1. Do Now After the bell (2 min) When the bell rings In your seat:
Answer the following: A dad and his son were riding their bikes and crashed. Two ambulances came and took them to different hospitals. The man’s son was in the operating room and the doctor said, “I can’t operate on you. You’re my son.” How is that possible?
In your seat:
With pen/pencil
With Notebook
With Handout
Packet from last class on your desk
Silent and ready for Do Now
Still needs Do Now
The doctor is his mom!

2. Agenda  Do Now (5 min) Remediation Topic: Props of H2O Quiz (10 min)
Warm Up (10 min)
Notes: Covalent Bonding (30 min)
Independent Practice (20 min)
Exit Slip (5 min)
Closeout (2 min) 
Next Class

3. Properties of Water: You do
Which two properties of water are demonstrated in the diagram to the left?
Give a simple definition of cohesion.

4. Properties of Water: You do
If water’s temperatures rose and fell at the same rate as the temperatures on land, marine life would be unable to exist. Which property of water is responsible for keeping the temperature of water relatively consistent?
Polarity
Universal Solvent
Adhesion
Specific Heat
3. A person fills a drinking glass with water until the water is bulging slightly over the glass rim. The property of water that prevents the water from spilling is _________________.

5. Forming and Naming covalent Compounds
Objectives:
Predict the formation of covalent compounds
Using the nomenclature rules, name or predict formulas of compounds when given a covalent compound

6. Guiding Question
How is a covalent compound different than an ionic compound?

7. Warm Up Which of the following is the formula for Copper (I) Selenide?
Cu2Se
CuSe2
Se2Cu
SeCu2
What is the name of the compound PbO?
Lead Oxide
Lead (II) Oxide
Lead (IV) Oxide
Lead (III) Oxide

8. Warm Up
When forming MgF2, magnesium and fluorine form ions that have the same electron configuration as what element? F Al Ne Ar
What is the name of Li2O
A student was given the formula BeF2 and named it Beryllium (II) Fluoride. Why is this answer wrong?

9. Covalent Bonds
Definition: A bond between two non-metals; electrons are shared
SO2

10. Identify each compound as ionic or covalent
SO2
Al3O2
K2S O2
C6H12O6

11. Properties of Covalent Compounds
Low Melting & Boiling Points
Soft and brittle
Does not dissolve in Water
Does not conduct electricity
If we could zoom in SUPER close

12. Writing Covalent Compounds
Follow this format
N2O5
Include on a right hand page in your notebook (Notes)
Number of atoms of O
The least electronegative, listed first
The most electronegative, listed second
Number of atoms of N

13. 2 Type of covalent compounds
Polar
Non-polar
Definition: Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms.
Definition: Nonpolar covalent bonds are a type of chemical bond where two atoms equally share a pair of electrons with each other. 

14. Polar Molecules Molecules are polar bc….
Electrons are not shared equally
One element is more electronegative
Not symmetrical (asymmetrical)
Partial charges
Examples:
H__ (ex. HCl, HF, HI)
H2O
NH3

15. Non-Polar Molecules Molecules are non-polar bc…
Electrons are shared equally
Diatomic molecules
Symmetrical
No permanent charges (because it is being equally pulled in all directions)
Examples:
X2 (ex. H2, Cl2, I2)
CO2
C_4 (ex. CH4, CCl4, CI4)

16. C.F.U. H2 HF
NH3
H2O
NO2
Identify each of the following compounds as Polar or Non-Polar

17. The Octet Rule Covalent compounds still follow the Octet Rule
They will settle for sharing electrons
How many electrons do each of the following elements want to share? P Br N C Ne
The Octet Rule

18. Making a Covalent Compound
Example: H + Cl
3 Steps:
Draw the Lewis Structure for each element
Match the sides with single electrons
Draw a line to connect the two single electrons H Cl
Formula: HCl

19. Making a Covalent Compound
You do:
F + F
C + F
Making a Covalent Compound
3 Steps:
Draw the Lewis Structure for each element
Match the sides with single electrons
Draw a line to connect the two single electrons F2
CF4

20. Types of bonds Single: one electron from each atom is shared (2 Total)
Double: two electrons from each atom are shared (4 Total)
Triple: three electrons from each atom are shared (6 Total)

21. C.F.U. 1. 3.
Look at each diagram and determine how many electrons are shared in each compound 4. 2.

22. Rules for naming covalent compounds:
The first element in the compound is named as it appears on the periodic table
The second element is named with the root word + the suffix “ide”
Prefixes are used to denote the numbers of each atom present
exception: the prefix “mono” is never used with the first element

23. List of Prefixes Example 1: CO Example 2: CO2 Number of atoms: Prefix:
mono 2 di 3
tri 4
tetra 5
penta 6
hexa 7
hepta 8
octa 9
nona 10
deca
List of Prefixes
Example 1: CO
Example 2: CO2

24. Table Group Problems: Number of atoms: Prefix: 1 mono 2 di 3 tri 4
tetra 5
penta 6
hexa 7
hepta 8
octa 9
nona 10
deca
N2O
NO2
Dinitrogen Trioxide
NO4
Phosphorous Pentachloride
SO2

25. Table Group Answers: Dinitrogen Oxide Nitrogen dioxide N2O3
Dinitrogen Tetraoxide
PCl5
Sulfur Dioxide

26. Activity: Independent Practice
What?
How?
C – None
H – Raise hand
A – Writing electron configurations
M – None
P – Recoding answers on left page, head up, reading and thinking through all questions, discussing with group
15 minutes  Discuss for 5 minutes  Verify & Review

27. Exit Slip How? What? (5 min)
C – No talking
H – Raise hand
A – Taking exit slip
M – In seat
P – Completing exit slip without notes and turning in
If you finish early, summarize what you learned at the bottom of your notes OR answer today’s guiding question

28. Forgetting to stretch is a bear.
Closing
What are 3 key takeaways from today and yesterday?
Complete the 8 Stretch questions