NAME:
PERIOD:
UNDERSTANDING ELECTRON CONFIGURATION
PRELAB
Complete energy level diagrams for the following elements (given the atomic number):
Group member 1:
1, 5, 9, 13, 17, 21, 25, 29, 33, 37, 58, 62
Group member 2:
2, 6, 10, 14, 18, 22, 26, 30, 34, 38, 59, 63
Group member 3:
3, 7, 11, 15, 19, 23, 27, 31, 35, 39, 60, 64
Group member 4:
4, 8, 12, 16, 20, 24, 28, 32, 36, 40, 61, 65
PURPOSE
1. Use energy level diagrams to determine the electron configuration of the 12 elements.
2. Relate the chemical behavior of elements to their electron configurations.
3. Relate the electron configurations of elements to the periodic table.
MATERIALS
Energy level diagrams
Periodic table
Blank periodic table
Colored pencils
PROCEDURE
1.
You will be a member of a group for this experiment. Each person in the group will be assigned 12
elements.
2. For each assigned element, complete the energy diagram following the Aufbau principle, Hund’s rule and
Pauli Exclusion Principle. The electron configuration and the quantum set (n, l, ml, and ms) should also
be completed.
3. Work with your group to complete the following analysis questions.
ANALYSIS QUESTIONS
1.
Distinguish between the following terms: energy level, sublevel, and orbital.
NAME:
PERIOD:
2.
Define the following rules or principles:
a. Aufbau –
b. Hund’s rule-
c.
Pauli exclusion principle -
3. In each of the following pairs, indicate which is the higher energy orbital.
a. 1s or 3s
b. 4s of 3d
c.
5f or 6s
4. What is the maximum number of electrons possible for the following energy levels?
a. 1st _____________
b. 2nd ____________
c.
3rd ____________
d. 4th____________
5. Find all of the elements that end with a single s electron (either 1s, 2s, 3s, 4s, etc.)
a. What are the symbols of these elements in increasing atomic number order?
b. Use the periodic table to determine the most common charge when these elements become ions.
c.
Explain the connection between the charge and the electron configuration of these elements?
That is, what will happen to the valence electrons of these atoms.
d. Where are these elements located on the periodic table (group number)? Shade the entire
column red.
6. Find all of the elements that end with two s electrons.
a. What are the symbols of these elements in increasing atomic number order?
b. Use the periodic table to determine the most common charge when these elements become ions.
NAME:
PERIOD:
c.
Explain the connection between the charge and the electron configuration of these elements?
d. Where are these elements located on the periodic table (group number)? Shade the entire
column orange.
e. Explain why helium does not seem to fit in the rest of the elements in this group.
7. Find all of the electrons that have two s electrons and six p electrons in their outermost energy level.
a. What are the symbols of these elements in increasing atomic number order?
b. Where are these elements located on the periodic table (group number)? Shade the entire
column blue.
c.
Explain why helium is found with these elements on the periodic table even though it does not
have the same electron configuration.
8. Find all the elements that end with electrons in a d orbital.
a. What are the symbols of these elements in increasing atomic number order?
b. What do you notice about the possible charges on these elements?
c.
Shade the entire central block of the periodic table (from 21-30 39-48, 57, 72-80, and 89, 104112) yellow.
9. Find all of the elements that end with f electrons.
a. What are the symbols of these elements in increasing atomic number order?
b. Shade the two rows that are removed from the table (58-71 and 90-103) violet.
10. Find all of the elements that have their outside electrons in the third energy level.
a. What are the symbols of these elements in increasing atomic number order?
NAME:
PERIOD:
b. Mark a small 3 on each of these elements on your periodic table. Where are they located?
11. Find all of the elements that have their outside electrons in the fourth energy level.
a. What are the symbols of these elements in increasing atomic number order?
b. Mark a small 4 on each of these elements on your periodic table. Where are they located (which
rows)?
12. A scrap of paper with the electron configuration of an element was picked up off the floor. The last thing
listed was 6s24f45d10 6p4. What is this element’s complete electron configuration? Identify the element.
13. Look for a column on the periodic table that includes elements that have a ( -1) charge when they
become ions. Shade this column light blue.
a. What do the elements in this column have in common? Discuss in terms of valence electrons
and electron configuration.
14. Look for a column on the periodic table that includes elements that have a (-2) charge when they
become ions. Shade this column green.
a. What do the elements in this column have in common? Discuss in terms of valence electrons
and electron configuration.
15. How many valence electrons does aluminum have?
a. What will an aluminum atom do to become stable?
b. What is the charge on aluminum when it becomes stable?
c.
Which noble gas electron configuration will aluminum achieve after becoming stable?
16. How many valence electrons does phosphorus have?
a. What will a phosphorus atom do to become stable?
NAME:
PERIOD:
b. What is the charge on phosphorus when it becomes stable?
c.
Which noble gas electron configuration will phosphorus achieve after becoming stable?
17. Where are the following regions on the periodic table? Label the regions
a. S block
b. P block
c. D block
d. F block
SUMMARY
All of the questions in this lab have been designed to make you think about the connections among electron
configuration, periodic table, and chemical behavior. Write a clear essay summarizing these connections.
Discuss e configuration, location on the periodic table (group and period number), chemical behavior, ion
formation (most likely charge) and stability through loss or gain of electrons. Your summary should be typed. (15
points)