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Chapter 2
Periodicity and the Electronic Structure of Atoms
2.10–2.13, 3.3
Electromagnetic radiation
The photoelectric effect
Atomic orbitals and quantum numbers
Atomic line spectra
Multielectron atoms and electron configurations
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
Electromagnetic radiation
Electromagnetic spectrum
Wavelength ()
Frequency ()
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
Balmer-Rydberg equation: