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Understanding Photoelectron Spectroscopy in Quantum Theory

Photoelectron Spectroscopy (PES) provides insights into shells and orbitals in quantum theory. It explains the photoelectric effect using energized photons to remove electrons from atoms. PES examines the energy required to dislodge electrons. By exposing atoms to X-rays, electrons are ejected, allowing a closer look at binding energy. The Photoelectron Spectrometer analyzes differences between photon energy and electron kinetic energy, showcasing binding energy in a spectrum.

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Understanding Photoelectron Spectroscopy in Quantum Theory

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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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