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# Quantum Numbers (13 Favorites)

LESSON PLAN in Quantum Numbers, Electron Configuration, Electrons, Orbitals . Last updated October 8, 2019.

### 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.

### 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

*=-2, m*

_{l}*=-1/2*

_{s}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.