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# Quantum Numbers Mark as Favorite (24 Favorites)

LESSON PLAN in Quantum Numbers, Electron Configuration, Electrons, Orbitals . Last updated March 25, 2020.

### Summary

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

High School

### NGSS Alignment

This simulation will help prepare your students to meet the performance expectations in the following standards:

• HS-PS1-1: Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.

### 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: 5 minutes

Lesson: 30 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.

### 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. Determine how many e can have the following quantum numbers:

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:

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 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 orbital diagrams, with quantum numbers l and ml labeled, of both the neutral atom and the most common oxidation state.