1. Creating a Positive Learning Environment for Everyone
Be respectful of your classmates
Save conversation for clicker portions of lecture
Put cell phones in “airplane” mode
Turn off tablets
Close laptops

2. Joke of the Day
Q: Why did the turkey cross the road before Thanksgiving? A: He was trying to give people the impression that he was a chicken. (Even though it wasn’t a chemistry joke, I slapped my neon that one it was so funny.)

3. Announcements
Lon-capa HW 6 – Type 1 due Monday (11/27) and Type 2 due Wednesday (11/29) by 7pm
“Lab 5: Modern Atomic Theory” write-up due tomorrow in discussion (and text homework)
Exam 3 is Thursday December 7

4. Valence Electrons Highest or outermost energy level electrons
Where the chemistry happens! 
Look at principal quantum level n
Look at group or family
Sulfur: 1s22s22p63s23p4
Valence electrons are in n = 3 level
Valence electrons = = 6 electrons

5. Number of Valence Electrons in…?P Br
1s22s22p4
[Ar]5s24d105p3 2 5 7 6 5

6. Clicker #1
How many unpaired electrons are in a neutral ground state atom of phosphorus? A) 1 B) 3 C) 5 D) 7 E) 15

7. Atomic Radius (Size) Increases down a group Hydrogen
Francium
Orbitals are getting larger and electrons fill further and further from the nucleus at higher energy levels

8. Atomic Radius (Size)
Decreases across a row (period) – outer electrons in the same energy level
Lithium Fluorine
DECREASES!
More protons in each element as you move across the row. More protons will create a stronger positive force, thus attracting the electrons more strongly, pulling them in and shrinking the size.

9. Clicker #2
Which of the following elements has the largest atomic radius?
A) Ca
B) Al
C) N
D) Sr
E) F

10. General Trend (Atomic Size/Radius)

11. Ionization Energy Decreases down a group Hydrogen
Francium
Orbitals are getting larger and electrons fill further and further from the nucleus at higher energy levels. Electrons are not as tightly bound by the nucleus at higher energy levels so it takes less energy to remove an outer electron.

12. Ionization Energy
Increases across a row (period) – outer electrons in the same energy level
Lithium Fluorine
INCREASES!
More protons in each element as you move across the row. More protons will create a stronger positive force, thus attracting the electrons more strongly and pulling them in closer to the nucleus, requiring MORE energy to remove an outer electron.

13. Clicker #3
Which of the following elements has the largest ionization energy?
A) P
B) Al
C) Cl
D) Ba
E) K

14. General Trend (Ionization Energy)

15. Clicker #4 What are the electron configurations of Na+ and F-? Na+ F-
1s22s22p63s1
1s22s22p5 b)
1s22s22p63s2
1s22s22p4 c)
1s22s22p6

16. Overall goal: Atomic Structure Chemical Bonding 3D Molecular Structure
Molecular Properties

17. Overall goal: Atomic Structure Chemical Bonding 3D Molecular Structure
Molecular Properties

18. Bond (Intramolecular)
Force that holds groups of two or more atoms together and makes them function as a unit.
Bond is more stable than the two separated atoms (lower energy state).

19. Ionic Bonding

20. Ionic Bonding

21. Covalent Bonding

22. Electronegativity

23. Covalent Bonding

24. Polar Covalent Bonding

25. Polar Covalent Bonding

26. Clicker #5 Rank the following bonds from least polar to most polar:
Si-Cl P-Cl Mg-Cl S-Cl
A) S-Cl, P-Cl, Mg-Cl, Si-Cl
B) P-Cl, S-Cl, Si-Cl, Mg-Cl
C) Mg-Cl, Si-Cl, P-Cl, S-Cl
D) Mg-Cl, S-Cl, P-Cl, Si-Cl
E) S-Cl, P-Cl, Si-Cl, Mg-Cl