To determine if a complete photoelectron spectrum for an element is consistent with the atomic model of that element, the following observations provide evidence:
- The spectrum should show distinct peaks corresponding to electrons in different atomic subshells or orbitals. Each peak represents electrons with a specific binding energy, reflecting their energy level and subshell (e.g., 1s, 2s, 2p, etc.) as predicted by the quantum mechanical atomic model
- The relative heights of the peaks should correspond to the number of electrons in each subshell. For example, a peak for a subshell with more electrons will have a greater intensity, consistent with electron count in atomic orbitals
- The binding energies should increase for electrons closer to the nucleus, reflecting stronger nuclear attraction and higher ionization energy for inner-shell electrons. This aligns with Coulomb’s law and the quantum model of electron shells and subshells
- The spectrum should display energy spacing and splitting consistent with known subshell structures and electron configurations of the element, supporting the existence of subshells and the quantum mechanical model rather than the simpler Bohr model
- The presence of fine structure or vibrational sublevels in molecular cases further supports the detailed quantum mechanical description of electron states
In summary, evidence that the spectrum matches the atomic model includes distinct, quantized peaks at binding energies corresponding to known subshells, peak intensities matching electron counts, and energy ordering consistent with nuclear attraction and electron configuration theory
