CHEM 1215 Experiment 2 Summer 2022 (b) From your spectra above, write down the emission wavelengths (i.e. the peak wavel

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Chem 1215 Experiment 2 Summer 2022 B From Your Spectra Above Write Down The Emission Wavelengths I E The Peak Wavel 1 (51.2 KiB) Viewed 33 times

CHEM 1215 Experiment 2 Summer 2022 (b) From your spectra above, write down the emission wavelengths (i.e. the peak wavelength(s)) for each sample. Note: There may be only one OR multiple peaks. Include all of them. i. NaCl 589.0 ii. CaCl₂ 24.8 Hi. CUCB769,6 iv. KCI 769.6 v. FeCl, 767 and 682.5 (c) The Bohr Model was used in Part A to predict the emission wavelengths of hydrogen, which only as Is electrons in its ground state. When hydrogen is excited and electrons fall back down toward the nucleus, it can emit photons. For hydrogen, Eqn. 2.1 is excellent at predicting the energy difference between these shells and therefore the emission wavelengths for the first element (atomic number Z = 1). However, we mentioned that the equation begins to fail for elements larger than helium. A lithim cation Li", which is the species you tested in LiCI, has an atomic number Z=3 and is somewhat similar in size to helium. In order to use Eqn. 2.1 for elements other than hydrogen, the atomic number must be added to the equation as shown in Eqn. 2.6. 1 AE-2.18x10-18 J (2.6) final initial For the LiCl peaks observed, complete the observed wavelength and energy in the table below. Then, apply Eqn. 2.6 to determine the likely initial and nfinal, based on the calculated energy. Table 2.3: Lit Emission Spectra Observed Wavelength Observed Energy Calculated Energy Determined Determined (nm) J J Britial nfinal (d) Based on Table 2.3, in 2-3 sentences describe whether the the Bohr Model applies to a larger element, such as Li*. Quantiatively support your assertion. 24