1. Tuesday, December 9th, 2014 HW: Agenda Questions
Objective: We will be able to determine the electron configuration for an atom.
Standard: IOD 402
Catalyst: F. The number of ants at each site
G. The number of seed dishes placed at each site
H. The mass of the elaiosome of each seed
J. The type of seeds taken by the ants in each site
Classroom expectations:
Wear Kenwood ID.
Cell phones, music players, and headphones are put away.
Food is disposed of or put away.
Dressed appropriately.
Notebook is out and you are ready for today’s class.
Answer: C
***Table of Contents
12/9 Week 15 Catalyst
12/ Week 15 Agenda
12/ Week 15 Textbook Reading
12/ Notes: Electron Configuration

2. Tuesday, December 9th, 2014 HW: Agenda Questions
Objective: We will be able to determine the electron configuration for an atom.
Standard: IOD 303
Catalyst:
F. 5.0 N
G. 7.0 N
H. 9.0 N
J N
Classroom expectations:
Wear Kenwood ID.
Cell phones, music players, and headphones are put away.
Food is disposed of or put away.
Dressed appropriately.
Notebook is out and you are ready for today’s class.
Answer: A
***Table of Contents
12/9 Week 15 Catalyst
12/ Week 15 Agenda
12/ Week 15 Textbook Reading
12/ Notes: Electron Configuration

3. Announcements No tutoring today Tutoring will be Weds of this week
Quiz Thursday

4. Catalyst/Announcements Review POGIL Notes: Electron Configuration
Agenda
Catalyst/Announcements
Review POGIL
Notes: Electron Configuration

5. Electron Configuration Notes87

6. Electron Configuration Notes81

7. Electrons are always moving around the nucleus in energy levels.

8. Within these energy levels, there are specific regions or sublevels where electrons are more likely to be found.

9. Example:
Hydrogen (H):
1s1
# electrons
Energy level
sublevel

10. Energy level 1: 1 sublevel (s)
Energy level 2: 2 sublevels (s, p)
Energy level 3: 3 sublevels (s, p, d)
Energy level 4: 4 sublevels (s, p, d, f)

11. TAPE!!!

12. Orbital Diagrams

13. Aufbau principle
Electrons occupy the lowest energy first.

14. Suborbitals Each sublevel can hold a specific number of electrons.
s: holds 2 electrons, 1 pair with opposite spins
p: holds 6 electrons, 3 pairs with opposite spins
d: holds 10 electrons, 5 pairs with opposite spins
f: holds 14 electrons, 7 pairs with opposite spins

15. Rules for Electron Configuration
Electrons fill the lowest sublevel first.
Only one electron goes in an orbital at a time before doubling up.
Only 2 electrons can be in an orbital and they must have opposite spins.

16. S-block
p-block
d-block
f-block

17. Example
Element: Sulfur
Electron Configuration:
Orbital Diagram:

18. Whiteboard Practice Only write when you are completing a problem.
Hold up board ONLY when asked.
Keep marker capped when possible.

19. White board practice
Draw the orbital diagram for Nitrogen Draw the spdf configuration 1s22s22p3

20. White board practice
Draw the orbital diagram for Chlorine Write the spdf notation 1s22s22p63s23p5

21. White board 1s22s22p63s1 1s22s1 1s22s22p63s23p64s1 1s22s22p1
Write the electron (spdf) configuration of
Sodium
Lithium
Potassium
Boron
Aluminum
Gallium
1s22s22p63s1
1s22s1
1s22s22p63s23p64s1
1s22s22p1
1s22s22p63s23p1
1s22s22p63s23p64s23d104p1

22. Noble Gas notation
Electron configurations can be written in noble gas configuration
The noble gas of each row becomes a placeholder for the configurations that came before.
This is kind of like a checkpoint in a game you start your configuration from after each noble gas.

23. Practice Write the configuration of Argon 1s22s22p63s23p6
Now write the configuration of calcium
1s22s22p63s23p64s2
Now we can use the symbol [Ar] in brackets as a placeholder
[Ar]4s2

24. Noble gas configuration
You can only use noble gases for shorthand notation

25. White board [Kr]5s2 [He]2s2 [He]2p5 [Xe]6s1
Write short hand for the following
Strontium
Beryllium
Fluorine
Cesium
Radium
[Kr]5s2
[He]2s2
[He]2p5
[Xe]6s1

26. Whiteboard [He]2p2 [Ne]3p2 [Ar]4s2 [Ne]3s2
Write the noble gas configuration for the following
Carbon
Silicon Ca Mg
[He]2p2
[Ne]3p2
[Ar]4s2
[Ne]3s2

27. Exceptions to Aufbau Principle

28. Exceptions to the Aufbau Principle
(HONORS only)
Exceptions to the Aufbau Principle
d and f orbitals require LARGE amounts of energy
If we can’t fill these sublevels, then the next best thing is to be HALF full (one electron in each orbital in the sublevel)
There are many exceptions, but the most common ones are
Copper (ends in 4s13d10)
Silver (ends in 5s14d10)
Gold (ends in 6s14f145d10)
Chromium (ends in 4s13d5)
d4 and d9

29. Exceptions to the Aufbau Principle
(HONORS only)
Exceptions to the Aufbau Principle
OK, so this helps the d, but what about the poor s orbital that loses an electron?
Remember, half full is good… and when an s loses 1, it too becomes half full!
So… having the s half full and the d half full is usually lower in energy than having the s full and the d to have one empty orbital.

30. Practice
1.) Write the electron configuration for helium.

31. Practice
2.) Write the electron configuration for beryllium.

32. Practice
3.) Write the electron configuration for fluorine.

33. Practice
4.) Write the electron configuration for argon.

34. Practice
5.) Draw the aufbau diagram for boron.

35. Practice
6.) Draw the complateaufbau diagram for sodium.

36. Practice
7.) Write the electron configuration for oxygen.

37. Exit Ticket
8.) Draw the aufbau diagram AND write the electron cofiguration for calcium for titanium.