Job Name:
LESSON
9
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/306076t
Billions and Billions
Avogadro’s Number
Name
Date
Period
C L A S S WO R K
Purpose
To find the relationship between mass and number of atoms.
Analysis
1. The table on the next page shows the mass of different numbers of atoms of zinc,
aluminum, and iron. Complete the table.
2. What is scientific notation?
3. Why do you think scientists use scientific notation?
4. What are two ways of writing the smallest number in the table? What does it represent?
5. What are two ways of writing the largest number in the table? What does it represent?
6. Which has the most mass, 1 trillion atoms of zinc, 100 trillion atoms of iron, or
500 trillion atoms of aluminum? Explain how you can tell.
7. How many zinc atoms are there in 65.4 g?
8. Some of the numbers in scientific notation have a negative exponent, and some have a
positive exponent. Explain the difference between these two types of numbers.
9. What do 65.4 g of zinc, 27.0 g of aluminum, and 55.8 g of iron have in common?
10. What name do chemists give to a collection of 602 sextillion objects?
Living By Chemistry Teaching and Classroom Masters: Units 4–6
© 2010 Key Curriculum Press
Unit 4 Toxins
Lesson 9 • Worksheet
27
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Unit 4 Toxins
Lesson 9 • Worksheet
100,000,000,000,000
100 trillion
1,204
sextillion
602
sextillion
1,000,000,000
1,000,000,000,000,000,000
1 billion
602
sextillion
1
quintillion
500,000,000,000,000
1,000,000
1 million
500 trillion
602,000,000,000,000,000,000,000
602
sextillion
100,000
1 hundred
thousand
1,000,000,000,000
100
1 hundred
1 trillion
Number of atoms
Amount
6.02 1023
1.0 1018
111.6 g
0.0000000093 g
0.000000000000093 g
27.0 g
0.000000022 g
0.000000000000000045 g
65.4 g
0.000000000000000011 g
0.000000000000000000011 g
1.0 102
1.0 105
Mass (g)
Number of atoms in
scientific notation
5.58 101 g
9.3 109 g
2.70 101 g
4.5 106 g
4.5 1017 g
6.54 101 g
1.1 1010 g
1.1 1017 g
1.1 1020 g
Mass in scientific
notation
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iron Fe(s)
aluminum
Al(s)
zinc Zn(s)
Substance
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Living By Chemistry Teaching and Classroom Masters: Units 4–6
© 2010 Key Curriculum Press
Job Name:
LESSON
10
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What’s in a Mole?
Name
Date
Molar Mass
Period
LAB
Part 1: Molar Mass
1. Use a periodic table to complete the second column in the table. You
will complete the last column in Part 2.
Chemical formula
Molar mass
g/mol
Mole of what?
Equivalent to:
Cu(s)
63.55 g
Cu atoms
50 ft of 20-gauge copper wire
O2 (g)
32.00 g
O2 molecules
22.4 L oxygen gas at STP
Ni(s)
Ni atoms
Al(s)
Al atoms
H2O(l)
H2O molecules
He(g)
He atoms
NaCl(s)
NaCl units
Hg(l)
Hg atoms
Fe(s)
Fe atoms
C12H22O11(s)
sugar molecules
22.4 L helium gas at STP
14.7 mL mercury
0.75 lb sugar
2. How many copper atoms are in 63.55 g of copper?
3. Copper has a larger molar mass than aluminum. Explain what this means.
4. Which contains more moles, 1.0 g Al(s) or 1.0 g Hg(l)? Explain your thinking.
5. Explain how you determined the molar mass of sugar. Show your work.
Living By Chemistry Teaching and Classroom Masters: Units 4–6
© 2010 Key Curriculum Press
Unit 4 Toxins
Lesson 10 • Worksheet
29