You will be able to:
explain the wave nature of light (basics of wavelength, frequency, amplitude, spectrum IR through UV, energy/frequency relationships -- qualitative)
explain how light can act as a particle in the photoelectric effect.
describe the observations made in studying the double-slit experiment and photoelectric effect and their impact on atomic theory.
explain emission and absorption spectrums, how they are created, and how they are related
explain the quantum concept
describe the Bohr model of the atom.
explain the relationship between energy levels in an atom and lines in an emission or absorption spectrum.
explain the importance of the de Broglie hypothesis.
state the Heisenberg Uncertainty Principle and relate its significance to the atomic model
explain the key aspects of the Schrödinger model for the atom. How is is similar to and different from the Bohr model?
state the Aufbau Principle, Hund's Rule, and the Pauli Exclusion Principle.
state the energy sublevels within a given energy level.
state the maximum number of electrons that can occupy a given energy level and sublevel.
write an electron configuration in subshell notation and orbital notation. (Note: remember to layer your orbital diagrams by energy as we did in notes and as the example on the slides, not draw them flat like the textbook does.)
determine the element given an electron configuration.
read an electron configuration from the position of the element in the periodic table.
1.
5.1Â Electromagnetic Spectrum
5.4Â Photoelectric Effect
5.5Â Atomic Emission Spectra
2.
5.6Â Bohr's Atomic Model
5.7Â Spectral Lines of Hydrogen
5.9Â Quantum Mechanics
5.10Â Heisenberg Uncertainty Principle
5.11Â Quantum Mechanical Atomic Model
5.12Â Energy Level
5.13Â Orbital
3.
5.16Â Pauli Exclusion Principle
5.17Â Hund's Rule and Orbital Filling Diagrams
5.20Â Noble Gas ConfigurationÂ
Notes
Lab
Homework
For more practice, pick any element. You can check the electron configurations on this page.
This page has orbital diagrams for all of the elements. They are drawn flat, not properly stacked, to save space. These include just noble gas abbreviations.
There are some elements that violate the Aufbau-predicted electron configurations. Honors will need to explain this, CP does not.
Additional Resources
White Light and the Spectrum
Is light a wave?
Or a particle?
More details and math behind the Bohr model of the atom. This is optional, but if you are interested in a deeper dive into atomic theory, the entire playlist (of which this video is the second) is a good introduction at a little higher level than the course.
Aufbau Principle, Hund's Rule, and Pauli Exclusion Principle in Orbital Diagrams
More examples of Aufbau Principle, Hund's Rule, and Pauli Exclusion Principle in Orbital Diagrams
Reading Electron Configurations from the Periodic Table
Including noble gas abbreviations