please answer these 2 questions in detail. thank you
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Untitled.sp 2022-01-07 11:37 Source #1 78 ms Analyze Light Integration Time Number of Scans to Average Smoothing 10 0 Intensity Source 1 vs Wavelength (nm) 100 0 30 will 05 Intensity Source 5 30 20 10 100 200 8 100 400 600 700 3 300 01 San Wavelength 1) Specify the orbital transitions for the electron in the hydrogen atom for the Balmer series that was recorded in this experiment. The Balmer series are electron transitions from a p orbital to a 2s orbital. To determine the He transitions that correspond to the (known) H transitions, begin by tabulating your results in Excel using the following format (be sure to include all He spectral lines). In the cross cells calculate the energy differences (in eV) between the hydrogen and helium atoms (eq. 1), 2) 3 661 4 491 5 438 6 412 Hydrogen (n) Hydrogen Balmer Series (n=2) Wavelengths (nm) Helium 781 Wavelengths (nm) 710 1 1 1 = 1240 () D2 1 etc. 1 = 1240 B3 1 = 1240 B4 1 = 1240 B5 C2 1 671 02 618 etc. Experiment #1 ATOMIC SPECTROSCOPY Objective/Learner Outcome To demonstrate quantization of energy levels, to observe and explain the difference in electronic configurations between one-electron (hydrogen) and multi-electron (helium) atoms. Introduction Atomic spectroscopy is the study of emission or absorption of energy when an electron undergoes a change in energy level within its atom. These emission/absorption processes produce a line spectrum with each line corresponding to a difference in energy between two atomic energy levels involved in the transition. Selection rules determine allowable electronic transitions between atomic energy levels and are often visualized via a Grotrian diagram (see Fig. 8C.1 of your textbook for the Grotrian diagram of hydrogen). Atomic spectra become increasingly complex as the number of electrons (and atomic number) increase. For instance, when an electron of helium is promoted from the ground state the electrons no longer occupy the same orbital. This generates an open-shell configuration where the electrons can have spins being parallel (triplet) or antiparallel (singlet). Although more complicated than hydrogen, helium can be simplified compared to larger atoms in two ways: (1) Only one electron can be excited as the energy required to excite the second electron exceeds the ionization energy of helium (.e. He would form instead of a doubly excited atom) and, (2) the spin of the excited electron does not change during a transition. Therefore, transitions will only occur from singlet to singlet (including the ground state), and triplet to triplet (see Fig. 8C.3 of your textbook). In this experiment, the line spectra for hydrogen and helium will be observed and recorded. A spectrophotometer will record peaks at the energies (wavelengths) at which the transitions occur, and you will assign electronic transitions to those peaks. An exact (unambiguous) analysis can be done on the Hatom, knowing that visible light gives rise to a specific series in the line spectrum (in this context, a "series refers to transitions involving a common low-energy orbital). Comparing the helium spectrum to that of hydrogen will allow the electronic transitions associated with helium to be assigned. This will be done by calculating (eq. 1) the energy differences between the transitions associated with hydrogen and helium atoms. SE = hc Cute ) = 1240 GA (1) In eq. 1 his Planck's constant, cis the speed of light in a vacuum, and he and I are the wavelengths corresponding to the peaks from the data collected for the helium and hydrogen atoms respectively. = Alle nm 1 Procedure Spectrum tubes heat up with use. Care should be taken not to touch the hot tube. - we Emission Spectra of Hydrogen and Helium Insert the hydrogen spectrum tube into the provided power supply and turn the power on. While the tube is warming up insert the lead of the spectrophotometer fiber optic cable assembly into the holder attached to the power supply. Position the lead such that its tip is centered and as close to the bulb, without touching, as possible. Tighten to secure. Begin data acquisition by selecting the red record button found in the Tight path bottom left corner of the PASCO Spectrometry App. Place the cuvette end of the fiber optic cable assembly into the cuvette holder of the PASCO spectrometer ensuring the emitted light PASCO follows the light path. Adjust the position of the cuvette to SPECTROMETER achieve maximum emission intensity. Select AUTOSET (under Integration Time) to obtain the emission spectrum with the best signal to noise ratio. Stop data recording and select the share icon to export the data in.csv format. To aid peak identification, scroll through the reference spectra, found at the bottom of the app, until the hydrogen spectrum is selected. Use the coordinate tool to identify the experimental peaks most closely associated with the reference peaks. You'll notice one of the expected hydrogen peaks is not Data acquisition 350 400 450 500 550 600 650 700 750 800 850 900 9501000 Coordinate tool Wavelength (mm) Reference spectrum Reference None PASCO observable at this integration set point. To obtain this peak, restart data recording and manually set the integration time to 1000. Once the single has stabilized, stop recording and identify the wavelength of the missing peak. Remove the lead of the fiber optic cable assembly from the holder. Replace the hydrogen spectrum tube with the available helium tube. Insert the fiber optic lead as before and collect the emission spectrum of helium using the AUTOSET integration. As all peaks should be resolved at these settings, there is no need to run a scan at maximum integration time. Export the data as a .csv. As with the hydrogen spectrum, select the helium reference spectrum and identify the experimental peaks most closely related to the reference peaks. Report When analyzing the data, we assume one of the electrons of the hellium atom fully screens the other from feeling the effects of the nucleus. Therefore, as hydrogen and helium have the same ground state orbitals (is), the energy difference for orbital transitions of the open-shell singlet type for each atom would be the same 2
