Name ___________________________________
Period _______
Date __________
Electron Configuration- Orbital Notation Notes
What we learned from our rules from the Quantum Numbers:
EVERY orbital can hold up to ______ electrons.
The s orbital (there is ____) can hold up to ________ electrons.
The p orbitals (there are _____) can hold up to ________ electrons.
The d orbitals (there are ____) can hold up to ________ electrons.
The f orbitals (there are ____) can hold up to __________ electrons.

Hund’s rule states that electrons must be placed successively in each _______________ of a orbital
first before additional electrons can occupy the same orbitals. (see p. 105-106 in your text)

The __________________ Exclusion principle states that when 2 electrons must occupy the same
orbital, they will have ____________________ spins. One will be symbolized by an _____________
arrow and the other by a _____________ arrow in a box or line. Such an example looks like this:

The ____________ (pronounced OFF-ba) principle tells how the electrons fill the orbitals by
increasing energy. Draw this diagram below. (Figure 3.4 on page 110 in your text) Be sure to add the
arrows!
Name ___________________________________
Period _______
Date __________
Orbital Notation Lab
Materials
cups
(represent the sublevel or orbital)
s orbitals have 1 cup
p orbitals have 3 cups
d orbitals have 5 cups
f orbitals have 7 cups
bingo chips (2 different colors for the clockwise and counterclockwise spins)
Procedure:
You will rotate to each station and complete TWO configurations at each station. Electron configuration for
neon looks like this: 1s2 2 s2 2 p6. Take special notice to write the energy levels in large numbers, the orbital in
lowercase letters, and the number of electrons in superscript above the letter. Orbital notation will be drawn
using the lines and arrows.
1. Find your labeled cups and place in the proper filling order designated by the Aufbau diagram.
2. As you visit each station, fill in the chart for each element by writing in the electron configuration for
that element.
3. Put the correct number of electrons (symbolized by the chips) into the orbitals of the
subshells (cups) that have been set up. One color will represent the clockwise spin and the
other color will represent the counterclockwise spin.
4. Using the model you have just created, draw the correct orbital notation for each element in the chart.
5. Count the number of electrons in the highest energy level cups and add the “valence electrons
number” to your chart.
Name ___________________________________
Period _______
Station #
Element
1. Li
1. C
2. Mg
2. Al
3. P
3. Ar
4. Ti
4. Ga
5. Fe
5. Rb
6. Sr
6. Zr
7. Sn
Electron Configuration
Orbital Notation
Date __________
# Valence
Electrons
Name ___________________________________
Period _______
7. I
8. Xe
8. Ba
9. Eu
9. Dy
10. W
10. Pb
Analysis- (answer these on the back of this lab sheet)
1. Which of the above elements had their final electron in the “s” sublevel?
2. Which element(s) had their orbitals completely filled?
3. Which element(s) had their orbitals completely half filled?
4. Which element(s) had their orbitals partially filled?
Date __________