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. 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.

10. 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?

11. 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

12. What about Magnesium and Oxygen?

13. Oxidation #’s Backwards
Give me the oxidation state (charge) for each atom (polyatomic ion) in the compound for the following chemical formulas:
Zn(OH)2
BeSO4
Mg3P2
MgBr2
KCl
NH4OH

14. 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)

15. 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?

16. More Polyatomics...

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

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

19. 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

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

21. Show me the formula hexaboron silicide chlorine dioxide
hydrogen iodide
iodine pentafluoride
dinitrogen monoxide