Atomic Spectra Lab report

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Marquette University *

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1001

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Chemistry

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Feb 20, 2024

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Uploaded by CommodoreFangAlbatross43

CHEM 1001 Atomic Spectra Laboratory Report NAME : Liam Cedeno Agosto DATE : 2/15 SECTION : 403 TA : Audrey Vice A. Goals/Purpose of Experiment ( 2 Points, ~50 words ) : The goal of this experiment was to be able to understand atomic energy levels and relate change in wavelengths or absorbed omitted protons to the understanding of quantum numbers. As well as analyze and understand the spectra of different elements using qualitative and quantitative tools. B. Theory/Introduction ( 6 Points, ~100 words ) : everyday examples of something called emission- which is when elements release different colored photons and emit light as a result of being excited- are fireworks and neon signs. These lights consist of many colors, even if to our naked eye there only seems to be one or two. We can see at a microscopic level these different colored lines, or spectra of different elements through tools like a spectroscope, or just try to see one or two of the colors with our naked eye. C. Procedure summary ( 5 Points, ~100 words ) : there were three parts to this experiment. Part one consisted of mostly calculations. We were given three equations with constants that we were to use to find energy in joules using quantum numbers, delta E of transmission and wavelength using upper and lower quantum numbers, then compare our calculated wavelengths to the ones in the emission spectra. For part two we had to use a spectrum tube carousel or spectroscope to determine the number of lines and its colors of different gasses. And for part three we were so watch different metals react with fire and annotate the color or length of the flame D. Results and Calculations: ( 12 Points ) : My results for part one were closely accurate, my calculated wavelengths were all a few decimals or around two integers off from the experimented wavelengths. For part two I was somewhat able to see some of the colored

lines, but possibly weren ’ t fully accurate. And part three was solely based on observation of the naked eye, so those were accurate as well. Part 1: Spectrum of the hydrogen atom Use the figure below to fill Table 1 and Table 2 below Table 1 : title Quantum Number (n) Calculated energy in J (Use Eq 1 of the handout) A 1 -2.18 x 10^-18 B 2 -5.45 x 10^-19 C 3 -2.42 x 10^-19 D 4 -1.36 x 10^-19 E 5 -8.72 x 10^-20 F 6 -6.05 x 10^-2- Table 2 : title

Transition ΔE of Transition (Use Eq 2 of the handout or calculate the difference between two energy levels in Table 1 above) Calculated Wavelength in nm (Use Eq 3 of handout and convert the wavelength in nm) Closest observed experimental wavelength (Figure 3 handout) n upper (Table 1 template) n lower (Table 1 template) K -3. 027 X 10^-19 J 659.92 nm 659.62 nm 3 2 L -4.087 X 10^-19 J 485.87 nm 485.07 nm 4 2 M -4.578 X 10^-19 J 433.8 nm 435.12 nm 5 2 N -4.844 x 10^-19 J 409.95 nm 411.38 nm 6 2 Demonstrate calculations for any one energy and wavelength observed in Part 1: Part 2: Line spectrum of various gases Observe lines and colors produced by various elements, using a handheld spectroscope. Table Title: Gas Number of lines Write ‘m’ if more than 8 lines are present Color of observed lines (Broadly indicate the color bands if more than 8 lines are present) Neon 5 Orange, green, purple, yellow, blue Hydrogen 4 Orange, purple, yellow, blue Helium 4 green, purple, yellow, blue Argon 5 Orange, green, purple, yellow, blue Part 3: Flame test of metal ion solutions Observe the color of a metal ion solution ignited by a Bunsen burner.

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