1. Electron Configuration, Electron Lab

2. Evaluation/ Assessment
Objective
Today I will be able to:
Calculate the electron configuration for elements on the periodic table
Construct a model of where electrons in the 1s orbital are located.
Evaluation/ Assessment
Informal assessment – student responses when reviewing electron configuration problems. Listening to group interactions on practice sheets and lab
Formal Assessment – collecting and analyzing responses to electron configuration worksheet 2 and the where is the electron lab?

3. Lesson Sequence Warm – Up
Elaborate: write electron configurations with a partner for questions 1-18
Evaluate: review the questions as a class (informal assessment)
Explain: electron configurations using 3d orbitals.
Elaborate: Students will complete on electron configuration WS with a partner
Evaluate: review the questions as a class (informal assessment)
Explain: abbreviated electron configurations
Elaborate: Students will add a column to the WS and repeat write the abbreviated configuration
Evaluate: Abbreviated configurations will be reviewed as a class (informal assessment)
Explore: Students will be sorted into groups and will complete the where is the 1s electron lab located
I will be assessing students progress during the lab as I monitor group discussions
Evaluate: Students will complete an electron configuration WS (assessment)
Explain: principles, rules and diagrams of electron configurations
Exit Ticket

4. Warm - Up How many electrons can each orbital hold?
f =
Write the electron configuration for the following elements
Helium
Nitrogen
Silicon

5. Objective Today I will be able to:
Calculate the electron configuration for elements on the periodic table
Construct a model of where electrons in the 1s orbital are located.

6. Homework
Electron Configuration Practice

7. Agenda Warm – Up Electron Configuration Practice
Electron Configuration Notes
Where’s the electron Lab
Exit Ticket

8. Electron Configuration Practice
Complete numbers 1-18

9. Electron Configuration

10. Electron Configuration1 2 3 4 5 6 7
p-block
s-block
d-block
n-1
f-block
n-2

11. Electron Configurations
We can write the electron configurations for each element (assuming the atom has a neutral charge) representing the location of the elements electrons in the energy levels

12. Examples Sodium (Na) Cobalt (Co) Has 11 electrons (when neutral)
Electron Configuration:
1s22s22p63s1
Cobalt (Co)
Has 27 electrons (when neutral)
Electron Configuration
1s22s22p63s23p64s23d7

13. Why does 4s come before 3d?
3d is of slightly higher energy than 4s, but 4s is further from the nucleus
It takes less energy for a 3d electron to form pairs then a 4s electron

14. Aufbau Diagram
Instead of using the periodic table as a road map, you can use the aufbau diagram to determine the order that the electrons occupy the different energy levels
Electrons fill the lowest energy orbitals first

15. Aufbau Diagram

16. Complete Electron Configuration Practice Worksheet 19 - 36

17. Abreviated Electron Configuration
Scientists are lazy ;)
We need a shorthand way to represent electron configuration
It would take a long time to write the configuration for elements with a lot of electrons
How do we do this?
Noble Gas Configuration

18. Noble Gas Configuration
The last column on the periodic table is referred to as the noble gases
To write in abbreviated configuration:
Find the last noble gas within the configuration
Write the symbol
Write the remaining configuration
Example
Ca - 1s2 2s2 2p6 3s2 3p6 4s2
Noble Gas Configuration = [Ar] 4s2

19. Noble Gas Configuration
Writing Noble Gas Configurations for ions is a little bit different
Must account for an electron being gained or lost
Chlorine Ion = Cl-1
[Ne] 3s2 3p6
Sodium Ion = Na+1
[He] 2s2 2p6

20. Electron Configuration Practice
Go back and write the Abbreviated (Noble Gas) configuration for the elements on the worksheet on the right hand margin

21. Where is the electron lab?

22. Electron Configuration Practice 2

23. More Electron Configuration Rules and Principles

24. Pauli Exclusion Principle
An orbital can hold a max of 2 e-
To occupy the same orbital, they must spin in opposite directions
If 2 e- occupy an orbital, they are said to be “paired”
If only 1 e- is present in an orbital, it is “unpaired”

25. Pauli Exclusion Principle

26. Hund’s Rule
e- occupy orbitals so that a max number of unpaired e- result
More stable arrangement

27. Orbital Diagram Shows the electrons in their sublevels
Represented with arrows

28. Orbital Diagram 1s 2s 2px 2py 2pz H ↑ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↑ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓He C ↑ ↓ ↑ ↓ ↑ ↑ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ Ne

29. Exit Ticket
Draw an orbital diagram representing the arrangement of the electrons in sulfer