The Mole Unit
Name: ________________
Acc Chemistry 14-15
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Lab – Bead Mania
Lesson 1 - The Mole and Molar Mass
Practice – The Mole and Molar Mass
Lesson 2 – Significant Digits
Practice – Significant Digits
Lesson 3 - Converting between particles,
moles and grams
____G. Practice - Converting between particles,
moles and grams
____H. Lab - Chalk Talk
____I. Lab – How Many Molecules of Water are in
Lake Erie
____J. Quiz 1
____A.
____B.
____C.
____D.
____E.
____F.
____K. Lesson 4 - Percent Composition
____L. Practice - Percent composition
____M. Lab - How Sweet You Are
____N. Quiz 2 - Percent Composition
____O. Lesson 5 - Empirical Formulas
____P. Practice - Empirical Formulas
____Q. Lab - The Strange Case of Moles Airline
____R. Lesson 6 - Molecular Formulas
____S. Practice - Molecular formulas
____T. Quiz 3 - Empirical vs. Molecular Formulas
____U. The Mole Unit Review
____V. The Mole Unit Test
A. Lab – Bead Mania
B. Lesson 1 - The Mole and Molar Mass
C. Practice – The Mole and Molar Mass (pg 309)
1. Define mole. ___________________________________________________________________________
_______________________________________________________________________________________
2. How is a mole similar to a dozen? ___________________________________________________________
_______________________________________________________________________________________
3. The mole represents an enormous number called Avogadro’s number.
Write this number. ______________________________________________________________________
a. Explain why Avogadro’s number is so huge. ____________________________________________
____________________________________________________________________________________
b. The smallest piece that makes up a substance is dependent on the type of substance.
This is called a representative particle.
i. For elements the representative particle is an ______________, for compounds the
representative particle is a ______________________.
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4. 1 mole of any substance contains ______________________________ particles.
5. Explain why chemists use the mole. _________________________________________________________
_______________________________________________________________________________________
6. Which has a larger mass a dozen limes or a dozen eggs? Justify your
answer._____________________________________________________
___________________________________________________________
___________________________________________________________
7. Explain what is meant by molar mass. ___________________________
__________________________________________________________
Determine the molar mass for each of the following compounds. Show your work. No work = no credit
8. CaCl2
10. C2H5OH
9. (NH4)3PO4
11. C12H22O11 (sucrose)
Mixed Review
Answer the following questions:
12. Which are there more of on the periodic table: Metals, nonmetals or metalloids? __________________
13. Which type of element loses electrons to create positive ions? _________________________________
14. Name the shapes that can produce polar molecules. _________________________________________
15. Which of the types of substance (elements, compounds or mixtures) can be separated by physical
means? __________________________________
16. Which element will have the smaller atomic radius: Arsenic or Phosphorus? _____________________
D. Lesson 2 – Significant Digits
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E. Practice – Significant Digits
Determine the number of significant digits in each number.
1) 0.012
_____
5) 0.0102
_____
9) 5.56 x 10-4
_____
2) 100
_____
6) 12,000
_____
10) 0.00010
_____
3) 120.
_____
7) 12,000.
_____
11) 98.06501
_____
4) 0.2070
_____
8) 15.0
_____
12) 1.0 x 10-9
_____
Round each number to the specified significant digits.
13) 790,001.01  1 sig. dig.
_______________________
14) 665.001  2 sig. digs.
_______________________
15) 15,984,123  4 sig. digs
_______________________
16) 789.65 3 sig. digs.
_______________________
Atomic Structure Unit Review
Fill in the chart.
#
#
Element
M/NM/ML?
protons neutrons
Noble gas notation
Sodium – 23
Phosphorus – 31
Antimony - 75
F. Lesson 3 - Converting between Particles, Moles and Grams
G. Practice - Converting between Particles, Moles and Grams
1. What is the relationship between the following
a. 1 mole Li = _____________________ atoms Li
b. 1 mole Li = _____________________ grams Li
c. 1 mole NaCl = _____________________ grams NaCl
d. 1 mole NaCl = _____________________ molecules NaCl
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Complete the following conversions. You MUST show your dimensional analysis. No work = no credit
Mole - Particles
2. Fill in the dimensional analysis conversion factor for converting from representative particles to moles
1.23 x 1023 atoms Ca
= 0.204 mols Ca
3. Fill in the dimensional analysis conversion factor for converting from moles to representative particles
1.25 mols H2O
= 7.53 x 1023 molecules H2O
4. Determine the number of atoms in 2.50 mol Zn.
5. How many moles contain 5.75 x 1024 atoms Al?
Mole – Grams
6. Determine the mass in grams of 3.57 mol Ag.
7. Determine the number of moles in each of 23.7 g S.
8. What is the mass of 0.0535 moles of (NH4)3PO4?
9. How many moles are in 45.0 g CaCl2
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Mole – Particles – Grams
10. Fill in the dimensional analysis conversion factor for converting from representative particles to grams
1.23 x 1023 atoms Ca
= 8.18 grams Ca
11. Fill in the dimensional analysis conversion factor for converting from moles to representative particles
= 7.52 x 1023 molecules H2O
22.5 grams H2O
12. How many atoms are in 76.63 g Li?
13. What is the mass in grams of 8.62 x 1024 atoms Mn?
Reactions Unit Review
Balance the following reactions
14. _____ PH3 
_____ P4 + _____ H2
15. _____ H2 +
_____ O2 
_____ H2O
16. _____ N2 +
_____ H2 
_____ NH3
17. _____ Al + _____ Pb(NO3)2  _____ Al(NO3)3 + _____ Pb
18. _____ KOH + _____ H3PO4  _____ K3PO4 + _____ H2O
19. _____ Cu + _____ AgNO3  _____ Cu(NO3)2 + _____ Ag
20. _____ Na + _____ Cl2  _____ NaCl
H. Lab - Chalk Talk
I. Lab – How Many Molecules of Water are in Lake Erie?
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J. Quiz 1

Perform conversion between all units including mass, moles, and particles (atoms and molecules).
K. Lesson 4 - Percent Composition
L. Practice - Percent Composition
1. Define percent composition. _______________________________________________________________
_______________________________________________________________________________________
Complete the following math calculations to determine percent composition.
No work = no credit
2. Determine the percent composition of calcium chloride, CaCl2.
3. Calculate the percent composition of sodium sulfate, Na2SO4.
4. Which has the larger percent by mass of sulfur, H2SO3 or H2S2O8?
5. Which has the higher percent by mass of hydrogen - phosphoric acid (H3PO4) or hydrochloric acid (HCl)?
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Mixed Review
6. When completing a single replacement reaction, metals always replace _____________________.
7. The products of a combustion reaction are _____________________________________________.
8. How does an ion differ from an atom? ____________________________________________________
9. Ionic compounds are made up of ________________________________________________________.
10. For a bond to be polar, the electronegativity difference must be higher than _____.
M. Lab - How Sweet You Are
N. Quiz 2 - Percent Composition


Calculate the percent composition for each element in a molecule.
Analyze compounds to compare the percent composition of a single element.
O. Lesson 5 - Empirical Formulas
P. Practice - Empirical Formulas
1. What is an empirical formula? ______________________________________________________________
_______________________________________________________________________________________
Complete the math calculations to figure out the empirical formulas. No work = no credit.
2. The pain reliever morphine contains 17.900 g C, 1.680 g H, 4.255 g O and 1.228 g N. Determine the
empirical formula.
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3. A blue solid is found to contain 36.84% nitrogen and 63.16% oxygen. What is the empirical formula for
this solid?
4. A solid compound decomposes when heated in the laboratory. Given the following data, determine the
empirical formula for the initial compound.
Reaction Equation
AxBy(s) ---------> xA(s) + yB(g)
Item
Mass
Solid Product
4.20 g
Gas Product
0.59 g
Molar mass
element A is 84.0 g/mol
element B is 23.7 g/mol
Properties of Elements Review:
Give the special name to the following groups on the periodic table.
Group 1 __________________________________________________
Group 2 __________________________________________________
Group 17 __________________________________________________
Group 18 __________________________________________________
The groups (columns) on the periodic table are also called ____________________________________.
The rows on the periodic table are called _________________________________________.
Q. Lab - Strange Case of Moles Airline
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R. Lesson 6 - Molecular Formulas
S. Practice - Molecular Formulas
1. What is the difference between a molecular formula and an empirical formula? _______________________
_______________________________________________________________________________________
2. Can an empirical formula also be a molecular formula? (YES or NO)
Complete the math calculations to figure out the molecular formulas. No work = no credit.
3. Analysis of a chemical used in photography indicates an empirical formula of C3H3O. The molar mass is
found to be 110.0 g/mol. Determine the molecular formula.
4. A compound was found to contain 49.98 g carbon and 10.47 g hydrogen. The molar mass of the compound
is 58.12 g/mol. What is the molecular formula?
5. Azobenzene is an important intermediate in the manufacture of dyes. It contains 79.1% carbon, 5.55%
hydrogen, and 15.4% nitrogen. It has a molar mass of 182 g/mol. What is the molecular formula?
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Bonding Review
Write the correct compound formulas. Identify them as covalent of ionic.
6. Methane _________________________________ (IONIC or COVALENT)
7. Zinc hydroxide_________________________________ (IONIC or COVALENT)
8. Copper (I) sulfide _________________________________ (IONIC or COVALENT)
9. Oxygen difluoride _________________________________ (IONIC or COVALENT)
T. Quiz 3: Empirical & Molecular Formulas
 Calculate the empirical formulas from percent composition or from mass composition.
 Calculate molecular formulas when given empirical formulas and molecular mass.
* You may need to calculate the empirical formula.
U. The Mole Unit Review
V. The Mole Unit Test
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