1. Launch: 2/8
 Grab your binder and immediately take a seat!
 Place launch paper and yesterday’s practice questions
on your desk.
 Friday’s Quiz Data:
90%!
 Today’s Objectives: I can draw a Lewis structure.

2. Launch 2/8
1. Look around the classroom and make a list of
all the new things you can see.

3. Launch 2/8
2. Which of the following is true about the Kinetic
Molecular Theory?
a) It can be used to measure the speed of molecules.
b) It states that gas molecules more slower at high
temperatures.
c) It states that the motion of a gas particle is fast
and random
d) All of the above.

4. Launch 2/8
3. Pressure is created by
a) the diffusion of two or more gases.
b) the random motion of molecules and their
collisions with a surface.
c) the phase change that occurs at 0°C.
d) the force of a solid exerted on the interior of a gas.

5. Announcements
 Quiz scores handed out at the end of class
 New items in the classroom
 Positive consequences
 Negative consequences
 Word wall
 Data wall
 Shout Outs!
 Change in schedule!
 Surprise benchmark

6. February Calendar
Quiz!
Today Benchmark Quiz!
Exam!

7. Opening
 Today’s Objective: I can classify a chemical bond as
either ionic, covalent, or metallic.

8. Chemical Bonding Review:
Part II
Mr. Heffner
2//09

9. What are Lewis structures?
 Lewis structures are…
 pictures of covalent molecules
• • • •
Covalent Bond
F- F
2 electrons = dash
• •
• •
Lewis
Structure
• • • •

10. Example #1
Draw the Lewis symbol for carbon.
 Step 1: Place element’s symbol in center
C

11. Example #1
Draw the Lewis symbol for carbon.
 Step 2: # of valence electrons?

12. Example #1
Draw the Lewis symbol for carbon.
 Step 2: # of valence electrons?
“The Trick”: Group #
Drop the 1!
group # = 14
# valence electrons = 4

13. Example #1
Draw the Lewis symbol for carbon.
 Step 3: Place electrons around symbol
 One on each of the 4 sides
 No doubling up!
• •
C
•
•

14. What is a Lewis structure?
 There is a 3-step process for creating Lewis
structures:
1. Draw Lewis symbol for each atom and count dots
2. Arrange atoms so they all have a full octet
 If more than 2 atoms, place first atom in center
3. Count dots and convert shared pairs to bonds

15. Example
Draw the Lewis structure for Cl2
 Step 1: Draw Lewis symbol for each atom and count
• • • •
dots
Cl Cl
•
• •
• •
•
• • 14 dots • •

16. Example
Draw the Lewis structure for Cl2
 Step 2: Arrange atoms so they have a full octet
• • • •
Cl Cl
• •
• •
• •
• =• 8• •
8 =

17. Example
Draw the Lewis symbol for Cl2
 Step 3: Count dots and convert shared pairs to dashes
• • • •
Covalent Bond
Cl-Cl
2 electrons = dash
• •
• •
• •
• •
• • dots
14

18. Example
Draw the Lewis structure for NH3
 Step 1: Draw Lewis symbol for each atom and count
• •
dots
•
•
•
N HHH
•
•
• 8 dots

19. Example
Draw the Lewis structure for NH3
 Step 2: Arrange atoms so they have a full octet
 If more than two atoms, place first atom in center
• •
HN H
• •
H is an exception to
• • • •
H
the octet rule
2= 8=

20. Example
Draw the Lewis symbol for Cl2
 Step 3: Count dots and convert shared pairs to
dashes
• •
H-N-H
• •
• •
•
- •
H 8 dots

21. Example
Draw the Lewis structure for CH4

22. Practice Questions
 Review worksheet

23. Exit Slip
1. In covalent bonding,
a. valence electrons are exchanged.
b. only metals interact with other metals.
c. valence electrons are shared
d. atoms become less stable due to the octet rule.

24. Exit Slip
2. Covalent bonds form between which two types of
elements?
a. metals and metals
b. metals and nonmetals
c. nonmetals and nonmetals
d. none of the above

25. Exit Slip
3. Ionic bonds form between which two types of
elements?
a. alkali and alkaline earth metals
b. halogens and other halogens
c. metals and nonmetals
d. nonmetals and other nonmetals

26. Exit Slip
4. What type of compound is H2SO4?
a. metallic
b. covalent
c. ionic
d. none of the above

27. Exit Slip
5. Which of the following is an example of an ionic
compound?
a. AlCl3
b. CCl4
c. O2
d. Zn2+

28. Homework
 Finish the review worksheet
 Study hard for Tuesday’s exam!