Electron Configuration
Chemistry Lab #6
Name_______________________________ Date__________________ Period____
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In this lab you will be writing electron configurations for several elements from
all over the periodic table. These electron configurations will then be used to find
patterns in the periodic table and help you to group elements.
Pre-lab Questions
1) Distinguish between the following terms: energy level, sublevel, and orbital.
2) For each of the following pairs, indicate which is the higher energy orbital.
a. 1s or 3s
b. 4s or 3d
c. 5f or 6s
3) What is the maximum number of electrons possible for the following principal
energy levels?
a. 1st energy level
b. 2nd energy level
c. 3rd energy level
d. 4th energy level
4) What is a valence electron? Give the valence shell and number of valence
electrons for the element whose configuration is 1s22s22p63s23p64s23d104p3.
Procedure
1) Divide your list of elements among your group members. Each student should
take one horizontal row from the element list.
2) Read the analysis questions prior to beginning the rest of the lab. This will give
you an idea of how you will be sorting your elements.
3) Each group member should cut a sheet of loose-leaf paper into nine sections.
On each section write the electron configuration with orbital filling diagrams for
each of the elements in your row.
4) Use the analysis questions below to sort your elements into groups and answer
all questions completely.
Element List
He
H
Li
C
B
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
As
Se
Br
Kr
Rb
Sr
Te
I
Xe
Fe
Zn
Mo
Cd
U
Pr
Eu
Am
Analysis Questions
1) Find all of the elements that end with a single s electron.
a. What are the symbols of these elements in increasing atomic number
order?
b. Find these elements on the periodic table. What do you notice about
their location? Use your text to find the group number and the name of
this group of elements in Chapter 6.
c. How many valence electrons do these elements have? How does that
relate to the group number for these electrons?
2) 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. Find these elements on the periodic table. What do you notice about
their location? Use your text to find the group number and the name of
this group of elements in chapter 6.
c. How many valence electrons do these elements have? How does that
relate to the group number for these electrons?
d. Explain why Helium does not seem to fit in with the rest of the elements
in this group based on its state of matter.
3) Find all of the elements that have both two s electrons and six p electrons in
their outside energy level.
a. What are the symbols of these elements in increasing atomic number
order?
b. Look on your periodic table and find the elements on this list. Where are
they located? Give the group number and name.
c. How many valence electrons do these elements have? How does that
relate to the group number for these electrons?
d. Explain why Helium is found on the periodic table with these elements,
but does not end with the same electron pattern. What does Helium have
in common with these elements?
4) Find all of the elements that end with d electrons.
a. What are the symbols of these elements in increasing atomic number
order?
b. Look on your periodic table and find the elements on this list. Where are
they located? What is this group of elements called?
5) Find all of the elements that end with f electrons.
a. What are the symbols of these elements in increasing atomic number
order?
b. Look on your periodic table and find the elements on this list. Where are
they located? What are these elements called as a group?
6) Find all of the elements that have their valence electrons in the third principal
energy level.
a. What are the symbols of these elements in increasing atomic number
order?
b. Look on your periodic table and find the elements on this list. Where are
they located?
c. What is the valence shell for these electrons? How does that relate to
period on the periodic table?
7) Find all of the elements that have their valence electrons in the fourth energy
level.
a. What are the symbols of these elements in increasing atomic number
order?
b. Look on your periodic table and find the elements on this list. Where are
they located?
c. What is the valence shell for these electrons? How does that relate to
period on the periodic table?
8) A scrap of paper with the electron configuration of an element was picked up off
the floor. It was incomplete, but the last thing listed was 6s24f145d106p3. What is
this element’s complete electron configuration?