Prelab2 - Lab Instructor: ______________________ Lab...

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Name: _____________________________ Date: _________________________________ Lab Instructor: ______________________ Lab Section: ___________________________ 57 EXPERIMENT 2 Optical Spectroscopy Prelaboratory Questions: 1. Explain the difference between continuous and line spectra. 2. Explain the difference between absorption and emission spectra. 3. For an atom with the energy levels below what wavelength light (in nm) will be emitted in a transition between E 2 and E 1 (indicated by the down arrow below)? What wavelength of light must be absorbed to cause a transition between E 3 and E 5 (indicated by the up arrow below)? E 5 = -8.0 kJ/mol E 4 = -17.0 kJ/mol E 3 = -39.5 kJ/mol E 2 = -200.0 kJ/mol E 1 = -1100.0 kJ/mol
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Unformatted text preview: Lab Instructor: ______________________ Lab Section: ___________________________ 58 4. Can the atom of Question 3 absorb or emit light with a wavelength of 555 nm? Can it absorb or emit light with a wavelength of 5320 nm? If so, state which energy levels the transition occurs between. 5. Consider the emission spectra of the two hypothetical elements X and Z. Emission spectrum of X 1.7 1.8 1.9 2.0 2.2 2.4 2.6 2.8 3.0 3.2 3.4 eV 700 600 500 400 nm Emission spectrum of Z 1.7 1.8 1.9 2.0 2.2 2.4 2.6 2.8 3.0 3.2 3.4 eV 700 600 500 400 nm Draw a picture of the emission spectra expected from a sample containing a mixture of X and Z on the spectrum blank below. Emission spectrum of a mixture of X and Z 1.7 1.8 1.9 2.0 2.2 2.4 2.6 2.8 3.0 3.2 3.4 eV 700 600 500 400 nm...
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This note was uploaded on 03/15/2011 for the course CHEM 211 taught by Professor Crane, b during the Fall '06 term at Cornell University (Engineering School).

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Prelab2 - Lab Instructor: ______________________ Lab...

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