Week Two Wrap-Up
Module Review
In this module, we continued to learn about atomic orbitals (regions in space where we have a high probability of finding an electron). We began by discussing the results of the Schrödinger Equation and exploring connections between the quantum numbers of an electron. After learning how to define orbitals, we discussed how exciting an electron in an atom can help us understand the connection between wavelength and frequency of light emitted as an electron transitions from a higher energy level to lower energy level in an atom.
We then looked at the different possible shapes (s, p, d, and f) and energies of orbitals in a multi-electron system defined by the Schrödinger Equation and the associated quantum numbers to each orbital. We also learned about the Pauli Exclusion Principle (that no two electrons in an atom can have the same four quantum numbers), which means that each orbital is limited to a maximum of two electrons.
Last, we learned how to put ground state electrons of a multi-electron atom into an orbital diagram, defining their electron configuration and quantum numbers using the Aufbau Principle (helps determine electron configuration order) and the periodic table.
Supplemental Material
If you would like to learn more on this topic, these resources may help:
Quantum Numbers and Atomic Orbitals
Los Alamos National Laboratory
Periodic Table of Elements Links to an external site.
Completion Checklist
Make sure you complete the following learning activities and assessments before moving on to the next topic:
- Lecture Videos
- Example Videos (where posted)
- Practice Problems and Discussion
- Quiz