Lesson plan

Summary

In this lesson plan, students complete a worksheet answering questions regarding quantum numbers.

Grade Level

High school

Objectives

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.

Chemistry Topics

This lesson supports students’ understanding of

• Quantum numbers
•  Electron configuration

Time

Teacher Preparation: 20 minutes

Lesson: 50- 60 minutes

Materials.

• Student Handout

Safety

There are no special safety considerations for this activity.

Teacher Notes

• Students will need to be familiar with the concepts of quantum numbers before completing this activity.

Downloads

• Teacher Guide.doc
  
• Teacher Guide.pdf
  
• Student Activity.doc
  
• Student Activity.pdf
  

Submitted by:
Robert Bice
Chattooga High School
Summerville, Georgia

Thanks to:
Flinn Scientific

For the Student

Lesson

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, m_l=-1
d.   n=5, l=0, m_l=-2, m_s=-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:

a.    2s
b.    7s
c.    6p
d.   5d
e.    4f

6.   State all of the four quantum numbers, their names and explain what they represent.

7.   What are the m_l 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.

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