1. The Mole
-just as a _____ is always ____, a _______ is always _______,
a ______ is always ____, and a _____ is always ____, a
_____ is always ____________________________, or
__________, and just like it is sometimes easier to buy things
by the _______ or by the _____, it is sometimes easier to
consider numbers of _________ of _______ by the _____
I. Converting Moles to Particles and Particles to Moles

2. The Mole
I. Converting Moles to Particles and Particles to Moles
How many molecules in 4.5 moles of sucrose?
How many moles in 1.75 x 1025 molecules of water?

3. The Mole
II. Molar Mass
-the _______ of ______ are established ________ to
the mass of one __________ atom, which has ____
_________ and ____ __________
-____-________ of the mass of a __________ atom,
or about the mass of a _______ or a ________, is
called an _______ _____ _____, or _____
-the ______ _____ is the _____ of one _____ of an
element, and is numerically equal to the ________
_____, but with units of ______ per _____, so the
_______ _____ of a Carbon-12 atom is ___ ____,
and the ______ _____ of Carbon-12 is ___ ______
per _____

4. The Mole
II. Molar Mass
A. Converting Mass to Moles and Moles to Mass
What is the mass of moles of Vanadium?
How many moles of Tantalum are in 75 grams
of Tantalum ?

5. The Mole
II. Molar Mass
A. Converting Mass to Atoms and Atoms to Mass
How many atoms are there in g Uranium?
What is the mass, in grams, of x 1024 atoms of Niobium?

6. The Mole
II. Molar Mass
A. Converting Mass to Molecules and Molecules to Mass
How many molecules are there in 456 g Silicon dioxide?
What is the mass, in grams, of 1.75 x 1026 molecules of cyclohexane?

7. The Mole
III. Empirical and Molecular Formulas
A. Calculating Percent Composition
What is the percent composition of Sodium, Sulfur, and Oxygen in
Sodium Sulfate?

8. The Mole
III. Empirical and Molecular Formulas
A. Calculating Percent Composition
What is the percent composition of Carbon, Hydrogen, and Oxygen in
fructose, C6H12O6?

9. The Mole
III. Empirical and Molecular Formulas
B. Determining Empirical Formula from Percent Composition
What are the empirical and molecular formulas for Ibuprofen if the molar
mass is 206 g/mole and the percent composition of 75.7% C, 8.80% H,
and 15.5% O?

10. The Mole
III. Empirical and Molecular Formulas
B. Determining Empirical Formula from Percent Composition
What are the empirical and molecular formulas for Glycerol if the molar
mass is g/mole and the percent composition of 39.12% C, 8.75% H,
and 52.12% O?

11. The Mole
III. Empirical and Molecular Formulas
B. Determining Empirical Formula from Percent Composition
What are the empirical and molecular formulas for Naphthalene if the
molar mass is 128 g/mole and the percent composition of 93.7% C and
6.3% H?

12. The Mole
III. Empirical and Molecular Formulas
B. Determining Empirical Formula from Percent Composition
What are the empirical and molecular formulas for a Lead chloride
compound if the molar mass of the compound is g/mole and the
percent composition is 59.37% Pb?

13. The Mole
III. Empirical and Molecular Formulas
A. Calculating Percent Composition
-lab
1. Hypothesis
2. Prediction
3. Gathering Data

14. The Mole
III. Empirical and Molecular Formulas
A. Calculating Percent Composition
-lab
3. Gathering Data
-procedure
4. Analyzing Data
5. Drawing Conclusions

15. -hydrates are __________ that have a specific number
The Mole
IV. Hydrates
-hydrates are __________ that have a specific number
of ______ molecules attached to them
A. Naming Hydrates
Formula
Name

16. The Mole
IV. Hydrates
B. Calculating the Formula for a Hydrate
What is empirical formula and for a hydrated compound of Copper(II)
sulfate, if 2.50 grams of blue CuSO4·nH2O is heated in a crucible until
1.59 grams of white anhydrous CuSO4 remains ?