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Photoelectron Spectroscopy (PES)

Photoelectron Spectroscopy (PES). PES. Provides explanation for shells and orbitals in quantum theory Photoelectric effect — Utilization of photons to remove electrons from atoms Photons have been energized, analyzing the energy needed to remove electrons from an atom/compound

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Photoelectron Spectroscopy (PES)

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  1. Photoelectron Spectroscopy (PES)

  2. PES • Provides explanation for shells and orbitals in quantum theory • Photoelectric effect— • Utilization of photons to remove electrons from atoms • Photons have been energized, analyzing the energy needed to remove electrons from an atom/compound • PES in detail: • Atoms exposed to X-rays • Electrons removed from atom due to photon

  3. Photoelectron Spectrometer Looks at difference between photon energy source and kinetic energy from removed electrons (binding/ionization energy) Spectrum shows binding energy vs. relative intensity

  4. Photoelectric Spectrum • Photoelectric spectrum— • Graphical representation of binding energy vs. number of electrons • Energy on x-axis • Number of electrons in a subshell on y axis 1) Peaks— • Number of subshells/orbitals • 2) Peak heights— • Number of electrons in subshell

  5. Photoelectric Spectrum • Energy shells represent how close electrons are to nucleus • Shells with high energies indicate electrons close to nucleus • Electrons within the same subshell have similar energy values but different orbital energies

  6. Example : • A third period element in the periodic table forms a PES spectrum with three peaks, in the ratio 2:2:1. Name this element. • Aluminum • Boron • Carbon • Sodium

  7. Example : • Aluminum has the following electron configuration: 1s22s22p63s23p1 • How many peaks should be expected in a PES spectrum for Al? • Which electrons will show the highest energies? Why?

  8. Example: (cont.) • Aluminum has the following electron configuration: 1s22s22p63s23p1 C) Which peak on the spectrum will be the most intense/largest? Why? D) Explain why the peaks for the 3s and 3p electrons would be closely grouped and why they are different than electrons in the 2s and 2p orbitals.

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