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Chapter 2 Periodicity and the Electronic Structure of Atoms CHAPTER READING Section 2.1 2.3 2.6–2.8 2.9 2.10–2.13, 3.3 Topic Electromagnetic radiation The photoelectric effect Atomic orbitals and quantum numbers Atomic line spectra Multielectron atoms and electron configurations LEARNING OBJECTIVES 1. Understand how electromagnetic radiation is characterized by its wavelength, frequency and energy and be able to convert between them. 2. Be able to explain the data observed in the photoelectric effect, including: a. The threshold frequency b. The correlation between radiant intensity and the number of emitted electrons 3. Understand that the electrons of an atom behave as waves, resulting in quantum numbers 4. Know all four quantum numbers (n, l, ml, ms), and the dependency rules between them 5. Be able to use the Balmer-Rydberg equation to relate orbital energy levels to the properties of the interacting photon 6. Understand how Coulomb’s law contributes to electron energy levels via: a. Electron-nucleus attraction b. Electron-electron repulsion 7. Know the order of how electrons fill into atomic orbitals in multielectron atoms based on orbital energy and Hund’s rule 8. Be able to write electron configurations of atoms and ions located in the first four periods (rows) of the periodic table 9. Distinguish between core electrons and valence electrons GLOSSARY Electromagnetic radiation Electromagnetic spectrum Wavelength () Frequency () Photon Node Planck’s Constant (h) The speed of light (c) Principal quantum number (n) Angular-momentum quantum number (l) Magnetic quantum number (ml) Spin quantum number (ms) Orbital shell Orbital subshell Pauli Exclusion Principle Orbital energy level Aufbau order Core electron Valence electron MAJOR EQUATIONS AND CONSTANTS ⁄ Balmer-Rydberg equation: [ ]