1. CHEM-R REVIEW
CHAPTERS 9,11,10,12

2. CHAPTER 9: Writing and Naming Chemical Formulas

3. IONIC compounds consist of a _________ and a __________
COVALENT compounds (Molecules) consist of 2 ________________

4. Which of the following compounds contains the Iron III cation?
a. FeO
b. FePO4
c. FeF2
d. Fe3N2

5. -ide ending comes from the periodic table (there are exceptions)
-ate and -ite are your polyatomic ions
Molecular compounds are named using prefixes

6. NAMING ACIDS -ate polyatomic ion results in an -ic acid
-ite polyatomic ion results in -ous acid
monoatomic ions results in Hydro-- acid

7. TIME TO GET UP AND MOVE!

8. Chapter 11: Chemical Reactions

9. Reactions that have energy as a reactant are called _______________ reactions:
They require energy for the reaction to occur
Reactions that have energy as a product are called _______________ reactions
Energy happens as a result of the reaction

10. Writing and Balancing Chemical Reactions
*** DONT forget charges when writing, and to add coefficients ONLY when balancing***

11. RULES for BALANCING COMBUSTION REACTIONS:
1. Determine the # of Hydrogens in the hydrocarbon molecule
ODD- Place the coefficient “4” in front of the molecule
EVEN- Place the coefficient “2” in front of the molecule
2. Balance both sides of the equations (Left to Right) with the Carbon atoms
3. Balance (Left to Right) the Hydrogen atoms
4. Balance the Oxygen atoms (Right to Left)
5. Reduce the coefficients (If necessary)

12. What are the 5 types of Chemical reactions?

13. TIME TO GET UP AND MOVE!

14. Chapter 10: Chemical Quantities (The Mole)

15. 1 mole of anything is equal to _____________ of that thing
This number is better known as ______________ number

16. The mole is at the center of your chemical
calculations

17. WHAT IS 1 Mole equal to???
1 Mole = 6.02 x 1023 (atoms, formula units, or molecules)
1 Mole = molar mass (of an element or compound)
1 Mole = 22.4 L (of a gas at STP)

18. Percent Composition
Percent composition tell us what percent, by mass, each element is in a given compound
% by mass of element =
mass of element
molar mass of compound
× 100
K = 40.3%
Cr = 26.8%
+ O = 32.9%
100%

19. Empirical Formula
A compound that gives the lowest whole-number ratio of the atoms or moles of the elements in a compound
For example:
Hydrogen peroxide has a molecular formula H2O2 but an empirical formula HO
Carbon dioxide (CO2) has the same molecular and empirical formula

20. Calculating Empirical Formula (from percent composition)
1. Percent to mass
2. Mass to moles
3. Divide by small
4. Multiple ‘til whole (sometimes)
1. A compound was found to have a percent composition as follows: 47.0 % potassium, 14.5 % carbon, and 38.5 % oxygen. What is its empirical formula?

21. So how would you determine which chemical you are dealing with?
Molecular Formula: a formula giving the actual number of atoms of each of the elements present in one molecule
Methanol (formaldehyde), ethanoic acid (acetic acid), and glucose have the same empirical formula
CH2O
So how would you determine which chemical you are dealing with?

22. TIME TO GET UP AND MOVE!

23. Chapter 12: Stoichiometry “stoicheion” = Greek for element “metron” = measurement

24. Stoichiometry: a process of relating the quantities of reactants and products in a chemical reaction to one another
Mole Ratio: Conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction
** All reaction stoichiometry calculations begin with a balanced chemical equation**

25. Steps to follow when solving stoichiometry calculations:
1. Write/Balance the chemical equation
2. Determine the mole ratio
3. Determine the given and wanted quantity
4. If necessary, convert the given quantity to moles
5. Use the proper mole ratio to get rid of the given moles and determine the wanted moles
6. If necessary, convert the wanted quantity (in moles) to grams, representative particles, or liters

26. ____KClO3 ____KCl + ____O2
What mass of KClO3 do you need to produce moles of O2?

27. Limiting Reactants

28. Ideal stoichiometry problems assume that the given quantity is completely used up and therefore we can predict how much product is formed
In real stoichiometry calculations, you are given the starting amount of both reactants. One of the reactants is used up before the other and therefore limits the reaction
Once the limiting reactant is used up, the reaction will stop

29. TIME TO GET UP AND MOVE!