1. In groups discuss:
How would you define a compound? Use some key vocabulary terms from the first chemistry test to help you.
If H2O and H2O2 are both compounds, how are they different?
How do atoms combine to form compounds?
How do ionic bonds and covalent bonds differ? How are they the same?
Think back to our global warming project. What compounds (greenhouse gases) have we already studied? Explain how the electrons move in order for each of the greenhouse gases to form. Label each greenhouse gas as an ionic or covalent bond.

2. Adapted from http://sciencespot.net/
Bonding Basics
8th Grade Science
Adapted from

3. Section A: Complete the chart using a periodic table to help you.

4. NEGATIVE POSITIVE ION CATION ANION
Answer these questions:
An atom that gains one or more electrons will have a ____________________ charge.
An atom that loses one or more electrons will have a ____________________ charge.
An atom that gains or loses one or more electrons is called an ____________.
A positive ion is called a ______________ and a negative ion is called an _______________.
NEGATIVE
POSITIVE
ION
CATION
ANION
“An-Eye-On”
“Cat-Eye-On”

5. ELECTRONS COMPLETE METAL NONMETAL
What is an ionic bond?
Atoms will transfer one or more ________________ to another to form the bond.
Each atom is left with a ________________ outer shell.
An ionic bond forms between a ___________ ion with a positive charge and a ________________ ion with a negative charge.
Example B1: Sodium + Chlorine Example B2: Magnesium + Iodine
ELECTRONS
COMPLETE
METAL
NONMETAL

6. Example B3: Potassium + Iodine Example B4: Sodium + Oxygen
Example B5: Calcium + Chlorine Example B6: Aluminum + Chlorine

7. SHARE COMPLETE NONMETAL
What is a covalent bond?
Atoms ___________ one or more electrons with each other to form the bond.
Each atom is left with a ________________ outer shell.
A covalent bond forms between two _________________.
Example C1: Hydrogen + Hydrogen Example C2: 2 Hydrogen + Oxygen
SHARE
COMPLETE
NONMETAL

8. Example C3: Chlorine + Chlorine Example C4: Oxygen + Oxygen
Example C5: Carbon + 2 Oxygen Example C6: Carbon + 4 Hydrogen

9. Review Vocab… What is an oxidation number? How is it determined?
What is a subscript? What does it tell you about the atoms in the compound?
What is a chemical formula?

10. Oxidation Numbers
Same thing as typical charge an atom will have once it has lost or gained electrons
Shortcut to writing chemical formulas:
1. Ca I
2. Ca+2 I1-
3. Ca I1-
Ca1 I2
CaI2

11. Bond With A Classmate Purple = Cations ; Pink = Anions
Find a classmate to “bond” with and together decide on the correct chemical formula (use the oxidation numbers to help you!)
You will have to decide how many of each ion you need to make a STABLE IONIC BOND.
Record all bonds on your Date Book (data table)
Look at the box on your paper for helpful hints
You will have 5 minutes to make as many bonds as possible.

12. Oxidation #’s Backwards
Give me the oxidation state (charge) for each atom in the compound for the following chemical formulas:No Periodic Tables Allowed!
BaCl2
CaF2
Mg3N2
MgBr2
KCl
K2O

13. What’s in a Name?
Naming
Compounds

14. Compound Naming- 3 minutes
Separate the cards into 2 groups:
1 group = (18 cards) with exactly 2 elements
1 group = (6 cards) with more than 2 elements
Keep the group of 6 separated

15. Card Sorting – 5 minutes
How do you tell the difference between ionic and covalent compounds?
Identify 6 cards that have only two elements that have formed a covalent bond (look in your group of 18)
3. Similar to #1 how are ionic different than covalent?
Once I have approved those 6, set them back in the bag

16. Discuss (only) in groups
What are transition metals?
How are they different from metalloids?
Find 6 compounds that start with a transition metal

17. Ionic group #1 Transition elements: 5 minutes
Answer #1-4
Copy the chemical formulas exactly as they appear on your cards.
Copy the compound name exactly as it appears on the card (THE ROMAN NUMERAL TOO!!!!)
What pattern in the names of the compounds do see for the cation and for the anion?
We will fill out #6 together 

18. Ionic group #1 Transition Metals
6. Give me the oxidation state (charge) for each atom in the compound for the following chemical formulas:No Periodic Tables Allowed!
V2O5
Cu3As
FeBr2
Fe2O3
PbO
VF4

19. Ionic group #1
7. How are the names of compounds containing transition metals related to the oxidation state of the cation?

20. Transition Metal + Nonmetal Patterns
Cation = (+)
Roman numeral = cation charge
Metal name is unchanged
Anion= (-)
Change ending to -ide

21. Ionic Group # 2 Polyatomic Ions
Find the 6 cards that contain more than two elements and fill in the blanks for #8
We will do #9 together
Red = cation
Black = anion

22. Polyatomic Ions
Find the 2 compounds that contain a polyatomic ion for the cation and for the anion

23. Polyatomic + Polyatomic
Cation
Only NH4+
Anion
Name = polyatomic ion chart

24. Metal + Polyatomic
Find the 3 compounds that contain a metal ion for the cation and a polyatomic for the anion

25. Name = Name as it appears on periodic table Anion
Metal + Polyatomic
Cation
Metal
Name = Name as it appears on periodic table
Anion
Name = polyatomic ion chart

26. Polyatomic + Nonmetal
Find the 1 compound that contain a polyatomic ion for the cation and a nonmetal for the anion

27. Cation Only NH4+ Anion Name = nonmetal Change ending to -ide
Polyatomic + Nonmetal
Cation
Only NH4+
Anion
Name = nonmetal
Change ending to -ide

28. Transition Metal + Polyatomic
Do you have any cards that have a transition metal for the cation and a polyatomic ion for the anion?

29. Transition Metal + Polyatomic
Cation
Roman numeral = cation charge
Metal name is unchanged
Anion
Name = polyatomic ion chart

30. What are the patterns in naming the cation and anion?
Metal and Nonmetal
Find the 6 cards that have just one metal (not transition) and one non metal
What are the patterns in naming the cation and anion?

31. Anion Name = nonmetal Change ending to -ide Cation Metal
Metal and Nonmetal
Cation
Metal
Name = Name as it appears on periodic table
Anion
Name = nonmetal
Change ending to -ide

32. Naming Ionic Compounds
For #1-20
Write a P to the left of the # if the compound contains a polyatomic ion
Write a T to the left of the # if the compound contains a transition metal
Write MNM if the compound is a metal and a nonmetal

33. Name that Compound…
NaCl
NaCO3
NaOH
NH4OH
Fe2(SO4)3

34. Show me the formula Ammonium Chloride Potassium Nitrate
Calcium hydroxide
Sodium Oxide
Copper (II) Sulfate

35. Naming Ionic Compounds
Metal and nonmetal: Name the metal and change the nonmetal to –ide
Transition metals and nonmetals: Use roman numerals to represent the charge and name the nonmetal using –ide
Polyatomic Ions : If positive are more like metals and come first, if negative are more like nonmetals and come second. They have their own names and oxidation numbers (see chart on back)

36. More Polyatomics...

37. Polyatomic ions Kinda annoying
But super cool when you react them together and light them on FIRE!!!
COOL VIDEO OF ammonium dichromate and mercury thiocyanide
We’ll watch it if you can write the correct chemical formula for each!

38. Naming Ionic Bonds Practice
What is the chemical formula for the compound that results when Magnesium and Chlorine combine? Use the lewis dot structures and the criss cross method to show how you get the same formula.
How do you name this compound?

39. Compound Naming
How do you tell the difference between ionic and covalent compounds?
Identify 6 cards that have only two elements that have formed a covalent bond
Once I have approved those, fill out #1-5 on your naming notes sheet

40. Naming Covalent Compounds Guidelines for Inorganic Compounds1
Mono- 2
Di- 3
Tri- 4
Tetra- 5
Penta- 6
Hexa- 7
Hepta- 8
Octa- 9
Nona- 10
Deca-
In covalent compounds, the least electronegative element comes
first and its name is unchanged.
2. The more electronegative element comes second and takes on the
–ide ending like in ionic bonds
Subscripts are represented by
Greek prefixes
Example: H2O –dihydrogen monoxide

41. Name that Compound Can you use the inorganic guidelines for all of these?
4. CH4

42. Show me the formula hexaboron monosilicide chlorine dioxide
hydrogen monoiodide
iodine pentafluoride
dinitrogen monoxide