Ionic Bonding Lab Activity
This lab activity will consist of two different approaches to understanding ionic bonding and consist of three parts.
Part 1 will require your knowledge of the periodic table and electron configurations. Part 2 will use a coloring
activity to reinforce the definitions of metals and nonmetals and how electrons are transferred between these
categories of elements to create stable positive and negative ions. Part 3 will be a wrap up section to assess your
understanding of ionic bonds.
This is a collaborative lab activity. This means each lab group (based on the seating chart) will submit one copy to
be graded and all partners will receive the same grade. This is not an exploratory lab, your answers must be
correct, filled with detail and complete to receive full credit on a response.
Part 1 – Periodic Table and Electron Configuration
For each of the atoms below:
 Shade the box containing the symbol of each element with a difference colored pencil. This color will be
used in part 2 of the lab activity.
 Indicate the group of family number using the CAS system
 Write the electron configuration of the element (Use the Nobel Gas shortcut where appropriate)
 Circle the valence shell of each electron configuration
 Record the number of valence electrons
 Write the Lewis Dot Structure for each element
Element – Color
coded for part 2
CAS Group
Number
Electron Configuration
Number of
Valence Electrons
Lewis Dot Strucutre
Lithium
Aluminum
Oxygen
Nitrogen
Calcium
Chlorine
Part 2 – Coloring Activity
In this part of the activity, you will show the transfer of electrons from the metal to the nonmetal.
 Write the symbol of the element in the Lewis Dot Model that has the correct number of valence electrons
 Color the entire model, including the electrons – use the color assigned in part 1
 Color a second set of models, use scissors to remove the valence electrons from the metal creating a cation
 Use tape to attach the electrons to the nonmetal creating the anion
Your final answer must show:
 Model of the neutral atoms
 Model of the cation, with the correct charge
 Model of the anion, with the correct charge
 The electrons must be color coded the same color as the element of their origin
 The final compound must show the correct amount of each ion in the a single formula unit
 Write the chemical formula for the compound, under the name of the compound
Example:
Using the example as your guide – each member of the group should devote their energy to completing two
different compounds. When all members have finished, take turns explaining your logic to the group.
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Compound #1 – Aluminum + Nitrogen  Aluminum nitride
Compound #2 – Aluminum + Oxygen  Aluminum Oxide
Compound #3 – Calcium + Chlorine  Calcium chloride
Compound #4 – Lithium + Nitrogen  Lithium nitride
Compound #5 – Calcium + Nitrogen  Calcium nitride
Compound #6 – Calcium + Oxygen  Calcium oxide
Compound #7 – Magnesium + Fluorine  Magnesium fluoride
Compound #8 – Potassium + Sulfur  Potassium sulfide
Part 3 – Conclusion Section
These questions are to be discussed as a group and then response written together representing the best and most
complete answer the group can propose based on video notes, class activities and this lab activity.
Relate the number of valence electrons to the position of an element on the periodic table. Give one example NOT
used in this lab to illustrate your idea.
Which categories of elements form ionic bonds? Briefly explain your reasoning.
What is the octet rule? Relate the octet rule to the formation of ionic bonds. To receive full credit for your answer
you must address the octet role as it relates to both ions in the compound. Illustrate your reasoning with an
example that was NOT used in this lab.
How does the total positive change compare to the total negative charge in a stable ionic compound? Briefly
explain your reasoning. Illustrate your reasoning with an example that was NOT used in this lab.