Week Three: Periodic Trends

 Module Overview

Once we understand the electronic structure, we will be able determine how the periodic table can be used to compare the elements according to atomic size and various energies. We will conclude by seeing how these trends can be used to predict chemical properties of the elements.

 Learning Objectives

After completing this module, you will be able to:

  1. To recognize the connection between the electron configuration on an atom and the location of the atom on the periodic table.
  2. To predict the charge of a stable ion formed for any representative element and write the ground state electron configuration of any monoatomic ion.
  3. To develop the working understanding of effective nuclear charge and its role in predicting the periodic trends of atomic and ionic radii.
  4. To explain what ionization energy is and the role that electron configurations and effective nuclear charges have on the magnitude of the ionization energy.
  5. To describe what electron affinity is and the basic periodic trends.
  6. To discuss how electron configurations, ionization energy and electron affinity affect the reactivity of the representative elements.

 Lecture Notes

Please download the unit's Download presentation guide

. This guide can be printed to use for notes and/or reviewed before the unit assessment.

 Due This Week

Assignment Format Grading
3.01 Navigating the Periodic Table Practice Problems Self-evaluation PDF 0 pts.
3.02 Monoatomic Ions and Electron Configuration Practice Problems Self-evaluation PDF 0 pts.
3.03 Effective Nuclear Charge and Atomic and Ionic Radii Practice Problems Self-evaluation PDF 0 pts.
3.04 Ionization Energy Practice Problems Self-evaluation PDF 0 pts.
3.05 Electron Affinity Practice Problems Self-evaluation PDF 0 pts.
3.06 Properties of Representative Elements Practice Problems Self-evaluation PDF 0 pts.
Quiz 3: Periodic Trends Quiz 10 pts.