Electron Configuration “Lab”
You will explore how electron configurations vary around the periodic table. You will
compare this data to reactivity information to examine any relationships between electron
configurations and reactions.
Your Task:
Part One: You will complete electron configurations for a number of elements and then
compare them to each other in an attempt to discover any patterns.
Part Two: You will compare electron configurations to reactions to discover any patterns.
Pre-Lab Requirements:
None
Notes about the “Original Data Sheet”:
For this lab, you will not technically have data. As a replacement for the Data Sheet, you
will turn in your papers where you did the work to get the electron configurations. You
do not have to have work for every element, but you must demonstrate that you
contributed your fair share to the group effort.
In the “Lab”:
Part One:
1. Write out the electron configurations and orbital filling diagrams for the following
elements—one set per group. Each person in the group needs to contribute.
Sodium
Magnesium
Aluminum
Silicon
Phosphorus
Sulfur
Chlorine
Argon
Potassium
Calcium
Scandium
Manganese
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
Yttrium
Technetium
Cadmium
Fluorine
Rubidium
2. Look for patterns in the electron configurations based on where the elements are
on the periodic table. Think in terms of total electrons, valence electrons, energy
levels, periods, sublevels, blocks, and groups/families.
3. Once you think you have noticed all the patterns you can, call me over to discuss
your conclusions.
Part Two:
1. Compare your electron configurations with the following reference material on
the reactions of the elements.
Na – Very easily loses one electron
Mg – Easily loses two electrons
Al – Loses three electrons with effort
Si – Can gain or lose four electrons
P – Gains three electrons with effort
S – Easily gains two electrons
Cl – Very easily gains one electron
Ar – Does not react, gain, or lose.
K – Very easily loses one electron
Ca – Easily loses two electrons
Ga – Loses three electrons with effort
Ge – Can gain or lose four electrons
As – Gains three electrons with effort
Se – Easily gains two electrons
Br – Easily gains one electron
Kr – Rarely reacts. Doesn’t gain or lose.
2. Write the electron configuration for each of the elements listed under Part Two
after they have undergone the reactions listed for them. For example, since
sodium (Na) normally has 11 electrons, it will have 10 electrons once it loses one.
You should then write the electron configuration for 10 electrons. For Si and Ge,
write both electron configurations.
3. Look for patterns in the electron configurations from before the reactions and
after the reactions.
4. Once you think you have noticed all the patterns you can, call me over to discuss
your conclusions.
Lab Report:
A) Purpose (5%)
B) Work for the electron configurations (30%)
C) Analysis Questions (50%)
1) Explain all of patterns discovered in Part 1 such that you explain how to
determine the electron configuration simply by looking at the periodic
table.
2) Explain the connection between the patterns discovered in Part 1 and the
historical reasons for grouping elements in families.
3) Explain the shape of the periodic table in terms of the patterns discovered
in Part 1.
4) Based on Part 2, what electron configurations are the most stable
configurations?
5) Explain the properties of the elements that have the stable configuration
discovered in Part 2 without needing to lose or gain electrons.
6) The most common reaction pattern for transition elements (d block) is
losing two electrons. What does this fact suggest about how these
elements lose electrons? A few sample electron configurations may be
useful to show what you are talking about.
D) Conclusion (15%)