In this lesson plan, students complete a worksheet answering questions regarding quantum numbers.
AP Chemistry Curriculum Framework
- Big Idea 1: The chemical elements are fundamental building materials of
matter, and all matter can be understood in terms of arrangements of atoms.
These atoms retain their identity in chemical reactions.
- 1.12 The student is able to explain why a given set of data suggests, or does not suggest, the need to refine the atomic model from a classical shell model with the quantum mechanical model.
- 1.13 Given information about a particular model of the atom, the student is able to determine if the model is consistent with specified evidence.
- 1.15 The student can justify the selection of a particular type of spectroscopy to measure properties associated with vibrational or electronic motions of molecules.
By the end of this lesson, students should be able to
- determine the number of electrons occupying various electron orbitals.
- list the four quantum numbers and what they represent.
This lesson supports students’ understanding of
- Quantum numbers
- Electron configuration
Teacher Preparation: 20 minutes
Lesson: 50- 60 minutes
- Student Handout
There are no special safety considerations for this activity.
- Students will need to be familiar with the concepts of quantum numbers before completing this activity.
For the Student
1. Determine the total number of e- that can occupy the following:
a. One s orbital
b. Three p orbitals
c. Five d orbitals
d. Seven f orbitals
2. Calculate the e- given the following:
a. n=3, l=0
b. n=3, l=1
c. n=3, l=2, ml=-1
d. n=5, l=0, ml=-2, ms=-1/2
3. How many e- can exist in all of the n=5 orbitals?
4. How many possible orbitals are there for n=4?
5. Figure out the n and l values for the following orbitals:
6. State all of the four quantum numbers, their names and explain what they represent.
7. What are the ml values for a d orbital?
8. What is the lowest value of n for which a d subshell can occur?
9. A single subshell orbital can contain how many e-?
10. Fluorine commonly has an oxidation state of -1. Draw the orbital state of both the neutral and the most common oxidation state.