1. To Do… OWL Lectures Discussion
Chapter 11 (Part 2) due Wednesday, April 11
Chapter 12 (Part 1) due Friday, April 13
Lectures
Continue reading Chapter 12
Discussion
Chapter 12 text homework

2. 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

3. Atomic Radius (Size)
Decreases across a row (period) – outer electrons in the same energy level
Hydrogen 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.

4. Figure 11. 36 Relative atomic sizes for selected atoms
Figure Relative atomic sizes for selected atoms. Note that atomic size increases down a group and decreases across a period.
Figure p265

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

6. p263

7. 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.

8. Ionization Energy
Increases across a row (period) – outer electrons in the same energy level
Hydrogen 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.

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

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

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

12. Chemical Bond
Force that holds groups of two or more atoms together and makes them function as a unit.
Atoms will bond if the molecule is more stable than the two separated atoms (lower energy state).

13. Ionic Bonding

14. Na → Na+ + e–

15. Cl + e– → Cl–

16. Forming H2

17. Covalent Bonding

18. Clicker Question
Imagine the bond formed in the carbon monoxide molecule (C-O). Which atom would you expect to have a greater attraction for the electrons in the bond?
a) carbon
b) oxygen
c) They have the same attraction (both have n=2 as highest energy level with an electron).
d) I do not know.

19. Polar Covalent Bonding

20. Figure 12.4 The three possible types of bonds.
Figure 12-4 p271

21. Clicker Question
How do lithium, fluorine, and cesium compare with regard to attraction for an electron in a shared bond?
a) Li>Cs>F
b) F>Cs>Li
c) F>Li>Cs
d) Li>Cs>F
e) Cs>F>Li

22. Electronegativity

23. Table 12-1 p271

24. From the Periodic Table…
Electron configurations
Charges for ions in compounds (and thus formulas for compounds)
Trends
Atomic radius
Ionization energy
Electronegativity
Polarity of Bonds