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# Quantum Numbers (9 Favorites)

LESSON PLAN in Quantum Numbers, Electron Configuration. Last updated April 25, 2019.

### Summary

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

### Grade Level

High school

### AP Chemistry Curriculum Framework

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.__Big Idea 1:__**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.

### 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.