in the sodium atoms gaining energy and then emitting the energy as yellow light.
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.
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.
3 Σεπ 2009 · This handbook is designed to provide a selection of the most important and frequently used atomic spectroscopic data in an easily accessible format. The compilation includes data for the neutral and singly-ionized atoms of all elements hydrogen through einsteinium (Z = 1-99). The wavelengths, intensities, and spectrum assignments are given in a ...
For Higher Physics, revise emission or absorption of certain frequencies of light from the elements and atomic line spectra.
