1. Electron Config… ya digg? October , 2.009 * 103
Objective:
SWBAT compare and contrast the Bohr model with the “Modern Atom”
SWBAT write electron configurations for elements
Catalyst:
Draw the Bohr model for Aluminum.
Draw the Bohr model for Boron.
What similarities do these two elements have?

2. Agenda Catalyst Review Modern Atom Electron Configuration!!
Practice, Practice, Practice
Exit Question

3. Do we really know where electrons hang out?
Key Point #1: The Heisenberg Uncertainty Principle tells us that there are limits to how much we can really know about electrons
Electrons are super tiny and they move very fast!
Can we really know where they are?

4. Heisenberg Uncertainty Principle
Book Definition: The Heisenberg Uncertainty Principle states that it is fundamentally impossible to know precisely both the velocity and the position of a particle at the same time.
Our Definition: The Heisenberg Uncertainty Principle tells us that it is impossible to know where an electron is in an atom
But! We can make a pretty good guess!

5. How? Schrödinger Equation
Key Point #2: The Schrödinger Equation predicts the location of an electron in an atom.
It tells us that electrons hang out in atomic orbitals.

6. Schrödinger Equation and Atomic Orbitals
Key Point #3: There are 4 atomic orbitals… s p d f

7. A Saying to Remember the Four Atomic Orbitals
some pirates die fiercely!

8. The s Orbital One s orbital in each energy level
The s orbital is shaped like a sphere

9. The p Orbital Three p orbitals in each energy level
(starting in the 2nd energy level!)
Shape looks like dumbells or bowties

10. p and s Orbitals Side by Side

11. Start in the 3rd energy level! Shape looks like eggs or flowers
The d orbital
Five d orbitals
Start in the 3rd energy level!
Shape looks like eggs or flowers

12. The f orbital
Seven f orbitals - start in 4th energy level

13. Quick Review Questions Answer in your notes
What are the four atomic orbitals?
Draw the s and p orbitals and describe the shape of each.
List 2 similarities between the Bohr model and the “Modern Atom.”
List 2 differences between the Bohr model and the “Modern Atom.”

14. Electron Configuration
Knowing where electrons are in an atom helps us determine how that atom will behave in a chemical reaction
We write electron configurations for atoms of each element to help us map out the electrons
Small number =Number of electrons
1s2
Letter=orbital
Large number= energy level

15. Electron Configuration
Review: Where do electrons hang out?
Now, we have to know how many electrons can fit into each atomic orbital
Think of each orbital as a type of house
Some houses are big, some small
Some houses have more bedrooms than others

16. Electron Configuration (First Energy Level)
Each orbital (bedroom) can hold two electrons
Review: How many orbitals are on the first energy level?
Good, just one! This is an s orbital!
One bedroom = up to 2 electrons
= electron

17. Electron Configuration (Second Energy Level)
Review: Which orbitals are on the second energy level?
Good! s and p
Review: How many p orbitals are there?
Good! Three p orbitals

18. Electron Configuration (Second Energy Level)
So….how many electrons could shack up on the second energy level?
Eight electrons!
= electron

19. Electron Configuration (Third energy level and beyond)
Review: How many d orbitals are there?
Good, five d orbitals!
So….how many electrons could shack up in d orbitals?
Good! Ten electrons!

20. Electron Configuration (Fourth Energy Level and Beyond)
Review: How many f orbitals are there?
Good! Seven f orbitals
So….how many electrons could shack up in f orbitals?
= electron
Good! Fourteen electrons!

21. Electron Configuration Review
Fill in the table below on your notes.
Orbital Type
(s, p, d, or f)
Energy Level
# of Orbitals
Maximum # of Electrons s p 5 14 1
1,2,3,4… 2 3 6
2,3,4… d 10
3,4… f 4… 7

22. Electron Configuration
Key Point #4:
Electron configuration: Shows how the electrons are distributed among the various atomic orbitals and energy levels.
The format consists of a series of numbers, letters, and superscripts as shown below:
1s2

23. Electron Configuration
1s2
Large number = energy level
Letter = atomic orbital
Superscript (small) number = number of electrons in atomic orbital

24. Figure it out yourself!! (15 mins)
Look at the table that has 1s, 2s, 2p on your notes sheet.
Here I have put a couple electron configurations. See if you can figure out how to do the last two.
Mg-1s22s22p63s2
Ne- 1s22s22p6
Si- 1s22s22p2
K- 1s22s22p63s23p64s1 S- B-

25. Electron Configuration
N – 1s2

26. Electron Configuration
N – 1s2 2s2

27. Electron Configuration
N – 1s2 2s2 2p3

28. Electron Configuration
N – 1s2 2s2 2p3
= 7 e-

29. Electron Configuration
Na – 1s2

30. Electron Configuration
Na – 1s2 2s2

31. Electron Configuration
Na – 1s2 2s2 2p6

32. Electron Configuration
Na – 1s2 2s2 2p6 3s1
= 11 e-

33. Electron Configuration
Be:
Ne:
Br:

34. Electron Configuration
Be: 1s22s2
Ne: 1s22s22p6
Br: 1s22s22p63s23p64s23d104p5

35. Exit Question
Write the electron configuration for the following 2 elements:
Manganese
Fluorine

36. More Electron Configuration and Valence Electrons October , 2.009 *103
Objective:
SWBAT write noble gas configurations for elements in the periodic table
SWBAT identify trends in valence electrons on the periodic table
Catalyst:
Write the electron configuration for iron and argon.

37. Agenda Catalyst Noble Gas Configuration Valence Electron
Project Work Time
Exit Question

38. Catalyst
Iron: 1s22s22p63s23p64s23d6
Argon: 1s22s22p63s23p6

39. Electron Configuration
Scientists are WAY too lazy to write all that mess!

40. Electron Configuration FIGURE IT OUT YOURSELF!!! (10 mins)
Hg – [Xe]6s24f145d10
S – [Ne]3s23p4
Sm – [Xe]6s24f5
Si-
Rb-

41. Electron Configuration
Key Point #1:
Noble Gas Configuration –Start writing your notation from the last noble gas BEFORE the atom you are going to.

42. Electron ConfigurationAg

43. Electron Configuration
Ag – [Kr]5s24d9

44. Electron ConfigurationCa

45. Electron Configuration
Ca – [Ar]4s2

46. Electron ConfigurationS

47. Electron Configuration
S – [Ne]3s23p4

48. Electron Configuration and Valence Electrons
Each group: Write long electron configurations for first four elements in given family.
Group 1: Alkali Metals (1)
Group 2: Alkaline Earth Metals (2)
Group 3: Boron’s group (13)
Group 4: Nitrogen’s group (15)
Group 5: Halogens (17)
Group 6: Noble Gases (18)

49. Electron Configuration and Valence Electrons
Each group: Write long electron configurations for first four elements in given family.
Group 1: Alkali Metals (1)
Group 2: Alkaline Earth Metals (2)
Group 3: Boron’s group (13)
Group 4: Carbon’s group (14)
Group 5: Nitrogen’s group (15)
Group 6: Oxygen’s group (16)
Group 7: Halogens (17)
Group 8: Noble Gases (18)

50. Electron Configuration and Valence Electrons
What trends do you see? How many valence electrons are there in each group?
Group 1: Alkali Metals (1)
Group 2: Alkaline Earth Metals (2)
Group 3: Boron’s group (13)
Group 4: Nitrogen’s group (15)
Group 5: Halogens (17)
Group 6: Noble Gases (18)

51. Electron Configuration and Valence Electrons
What trends do you see? How many valence electrons are there in each group?
Group 1: Alkali Metals (1)
Group 2: Alkaline Earth Metals (2)
Group 3: Boron’s group (13)
Group 4: Carbon’s group (14)
Group 5: Nitrogen’s group (15)
Group 6: Oxygen’s group (16)
Group 7: Halogens (17)
Group 8: Noble Gases (18)

52. Valence Electron Trends on the Periodic Table

53. Project Work TIME!!! Write electron configurations for your family
Draw Bohr models for your family

54. Exit Question Write the noble gas configuration for Bromine Copper
Sodium